Riar: A.P Chemistry
UNIT 1: REVIEW OF CHEMISTRY BASICS ?
Day 1
Learning Objectives:
 Understand Units of measurements, uncertainty of measurements, significant figures and
calculations, dimensional analysis.
 Define and evaluate the uncertainty, accuracy, and precision of measurements
 Perform mathematical computations using methods of numerical problem solving.
NJCCC standards addressed:
5.2.2.A.1 Sort and describe objects based on the materials of which they are made and their
physical properties.
5.2.8.A.1 Explain that all matter is made of atoms, and give examples of common elements
5.2.8.A.2 Analyze and explain the implications of the statement “all substances are composed of
elements.”
5.2.6.B.1 Compare the properties of reactants with the properties of the products when two or
more substances are combined and reaction
5.2.8.B.1 Explain, using an understanding of the concept of chemical change, why the mass of
reactants and the mass of products
5.2.12.B.3 Balance chemical equations by applying the law of conservation of mass.
Motivation:
Development:
Students will review chapters 1, 2 & 3
Students will take turns in solving problems on the board as the class corrects their summer
assignment
Summary/Assessment:
Homework:
Review chapter 1,2 &3 notes
Check answers to the summer assignment
Riar: A.P Chemistry
UNIT 1: REVIEW OF CHEMISTRY BASICS?( chapter 1,2 &3)
Day2
Learning Objectives:
Students will be able to:
 Find the Atomic mass of a metal by converting a weighed amount of a unknown Metal to
an Oxide
 Determining formula of a compound, using stoichiometric calculations
 Apply the law of Dulong and Petite to determine the Atomic weight of a Unknown Metal
NJCCC standards addressed:
5.2.2.A.1 Sort and describe objects based on the materials of which they are made and their
physical properties.
5.2.8.A.1 Explain that all matter is made of atoms, and give examples of common elements
5.2.8.A.2 Analyze and explain the implications of the statement “all substances are composed of
elements.”
5.2.6.B.1 Compare the properties of reactants with the properties of the products when two or
more substances are combined and reaction
5.2.8.B.1 Explain, using an understanding of the concept of chemical change, why the mass of
reactants and the mass of products
5.2.12.B.3 Balance chemical equations by applying the law of conservation of mass.
Motivation:
ASK STUDENTS HOW CAN THE ATOMIC MASS OF AN UNKNOWN ELEMENT BE
DETERMINED
Development:
Students will perform the procedure of the Atomic Weight of a Metal lab
Students will use their collect data to calculate the ratio of the mass of oxygen that combined
with 1 gram of the metal and predict a possible empirical formula of the metal Oxide and the
identity of the metal
Students will apply the law of Dulong and Petite to determine the empirical formula of the metal
Oxide and the identity of the metal
Summary/Assessment:
Compare Class results
Discuss the importance of the law of Dulong and Petite in determing the atomic weight of some
metallic elements
Homework:
Lab report for Atomic Weight of a Metal lab due
Riar: A.P Chemistry
UNIT 1: REVIEW OF CHEMISTRY BASICS?( chapter 1,2 &3)
Day3
Learning Objectives:
Students will be able to:
 Find the Atomic mass of a metal by converting a weighed amount of a unknown Metal to
an Oxide
 Determining formula of a compound, using stoichiometric calculations
 Apply the law of Dulong and Petite to determine the Atomic weight of a Unknown Metal
NJCCC standards addressed:
5.2.2.A.1 Sort and describe objects based on the materials of which they are made and their
physical properties.
5.2.8.A.1 Explain that all matter is made of atoms, and give examples of common elements
5.2.8.A.2 Analyze and explain the implications of the statement “all substances are composed of
elements.”
5.2.6.B.1 Compare the properties of reactants with the properties of the products when two or
more substances are combined and reaction
5.2.8.B.1 Explain, using an understanding of the concept of chemical change, why the mass of
reactants and the mass of products
5.2.12.B.3 Balance chemical equations by applying the law of conservation of mass.
Motivation:
ASK STUDENTS HOW CAN THE ATOMIC MASS OF AN UNKNOWN ELEMENT BE
DETERMINED
Development:
Students will perform the procedure of the Atomic Weight of a Metal lab
Students will use their collect data to calculate the ratio of the mass of oxygen that combined
with 1 gram of the metal and predict a possible empirical formula of the metal Oxide and the
identity of the metal
Students will apply the law of Dulong and Petite to determine the empirical formula of the metal
Oxide and the identity of the metal
Summary/Assessment:
Compare Class results
Discuss the importance of the law of Dulong and Petite in determing the atomic weight of some
metallic elements
Homework:
Lab report for Atomic Weight of a Metal lab due
Riar: A.P Chemistry
UNIT 1: REVIEW OF CHEMISTRY BASICS (Chapter 1, 2 &3)
Day4
Learning Objectives:
Students will be able to:
 Write and name formulas of ionic compounds.
 Write and name formulas of ionic compounds using ions with more than one oxidation #
 Apply the rules for naming and writing the formulas of acids
 Write and name formulas of Binary Molecular Compound.
NJCCC standards addressed:
5.2.2.A.1 Sort and describe objects based on the materials of which they are made and their
physical properties.
5.2.8.A.1 Explain that all matter is made of atoms, and give examples of common elements
5.2.8.A.2 Analyze and explain the implications of the statement “all substances are composed of
elements.”
5.2.6.B.1 Compare the properties of reactants with the properties of the products when two or
more substances are combined and reaction
5.2.8.B.1 Explain, using an understanding of the concept of chemical change, why the mass of
reactants and the mass of products
5.2.12.B.3 Balance chemical equations by applying the law of conservation of mass.
Motivation:
Development:
Students will review chapters 1, 2 & 3
Students will take turns in solving problems on the board as the class corrects their summer
assignment
Summary/Assessment:
Homework
Review chapter 1,2 &3
Homework worksheets Chapter 1,2,3
Riar: A.P Chemistry
UNIT 1: REVIEW OF CHEMISTRY BASICS( Chapter 1,2 &3)
Day5
Learning Objectives:
Students will be able to:
 Find the percent composition of a compound
 Determining formula of a compound, using stoichiometric calculations,
 Find the amounts of reactants and products
 Perform calculations involving limiting reactants.
NJCCC standards addressed:
55.2.2.A.1 Sort and describe objects based on the materials of which they are made and their
physical properties.
5.2.8.A.1 Explain that all matter is made of atoms, and give examples of common elements
5.2.8.A.2 Analyze and explain the implications of the statement “all substances are composed of
elements.”
5.2.6.B.1 Compare the properties of reactants with the properties of the products when two or
more substances are combined and reaction
5.2.8.B.1 Explain, using an understanding of the concept of chemical change, why the mass of
reactants and the mass of products
5.2.12.B.3 Balance chemical equations by applying the law of conservation of mass.
Motivation:
Development:
Students will review chapters 1, 2 & 3
Students will take turns in solving problems on the board as the class corrects their summer
assignment
Summary/Assessment:
Chapter 1, 2 &3 Test
Homework
Review for the Test
Riar: A.P Chemistry
UNIT 1: REVIEW OF CHEMISTRY BASICS( Chapter 1,2 &3)
Day6
Learning Objectives:
Students will be able to:
 Find the percent composition of a compound
 Determining formula of a compound, using stoichiometric calculations,
 Find the amounts of reactants and products
 Perform calculations involving limiting reactants.
NJCCC standards addressed:
55.2.2.A.1 Sort and describe objects based on the materials of which they are made and their
physical properties.
5.2.8.A.1 Explain that all matter is made of atoms, and give examples of common elements
5.2.8.A.2 Analyze and explain the implications of the statement “all substances are composed of
elements.”
5.2.6.B.1 Compare the properties of reactants with the properties of the products when two or
more substances are combined and reaction
5.2.8.B.1 Explain, using an understanding of the concept of chemical change, why the mass of
reactants and the mass of products
5.2.12.B.3 Balance chemical equations by applying the law of conservation of mass.
Motivation:
Development:
Students will review chapters 1, 2 & 3
Students will take turns in solving problems on the board as the class corrects their summer
assignment
Summary/Assessment:
Chapter 1, 2 &3 Test
Homework
Review for the Test
Riar: A.P Chemistry
UNIT 2: Solutions and net ionic reactions ( chapter 4 Part I)
Day1
Learning Objectives:
Students will be able to:
 Demonstrate knowledge of solution Stoichiometry including
strong, weak and non electrolytes.
 Calculate the Molarity of unknown solutions and ions in the solution
 know the different parts of a solution, how they can influence a solution’s properties
 Calculate the concentration of a solution.
 Describe how to make a solution of known concentration
 Describe how to make a solution of a known concentration by diluting a stock solution
NJCCC standards addressed:
5.2.12.A.5 Describe the process by which solutes dissolve in solvents.
5.2.2.A.1 Sort and describe objects based on the materials of which they are made and their physical
properties.
5.2.8.A.1 Explain that all matter is made of atoms, and give examples of common elements
5.2.8.A.2 Analyze and explain the implications of the statement “all substances are composed of
elements.”
5.2.6.B.1 Compare the properties of reactants with the properties of the products when two or more
substances are combined and reaction
5.2.8.B.1 Explain, using an understanding of the concept of chemical change, why the mass of reactants
and the mass of products
5.2.12.B.3 Balance chemical equations by applying the law of conservation of mass.
Motivation:
Demonstrations – Conductivity of soluble Ionic compds
Electrolytes/ Non Electrolytes
Weak and strong Electrolytes
Development:
Solution Power point lecture
Summary/Assessment:
Homework
Section 1 – problems 5,7,11,15,17,19abef,20ace,21,22,23,24,82ad,93,95
Riar: A.P Chemistry
UNIT 2: Solutions and net ionic reactions( chapter 4 Part I)
Day 2
Learning Objectives:
Students will be able to:
 Demonstrate knowledge of solution Stoichiometry including
strong, weak and non electrolytes.
 Calculate the Molarity of unknown solutions and ions in the solution
 know the different parts of a solution, how they can influence a solution’s properties
 Calculate the concentration of a solution.
 Describe how to make a solution of known concentration
 Describe how to make a solution of a known concentration by diluting a stock solution
NJCCC standards addressed:
5.2.12.A.5 Describe the process by which solutes dissolve in solvents.
5.2.2.A.1 Sort and describe objects based on the materials of which they are made and their physical
properties.
5.2.8.A.1 Explain that all matter is made of atoms, and give examples of common elements
5.2.8.A.2 Analyze and explain the implications of the statement “all substances are composed of
elements.”
5.2.6.B.1 Compare the properties of reactants with the properties of the products when two or more
substances are combined and reaction
5.2.8.B.1 Explain, using an understanding of the concept of chemical change, why the mass of reactants
and the mass of products
5.2.12.B.3 Balance chemical equations by applying the law of conservation of mass.
Motivation:
Development:
Solution Power point lecture
Summary/Assessment:
Homework
Section 2- Problems 25all,27all,26all,29,30,31,32,33,34,67,41,43,87
Riar: A.P Chemistry
UNIT 2: Solutions and net ionic reactions( chapter 4 Part I)
Day 3
Learning Objectives:
Students will be able to:

Apply memorized solubility rules in writing precipitation reactions

Write the Overall Ionic equations and Net Ionic equations for Double Displacement
Reactions
Find the amounts of reactants and products
Perform calculations involving limiting reactants.


NJCCC standards addressed:
5.2.12.A.5 Describe the process by which solutes dissolve in solvents.
5.2.2.A.1 Sort and describe objects based on the materials of which they are made and their physical
properties.
5.2.8.A.1 Explain that all matter is made of atoms, and give examples of common elements
5.2.8.A.2 Analyze and explain the implications of the statement “all substances are composed of
elements.”
5.2.6.B.1 Compare the properties of reactants with the properties of the products when two or more
substances are combined and reaction
5.2.8.B.1 Explain, using an understanding of the concept of chemical change, why the mass of reactants
and the mass of products
5.2.12.B.3 Balance chemical equations by applying the law of conservation of mass.
Motivation:
Development:
Solution Power point lecture
Summary/Assessment:
Homework
Section 3 – Problems 35,36,37,38,39,40,68,70,71,72,73,74,83,84,85,90,91
Riar: A.P Chemistry
UNIT 2: Solutions and net ionic reactions( chapter 4 Part I)
Day4
Learning Objectives:
 Students will be able to:
 Perform Calculations involving acid-base titration
 Identify and explain the changes in precipitation, acid base reactions
 Understand the terms associated with acid-base reactions.
NJCCC standards addressed:
5.2.12.A.5 Describe the process by which solutes dissolve in solvents.
5.2.2.A.1 Sort and describe objects based on the materials of which they are made and their physical
properties.
5.2.8.A.1 Explain that all matter is made of atoms, and give examples of common elements
5.2.8.A.2 Analyze and explain the implications of the statement “all substances are composed of
elements.”
5.2.6.B.1 Compare the properties of reactants with the properties of the products when two or more
substances are combined and reaction
5.2.8.B.1 Explain, using an understanding of the concept of chemical change, why the mass of reactants
and the mass of products
5.2.12.B.3 Balance chemical equations by applying the law of conservation of mass.
Motivation:
Development:
Solution Power point lecture
Summary/Assessment:
Homework
Section 4 – Problems 45ac,46b,47,48,49,51,52,75,76,77,94
Riar: A.P Chemistry
UNIT 2: Solutions and net ionic reactions( chapter 4 Part I)
Day5
Learning Objectives:
 Students will be able to:
 Discover the mole ratio in which substances react and find the balancing coefficients for
the reaction without knowing the identity of the reactants
 To plot and interpret a continuous variation graph using graphing calculator
NJCCC standards addressed:
5.2.12.A.5 Describe the process by which solutes dissolve in solvents.
5.2.2.A.1 Sort and describe objects based on the materials of which they are made and their physical
properties.
5.2.8.A.1 Explain that all matter is made of atoms, and give examples of common elements
5.2.8.A.2 Analyze and explain the implications of the statement “all substances are composed of
elements.”
5.2.6.B.1 Compare the properties of reactants with the properties of the products when two or more
substances are combined and reaction
5.2.8.B.1 Explain, using an understanding of the concept of chemical change, why the mass of reactants
and the mass of products
5.2.12.B.3 Balance chemical equations by applying the law of conservation of mass.
Motivation:
Development:
Students will perform the procedure of the continuous variation lab
Students will use their collect data and given Molarity of the unknown reactants A & B to
calculate the mole/mole ratio
Students will use their collect data and class data to construct a continuous variation graph
using a graphing calculator
Students will be able to predict the mole/mole ratio of the two reactants from their graph using
the linear regression equations of the two lines which intersect at the ideal mole ratio
Summary/Assessment:
Compare Class results
Discuss the importance of the Continuous variation method of finding the stoichiometric ratios of two
unknown reactants.
Homework
Chapter 4 Section4 - 53,55,57,59, and 61
Review chapter 4 Part I test
Riar: A.P Chemistry
UNIT 2: Solutions and net ionic reactions( chapter 4 Part I)
Day 6
Learning Objectives:
 Students will be able to:
 Discover the mole ratio in which substances react and find the balancing coefficients for
the reaction without knowing the identity of the reactants
 To plot and interpret a continuous variation graph using graphing calculator
NJCCC standards addressed:
5.2.12.A.5 Describe the process by which solutes dissolve in solvents.
5.2.2.A.1 Sort and describe objects based on the materials of which they are made and their physical
properties.
5.2.8.A.1 Explain that all matter is made of atoms, and give examples of common elements
5.2.8.A.2 Analyze and explain the implications of the statement “all substances are composed of
elements.”
5.2.6.B.1 Compare the properties of reactants with the properties of the products when two or more
substances are combined and reaction
5.2.8.B.1 Explain, using an understanding of the concept of chemical change, why the mass of reactants
and the mass of products
5.2.12.B.3 Balance chemical equations by applying the law of conservation of mass.
Motivation:
Development:
Students will perform the procedure of the continuous variation lab
Students will use their collect data and given Molarity of the unknown reactants A & B to
calculate the mole/mole ratio
Students will use their collect data and class data to construct a continuous variation graph
using a graphing calculator
Students will be able to predict the mole/mole ratio of the two reactants from their graph using
the linear regression equations of the two lines which intersect at the ideal mole ratio
Summary/Assessment:
Compare Class results
Discuss the importance of the Continuous variation method of finding the stoichiometric ratios of two
unknown reactants.
Homework
Review chapter 4 Part I test
Riar: A.P Chemistry
UNIT 2: Oxidation / Reduction Reactions – Redox Reactions ( chapter 4 Part
II)
Day 1
Learning Objectives:




Students will be able to:
Explain what is an Oxidation State
Assign Oxidation # to elements in various compounds and in the elemental state
Identify Oxidation – Reduction Reactions and the corresponding oxidizing and reducing
agent
NJCCC standards addressed:
5.2.12.A.5 Describe the process by which solutes dissolve in solvents.
5.2.2.A.1 Sort and describe objects based on the materials of which they are made and their physical
properties.
5.2.8.A.1 Explain that all matter is made of atoms, and give examples of common elements
5.2.8.A.2 Analyze and explain the implications of the statement “all substances are composed of
elements.”
5.2.6.B.1 Compare the properties of reactants with the properties of the products when two or more
substances are combined and reaction
5.2.8.B.1 Explain, using an understanding of the concept of chemical change, why the mass of reactants
and the mass of products
5.2.12.B.3 Balance chemical equations by applying the law of conservation of mass.
Motivation:
Oxidation of Cu metal in HNO3 acid solution Demo
Development:
Redox Power point presentation
Summary/Assessment:
Students will be able Assign Oxidation # to elements in various compounds and in the
elemental state
Explain what is an Oxidizing and reducing agent
Homework
Worksheet assigning oxidation # to various elements
Riar: A.P Chemistry
UNIT 2: : Oxidation / Reduction Reactions – Redox Reactions
( chapter 4 Part II)
Day 2
Learning Objectives:





Students will be able to:
Identify a redox reaction
Identify and write Oxidation and Reduction Half reactions
Balance Redox reactions by the change in oxidation number method
Balance Redox reactions by Half reaction method
NJCCC standards addressed:
5.2.12.A.5 Describe the process by which solutes dissolve in solvents.
5.2.2.A.1 Sort and describe objects based on the materials of which they are made and their physical
properties.
5.2.8.A.1 Explain that all matter is made of atoms, and give examples of common elements
5.2.8.A.2 Analyze and explain the implications of the statement “all substances are composed of
elements.”
5.2.6.B.1 Compare the properties of reactants with the properties of the products when two or more
substances are combined and reaction
5.2.8.B.1 Explain, using an understanding of the concept of chemical change, why the mass of reactants
and the mass of products
5.2.12.B.3 Balance chemical equations by applying the law of conservation of mass.
Motivation:
Development:
Redox Power point presentation
Students will follow the method for balancing the Redox reactions
Summary/Assessment:
Exit Ticket – Balance one Redox reaction in acid solution
Homework:
Chapter 4 Section4 – 63,79, 80, 81,92all
Riar: A.P Chemistry
UNIT 2: Oxidation / Reduction Reactions – Redox Reactions ( chapter 4 Part
II)
Day 3
Learning Objectives:




Students will be able to: 
Perform a Redox Titration
Standardize a Stock KMnO4 (aq) Solution
Find the % of Fe+2 in Iron Pills
NJCCC standards addressed:
5.2.12.A.5 Describe the process by which solutes dissolve in solvents.
5.2.2.A.1 Sort and describe objects based on the materials of which they are made and their physical
properties.
5.2.8.A.1 Explain that all matter is made of atoms, and give examples of common elements
5.2.8.A.2 Analyze and explain the implications of the statement “all substances are composed of
elements.”
5.2.6.B.1 Compare the properties of reactants with the properties of the products when two or more
substances are combined and reaction
5.2.8.B.1 Explain, using an understanding of the concept of chemical change, why the mass of reactants
and the mass of products
5.2.12.B.3 Balance chemical equations by applying the law of conservation of mass.
Motivation:
Development:
Students will perform the procedure of Part A Standardization of KMnO4
Students will use their collected data of volume of KMnO4 used to titrate the samples to
calculate the Molarity of the KMnO4solution.
Students will use the moles of KMnO4 used to calculate the moles of Fe+2 present in the pill
sample based on the balanced redox equation
Students will determine the gram Fe+2 equivalent to this number of moles.
Students will Compare Class results
Summary/Assessment:
Discuss the importance of the Volumetric analysis method of finding the stoichiometric ratios of
reactants.
Homework
Lab report for the % Fe +2 in Iron pills lab due
Riar: A.P Chemistry
UNIT 2: : Oxidation / Reduction Reactions – Redox Reactions
( chapter 4 Part II)
Day 4
Learning Objectives:





Students will be able to:
Identify and write Oxidation and Reduction Half reactions
Balance a Redox reaction in an acid solution
Balance a Redox reaction in an Basic solution
Balance Redox reactions by Half reaction method
NJCCC standards addressed:
5.2.12.A.5 Describe the process by which solutes dissolve in solvents.
5.2.2.A.1 Sort and describe objects based on the materials of which they are made and their physical
properties.
5.2.8.A.1 Explain that all matter is made of atoms, and give examples of common elements
5.2.8.A.2 Analyze and explain the implications of the statement “all substances are composed of
elements.”
5.2.6.B.1 Compare the properties of reactants with the properties of the products when two or more
substances are combined and reaction
5.2.8.B.1 Explain, using an understanding of the concept of chemical change, why the mass of reactants
and the mass of products
5.2.12.B.3 Balance chemical equations by applying the law of conservation of mass.
Motivation:
Development:
Redox Power point presentation
Students will follow the method for balancing the Redox reactions
Summary/Assessment:
Homework
Mortimer Questions-13.13all ,13.19all ,13.21 all
UNIT 2: : Oxidation / Reduction Reactions – Redox Reactions
( chapter 4 Part II)
Day 5
Learning Objectives:




Students will be able to:
Balance a Redox reaction and do Volumetric analysis of the products
Balance Redox reactions by Half reaction method
Predict Products of a Redox reaction
NJCCC standards addressed:
5.2.12.A.5 Describe the process by which solutes dissolve in solvents.
5.2.2.A.1 Sort and describe objects based on the materials of which they are made and their physical
properties.
5.2.8.A.1 Explain that all matter is made of atoms, and give examples of common elements
5.2.8.A.2 Analyze and explain the implications of the statement “all substances are composed of
elements.”
5.2.6.B.1 Compare the properties of reactants with the properties of the products when two or more
substances are combined and reaction
5.2.8.B.1 Explain, using an understanding of the concept of chemical change, why the mass of reactants
and the mass of products
5.2.12.B.3 Balance chemical equations by applying the law of conservation of mass.
Motivation:
Development:
Students will be given an worksheet with a table that shows that possible products of oxidation and
reduction reaction
Students will follow the example problems for predicting products
Summary/Assessment:
Homework
A.P Exam questions an predicting Products of Redox reactions for the years 72, 73,74,
76,77, 80 , 82 ,85, 89
Riar: A.P Chemistry
UNIT 2: : Oxidation / Reduction Reactions – Redox Reactions
( chapter 4 Part II)
Day 6
Learning Objectives:




Students will be able to:
Balance a Redox reaction and do Volumetric analysis of the products
Balance Redox reactions by Half reaction method
Predict Products of a Redox reaction
NJCCC standards addressed:
5.2.12.A.5 Describe the process by which solutes dissolve in solvents.
5.2.2.A.1 Sort and describe objects based on the materials of which they are made and their physical
properties.
5.2.8.A.1 Explain that all matter is made of atoms, and give examples of common elements
5.2.8.A.2 Analyze and explain the implications of the statement “all substances are composed of
elements.”
5.2.6.B.1 Compare the properties of reactants with the properties of the products when two or more
substances are combined and reaction
5.2.8.B.1 Explain, using an understanding of the concept of chemical change, why the mass of reactants
and the mass of products
5.2.12.B.3 Balance chemical equations by applying the law of conservation of mass.
Motivation:
Development:
Students will be given an worksheet with a table that shows that possible products of oxidation and
reduction reaction
Students will follow the example problems for predicting products
Summary/Assessment:
Review Chapter 4 part II Redox reactions
Homework
A.P Exam questions an predicting Products of Redox reactions for the years
72, 73,74, 76,77, 80 , 82 ,85, 89
Chapter 4 part II Redox reactions test
Riar: A.P Chemistry
UNIT 3: : Gases Chapter 5
Learning Objectives:
 Students will be able to:
 Understand what is pressure and units of measuring pressure
 Understand how does a barometer works? And what does it measure
 Convert from one unit of pressure to the other
NJCCC standards addressed:
5.2.12.A.5 Describe the process by which solutes dissolve in solvents.
5.2.2.A.1 Sort and describe objects based on the materials of which they are made and their physical
properties.
5.2.8.A.1 Explain that all matter is made of atoms, and give examples of common elements
5.2.8.A.2 Analyze and explain the implications of the statement “all substances are composed of
elements.”
5.2.6.B.1 Compare the properties of reactants with the properties of the products when two or more
substances are combined and reaction
5.2.8.B.1 Explain, using an understanding of the concept of chemical change, why the mass of reactants
and the mass of products
5.2.12.B.3 Balance chemical equations by applying the law of conservation of mass.
Motivation:
Show them a Barometer and how to read a barometer
Demo: Crushing the can
Development:
Gas Laws chapter 5 Power point presentation
Summary/Assessment:
Homework
Section 2 - 59,61, 63, 85, 97,99
Riar: A.P Chemistry
UNIT 3: : Gases Chapter 5
Learning Objectives:
 Students will be able to:


Understand the Ideal gas Law formulated by Boyle, Charles, Dalton , and Graham and solve
problems based on these laws
Use the Kinetic Molecular Theory to explain the theoretical basis for the gas laws

NJCCC standards addressed:
5.2.12.A.5 Describe the process by which solutes dissolve in solvents.
5.2.2.A.1 Sort and describe objects based on the materials of which they are made and their physical
properties.
5.2.8.A.1 Explain that all matter is made of atoms, and give examples of common elements
5.2.8.A.2 Analyze and explain the implications of the statement “all substances are composed of
elements.”
5.2.6.B.1 Compare the properties of reactants with the properties of the products when two or more
substances are combined and reaction
5.2.8.B.1 Explain, using an understanding of the concept of chemical change, why the mass of reactants
and the mass of products
5.2.12.B.3 Balance chemical equations by applying the law of conservation of mass.
Motivation:
Demo: Hydrogen and Oxygen Balloon and hydrogen Balloon
Development:
Gas Laws chapter 5 Power point presentation
Summary/Assessment:
Homework
Section 1 - 21,23,25,33,41,45,57,91,93,94,98,99
Riar: A.P Chemistry
UNIT 3: : Gases Chapter 5
Learning Objectives:









Students will be able to:
Find the density of a sample of a gas at STP if its mass, volume and pressure are known under
non standard conditions
Use the Kinetic Molecular Theory to explain the theoretical basis for the gas laws
Find the density of a sample of a gas at specific temperature if density of the gas at another
temperature and pressure is known
Understand what is a mole fraction and how is it represented
Understand What does Dalton’s law mean when you collect a gas over water
Understand what is Partial pressure?
Understand the difference between diffusion and effusion
Calculate the Root mean square velocity of the gas particles under given conditions
NJCCC standards addressed:
5.2.12.A.5 Describe the process by which solutes dissolve in solvents.
5.2.2.A.1 Sort and describe objects based on the materials of which they are made and their physical
properties.
5.2.8.A.1 Explain that all matter is made of atoms, and give examples of common elements
5.2.8.A.2 Analyze and explain the implications of the statement “all substances are composed of
elements.”
5.2.6.B.1 Compare the properties of reactants with the properties of the products when two or more
substances are combined and reaction
5.2.8.B.1 Explain, using an understanding of the concept of chemical change, why the mass of reactants
and the mass of products
5.2.12.B.3 Balance chemical equations by applying the law of conservation of mass.
Motivation:
Development:
Gas Laws chapter 5 Power point presentation
Summary/Assessment:
Homework
Section 3 - 47, 49, 51, 52, 53,67,68,89
Riar: A.P Chemistry
UNIT 3: : Gases Chapter 5
Learning Objectives:
Students will be able to:
Find the Formula Mass of the disposable lighter gas using the Ideal gas Laws


NJCCC standards addressed:
5.2.12.A.5 Describe the process by which solutes dissolve in solvents.
5.2.2.A.1 Sort and describe objects based on the materials of which they are made and their physical
properties.
5.2.8.A.1 Explain that all matter is made of atoms, and give examples of common elements
5.2.8.A.2 Analyze and explain the implications of the statement “all substances are composed of
elements.”
5.2.6.B.1 Compare the properties of reactants with the properties of the products when two or more
substances are combined and reaction
5.2.8.B.1 Explain, using an understanding of the concept of chemical change, why the mass of reactants
and the mass of products
5.2.12.B.3 Balance chemical equations by applying the law of conservation of mass.
Motivation:
Development:
Students will perform the procedure of the Lighter gas lab
Students will measure the volume of the lighter gas collected and measure the temperature of the
gas and find the pressure of the gas collected over water from the barometric pressure
Students will use their collect data and Ideal gas law to determine the formula mass of the
unknown lighter gas
Students will Compare Class results
Summary/Assessment:
Homework
Lab report for the unknown lighter gas lab due
Riar: A.P Chemistry
UNIT 3: : Gases Chapter 5
Learning Objectives:





Students will be able to:
Understand the Ideal gas behavior
Understand the typical conditions for non-ideal behavior
Understand the Vander wails gas equation as the corrected gas equation for non-ideal
conditions
Understand What a and b stand for in Vander Waals equation
NJCCC standards addressed:
5.2.12.A.5 Describe the process by which solutes dissolve in solvents.
5.2.2.A.1 Sort and describe objects based on the materials of which they are made and their physical
properties.
5.2.8.A.1 Explain that all matter is made of atoms, and give examples of common elements
5.2.8.A.2 Analyze and explain the implications of the statement “all substances are composed of
elements.”
5.2.6.B.1 Compare the properties of reactants with the properties of the products when two or more
substances are combined and reaction
5.2.8.B.1 Explain, using an understanding of the concept of chemical change, why the mass of reactants
and the mass of products
5.2.12.B.3 Balance chemical equations by applying the law of conservation of mass.
Motivation:
Development:
Gas Laws chapter 5 Power point presentation
Summary/Assessment:
Homework
69,71,73,75,77,78,79,81,83,84,110,111
Test Chapter 5 Gases
Riar: A.P Chemistry
UNIT 3: : Gases Chapter 5
Learning Objectives:
 Students will be able to:
 Solve mixed mass volume problems when there are standard conditions of temperature
and pressure
 Solve mixed mass volume problems when there are non standard conditions of
temperature and pressure
 Use Avogadro’s law in stoichiometry
NJCCC standards addressed:
5.2.12.A.5 Describe the process by which solutes dissolve in solvents.
5.2.2.A.1 Sort and describe objects based on the materials of which they are made and their physical
properties.
5.2.8.A.1 Explain that all matter is made of atoms, and give examples of common elements
5.2.8.A.2 Analyze and explain the implications of the statement “all substances are composed of
elements.”
5.2.6.B.1 Compare the properties of reactants with the properties of the products when two or more
substances are combined and reaction
5.2.8.B.1 Explain, using an understanding of the concept of chemical change, why the mass of reactants
and the mass of products
5.2.12.B.3 Balance chemical equations by applying the law of conservation of mass.
Motivation:
Development:
Gas Laws chapter 5 Power point presentation
Summary/Assessment:
Homework
Old A.P Exam Free Response questions
Test Chapter 5 Gases
Riar: A.P Chemistry
UNIT 4: Thermo Chemistry Chapter 6
Learning Objectives:
 Students will be able to:





Distinguish the various forms that energy takes in an ensemble of atoms or molecules
Understand the first law of thermodynamics
Understand the difference between Heat and Temperature
Understand the difference between a system and surroundings
Understand that the internal energy of a system is changed by the transfer of heat and work
Recognize that temperature ,volume ,pressure and energy are all state functions


NJCCC standards addressed:
5.2.12.A.5 Describe the process by which solutes dissolve in solvents.
5.2.2.A.1 Sort and describe objects based on the materials of which they are made and their physical
properties.
5.2.8.A.1 Explain that all matter is made of atoms, and give examples of common elements
5.2.8.A.2 Analyze and explain the implications of the statement “all substances are composed of
elements.”
5.2.6.B.1 Compare the properties of reactants with the properties of the products when two or more
substances are combined and reaction
5.2.8.B.1 Explain, using an understanding of the concept of chemical change, why the mass of reactants
and the mass of products
5.2.12.B.3 Balance chemical equations by applying the law of conservation of mass.
Motivation:
Conservation of energy and transfer of energy Demo
Development:
Thermo Chemistry Chapter 6 power point presentation
Summary/Assessment:
Homework
Read and summarize the National Geographic Article from Oct 2007- Global Warming
Riar: A.P Chemistry
UNIT 4: Thermo Chemistry Chapter 6
Learning Objectives:






Students will be able to:
Explain which way is heat moving and the sign of each
Understand difference between Exothermic and Endothermic reactions
Calculate the change in energy as a result of heat transfer or work done or both
Understand the difference between specific heat and heat capacity
NJCCC standards addressed:
5.2.12.A.5 Describe the process by which solutes dissolve in solvents.
5.2.2.A.1 Sort and describe objects based on the materials of which they are made and their physical
properties.
5.2.8.A.1 Explain that all matter is made of atoms, and give examples of common elements
5.2.8.A.2 Analyze and explain the implications of the statement “all substances are composed of
elements.”
5.2.6.B.1 Compare the properties of reactants with the properties of the products when two or more
substances are combined and reaction
5.2.8.B.1 Explain, using an understanding of the concept of chemical change, why the mass of reactants
and the mass of products
5.2.12.B.3 Balance chemical equations by applying the law of conservation of mass.
Motivation:
Development:
Thermo Chemistry Chapter 6 power point presentation
Summary/Assessment:
Homework
Section 1 - 31,32,33,36,39,43,45,47,48,50,75,81
Riar: A.P Chemistry
UNIT 4: Thermo Chemistry Chapter 6
Learning Objectives:





Students will be able to:
Understand what is Hess law
Understand what is enthalpy
Calculate the change in enthalpy of a reaction by applying Hess law
Explain the difference between the direct method and indirect method of solving for
enthalpy
NJCCC standards addressed:
5.2.12.A.5 Describe the process by which solutes dissolve in solvents.
5.2.2.A.1 Sort and describe objects based on the materials of which they are made and their physical
properties.
5.2.8.A.1 Explain that all matter is made of atoms, and give examples of common elements
5.2.8.A.2 Analyze and explain the implications of the statement “all substances are composed of
elements.”
5.2.6.B.1 Compare the properties of reactants with the properties of the products when two or more
substances are combined and reaction
5.2.8.B.1 Explain, using an understanding of the concept of chemical change, why the mass of reactants
and the mass of products
5.2.12.B.3 Balance chemical equations by applying the law of conservation of mass.
Motivation:
Development:
Thermo Chemistry Chapter 6 power point presentation
Summary/Assessment:
Homework
Section 2 Hess law- 53,55,57,59,61,63,65,67,78,81,82,83,88,89
Riar: A.P Chemistry
UNIT 4: Thermo Chemistry Chapter 6
Learning Objectives:

Students will be able to:


Measure the heat of the reaction associated with complete ionization of Ammonia in water
Measure the enthalpy change of two separate reactions and then apply Hess law to
calculate the overall enthalpy change of the desired reaction
NJCCC standards addressed:
5.2.12.A.5 Describe the process by which solutes dissolve in solvents.
5.2.2.A.1 Sort and describe objects based on the materials of which they are made and their physical
properties.
5.2.8.A.1 Explain that all matter is made of atoms, and give examples of common elements
5.2.8.A.2 Analyze and explain the implications of the statement “all substances are composed of
elements.”
5.2.6.B.1 Compare the properties of reactants with the properties of the products when two or more
substances are combined and reaction
5.2.8.B.1 Explain, using an understanding of the concept of chemical change, why the mass of reactants
and the mass of products
5.2.12.B.3 Balance chemical equations by applying the law of conservation of mass.
Motivation:
Development:
Students will perform the procedure of the Enthalpy change for the complete Ionization of
ammonia lab
Students will use their collect data to calculate the heat transferred in both the reactions and then
calculate the H for both reactions
Students will apply Hess law to calculate the H of the desired reaction
Students will compare and analyze class results
Summary/Assessment:
Homework
Lab report Enthalpy change for the complete Ionization of ammonia lab due
Riar: A.P Chemistry
UNIT 4: Thermo Chemistry Chapter 6
Learning Objectives:





Students will be able to:
Understand what is the Bond energy
Calculate the H by the Bond energy equation
Understand what is lattice energy
Explain the effect of ionic radius and charge of the ion on the Lattice energy of an
Ionic Compound
 Illustrate the formation of an Ionic solid and calculate the H of formation by Bohrn
Haber Cycle
NJCCC standards addressed:
5.2.12.A.5 Describe the process by which solutes dissolve in solvents.
5.2.2.A.1 Sort and describe objects based on the materials of which they are made and their physical
properties.
5.2.8.A.1 Explain that all matter is made of atoms, and give examples of common elements
5.2.8.A.2 Analyze and explain the implications of the statement “all substances are composed of
elements.”
5.2.6.B.1 Compare the properties of reactants with the properties of the products when two or more
substances are combined and reaction
5.2.8.B.1 Explain, using an understanding of the concept of chemical change, why the mass of reactants
and the mass of products
5.2.12.B.3 Balance chemical equations by applying the law of conservation of mass.
Motivation:
Development:
Thermo Chemistry Chapter 6 power point presentation
Summary/Assessment:
Homework
Section 2 Chapter 8-35,37,39,41,43,45,55,51
A.P Free Response questions
Riar: A.P Chemistry
UNIT 4: Thermo Chemistry Chapter 6
Learning Objectives:





Students will be able to:
Understand what is the Bond energy
Calculate the H by the Bond energy equation
Understand what is lattice energy
Explain the effect of ionic radius and charge of the ion on the Lattice energy of an
Ionic Compound
 Illustrate the formation of an Ionic solid and calculate the H of formation by Bohrn
Haber Cycle
NJCCC standards addressed:
5.2.12.A.5 Describe the process by which solutes dissolve in solvents.
5.2.2.A.1 Sort and describe objects based on the materials of which they are made and their physical
properties.
5.2.8.A.1 Explain that all matter is made of atoms, and give examples of common elements
5.2.8.A.2 Analyze and explain the implications of the statement “all substances are composed of
elements.”
5.2.6.B.1 Compare the properties of reactants with the properties of the products when two or more
substances are combined and reaction
5.2.8.B.1 Explain, using an understanding of the concept of chemical change, why the mass of reactants
and the mass of products
5.2.12.B.3 Balance chemical equations by applying the law of conservation of mass.
Motivation:
Development:
Thermo Chemistry Chapter 6 power point presentation
Summary/Assessment:
Homework
Review for the test
Thermo Chemistry Chapter 6 Test
Riar: A.P Chemistry
UNIT 5: Atomic Structure and Periodicity Chapter 7
Learning Objectives:



Students will be able to:
Explain what is Electromagnetic Radiation
Explain the relationship between the wavelength and frequency of high energy
gamma rays and low energy radio waves
Understand the wave particle duality nature of light


NJCCC standards addressed:
5.2.12.A.5 Describe the process by which solutes dissolve in solvents.
5.2.2.A.1 Sort and describe objects based on the materials of which they are made and their physical
properties.
5.2.8.A.1 Explain that all matter is made of atoms, and give examples of common elements
5.2.8.A.2 Analyze and explain the implications of the statement “all substances are composed of
elements.”
5.2.6.B.1 Compare the properties of reactants with the properties of the products when two or more
substances are combined and reaction
5.2.8.B.1 Explain, using an understanding of the concept of chemical change, why the mass of reactants
and the mass of products
5.2.12.B.3 Balance chemical equations by applying the law of conservation of mass.
Motivation:
Development:
Atomic Structure and Periodicity Chapter 7 power point presentation
Summary/Assessment:
Homework
Section 1 - 35,37, 41, 47,49,54,109,110,111
Riar: A.P Chemistry
UNIT 5: Atomic Structure and Periodicity Chapter 7
Learning Objectives:






Students will be able to:
Explain the basis of quantum theory
Understand the atomic spectra of Hydrogen and Bohr’s model of an atom
Understand what are photons and emission spectra
Understand the difference between an electron in a ground state and excitedstate
Calculate the energy of an electron in its ground state and energy needed to move to a
higher energy state
NJCCC standards addressed:
5.2.12.A.5 Describe the process by which solutes dissolve in solvents.
5.2.2.A.1 Sort and describe objects based on the materials of which they are made and their physical
properties.
5.2.8.A.1 Explain that all matter is made of atoms, and give examples of common elements
5.2.8.A.2 Analyze and explain the implications of the statement “all substances are composed of
elements.”
5.2.6.B.1 Compare the properties of reactants with the properties of the products when two or more
substances are combined and reaction
5.2.8.B.1 Explain, using an understanding of the concept of chemical change, why the mass of reactants
and the mass of products
5.2.12.B.3 Balance chemical equations by applying the law of conservation of mass.
Motivation:
Development:
Atomic Structure and Periodicity Chapter 7 power point Presentation
Summary/Assessment:
Homework
Section 2- 49,51,109,110,111,113,114, 131
Riar: A.P Chemistry
UNIT 5: Atomic Structure and Periodicity Chapter 7
Learning Objectives:






Students will be able to:
Explain the use of wave mechanics in atomic theory
Describe the wave -mechanical model of an atom
Understand the Heisenberg’s uncertainty Principle
Understand the 4 quantum #s, orbital shapes, electron spin and Pauli’s exclusion
Principle
Explain how each of the quantum #s indicate an Electron location
NJCCC standards addressed:
5.2.12.A.5 Describe the process by which solutes dissolve in solvents.
5.2.2.A.1 Sort and describe objects based on the materials of which they are made and their physical
properties.
5.2.8.A.1 Explain that all matter is made of atoms, and give examples of common elements
5.2.8.A.2 Analyze and explain the implications of the statement “all substances are composed of
elements.”
5.2.6.B.1 Compare the properties of reactants with the properties of the products when two or more
substances are combined and reaction
5.2.8.B.1 Explain, using an understanding of the concept of chemical change, why the mass of reactants
and the mass of products
5.2.12.B.3 Balance chemical equations by applying the law of conservation of mass.
Motivation:
Development:
Atomic Structure and Periodicity Chapter 7 power point presentation
Summary/Assessment:
Homework
Section 2 44,55,57,59,60,63,64,65,66,67,71,73,74,75,77,78,79,80,113,114,115,117,119,121,129,
Riar: A.P Chemistry
UNIT 5: Atomic Structure and Periodicity Chapter 7
Learning Objectives:








Students will be able to:
Understand what is an electron Configuration
Write an electron configuration of an element
Explain Hund’s Rule and Aufbau principle
Explain the relationship between valence electrons and columns
Understand what is an atomic radius and the trends in the P.T
Explain how are ions derived from representative elements
Explain the concept of shielding
NJCCC standards addressed:
5.2.12.A.5 Describe the process by which solutes dissolve in solvents.
5.2.2.A.1 Sort and describe objects based on the materials of which they are made and their physical
properties.
5.2.8.A.1 Explain that all matter is made of atoms, and give examples of common elements
5.2.8.A.2 Analyze and explain the implications of the statement “all substances are composed of
elements.”
5.2.6.B.1 Compare the properties of reactants with the properties of the products when two or more
substances are combined and reaction
5.2.8.B.1 Explain, using an understanding of the concept of chemical change, why the mass of reactants
and the mass of products
5.2.12.B.3 Balance chemical equations by applying the law of conservation of mass.
Motivation:
Development:
Atomic Structure and Periodicity Chapter 7 power point presentation
Summary/Assessment:
Homework
Section 3 81,83,85,87,89,90,91,93,95,97,99,101,123,124,125,126,128,133,134
A.P Exam Free Response Take home due
Riar: A.P Chemistry
UNIT 5: Atomic Structure and Periodicity Chapter 7
Learning Objectives:









Students will be able to:
Understand the history of the Periodic table and the contributions of Moseley and
Mendeleev
Explain the relationship between valence electrons and columns
Understand what is an atomic radius and the trends in the P.T
Explain how are ions derived from representative elements
Understand what is Ionization energy and the trends in the P.T
Understand what is Electron affinity energy and the trends in the P.T
Understand what is an Ionic radius and the trends in the P.T
Explain how the properties of a group - Alkali metals
NJCCC standards addressed:
5.2.12.A.5 Describe the process by which solutes dissolve in solvents.
5.2.2.A.1 Sort and describe objects based on the materials of which they are made and their physical
properties.
5.2.8.A.1 Explain that all matter is made of atoms, and give examples of common elements
5.2.8.A.2 Analyze and explain the implications of the statement “all substances are composed of
elements.”
5.2.6.B.1 Compare the properties of reactants with the properties of the products when two or more
substances are combined and reaction
5.2.8.B.1 Explain, using an understanding of the concept of chemical change, why the mass of reactants
and the mass of products
5.2.12.B.3 Balance chemical equations by applying the law of conservation of mass.
Motivation:
Development:
Atomic Structure and Periodicity Chapter 7 power point presentation
Summary/Assessment:
Homework
Section 3 81,83,85,87,89,90,91,93,95,97,99,101,123,124,125,126,128,133,134
A.P Exam Free Response Take home due
Riar: A.P Chemistry
UNIT 5: Atomic Structure and Periodicity Chapter 7
Learning Objectives:









Students will be able to:
Understand the history of the Periodic table and the contributions of Moseley and
Mendeleev
Explain the relationship between valence electrons and columns
Understand what is an atomic radius and the trends in the P.T
Explain how are ions derived from representative elements
Understand what is Ionization energy and the trends in the P.T
Understand what is Electron affinity energy and the trends in the P.T
Understand what is an Ionic radius and the trends in the P.T
Explain how the properties of a group - Alkali metals
NJCCC standards addressed:
5.2.12.A.5 Describe the process by which solutes dissolve in solvents.
5.2.2.A.1 Sort and describe objects based on the materials of which they are made and their physical
properties.
5.2.8.A.1 Explain that all matter is made of atoms, and give examples of common elements
5.2.8.A.2 Analyze and explain the implications of the statement “all substances are composed of
elements.”
5.2.6.B.1 Compare the properties of reactants with the properties of the products when two or more
substances are combined and reaction
5.2.8.B.1 Explain, using an understanding of the concept of chemical change, why the mass of reactants
and the mass of products
5.2.12.B.3 Balance chemical equations by applying the law of conservation of mass.
Motivation:
Development:
Atomic Structure and Periodicity Chapter 7 power point presentation
Summary/Assessment:
Homework
Review for Atomic Structure and Periodicity Chapter 7
Riar: A.P Chemistry
UNIT 6: Chemical Bonding Chapter 8 &9 &10
Learning Objectives:
 Students will be able to:
Define, compare and contrast, classify, differentiate, put in order, predict using, identify correct
and incorrect examples of, identify correct and incorrect interpretations of, identify correct and
incorrect applications of…the following terms:
Lewis electron-dot symbol, Lewis electron-dot structure, octet rule ionic bonding, covalent
bonding, coordinate covalent bond ,bond order ,bond type, bond length
Polar covalent bond, partial positive charge partial negative charge, non polar covalent bond










Give the Lewis electron-dot symbol for elements
Give the Lewis electron-dot symbols for ions
Drawing Lewis electron-dot structures for molecules and polyatomic ion
Go into detail about ionic bonding
Use Lewis electron-dot structures to describe ionic bonding
Go into detail about covalent bonding
Use Lewis electron-dot structures to describe covalent bonding
Identify bond order
Draw Lewis structures for molecules that do not obey the octet rule
Classify bond types according to electronegativity
NJCCC standards addressed:
5.2.12.A.5 Describe the process by which solutes dissolve in solvents.
5.2.2.A.1 Sort and describe objects based on the materials of which they are made and their physical
properties.
5.2.8.A.1 Explain that all matter is made of atoms, and give examples of common elements
5.2.8.A.2 Analyze and explain the implications of the statement “all substances are composed of
elements.”
5.2.6.B.1 Compare the properties of reactants with the properties of the products when two or more
substances are combined and reaction
5.2.8.B.1 Explain, using an understanding of the concept of chemical change, why the mass of reactants
and the mass of products
5.2.12.B.3 Balance chemical equations by applying the law of conservation of mass.
Motivation:
Development:
Chemical Bonding Chapter 8 power point presentation
Summary/Assessment:
Homework
15,17,21,23,25(a,b) ,27, 31(a,b,c) 33,35 ,37, 39
Riar: A.P Chemistry
UNIT 6: Chemical Bonding Chapter 8 &9 &10
Learning Objectives:
 Students will be able to:
Define, compare and contrast, classify, differentiate, put in order, predict using, identify correct
and incorrect examples of, identify correct and incorrect interpretations of, identify correct and
incorrect applications of…the following terms:
Lewis electron-dot symbol, Lewis electron-dot structure, octet rule, ionic bonding
covalent bonding, coordinate covalent bond,bond order ,bond type, bond length
Polar covalent bond, partial positive charge partial negative charge, non polar covalent bond










Give the Lewis electron-dot symbol for elements
Give the Lewis electron-dot symbols for ions
Drawing Lewis electron-dot structures for molecules and polyatomic ion
Go into detail about ionic bonding
Use Lewis electron-dot structures to describe ionic bonding
Go into detail about covalent bonding
Use Lewis electron-dot structures to describe covalent bonding
Identify bond order
Draw Lewis structures for molecules that do not obey the octet rule
Classify bond types according to electronegativity
NJCCC standards addressed:
5.2.12.A.5 Describe the process by which solutes dissolve in solvents.
5.2.2.A.1 Sort and describe objects based on the materials of which they are made and their physical
properties.
5.2.8.A.1 Explain that all matter is made of atoms, and give examples of common elements
5.2.8.A.2 Analyze and explain the implications of the statement “all substances are composed of
elements.”
5.2.6.B.1 Compare the properties of reactants with the properties of the products when two or more
substances are combined and reaction
5.2.8.B.1 Explain, using an understanding of the concept of chemical change, why the mass of reactants
and the mass of products
5.2.12.B.3 Balance chemical equations by applying the law of conservation of mass.
Motivation:
Development:
Chemical Bonding Chapter 8 power point presentation
Summary/Assessment:
Homework 41,91,92,93,107 ,55,95 ,96(ef), 105
Riar: A.P Chemistry
UNIT 6:Chemical Bonding Chapter 8&9&10
Learning Objectives:
 Students will be able to:
Define, compare and contrast, classify, differentiate, put in order, predict using, identify correct
and incorrect examples of, identify correct and incorrect interpretations of, identify correct and
incorrect applications of…the following terms:
delocalized bonding ,resonance description, resonance bonding ,resonance forms , polar covalent
bond moderately polar covalent bond ,very polar covalent bond , polar molecule, formal charge






Identify delocalized bonding
Draw resonance structures
Draw Lewis structures for molecules that do not obey the octet rule
Classify bond types according to electronegativity
Calculate formal charges
Determine which Lewis electron-dot structure is best if more than one is possible
NJCCC standards addressed:
5.2.12.A.5 Describe the process by which solutes dissolve in solvents.
5.2.2.A.1 Sort and describe objects based on the materials of which they are made and their physical
properties.
5.2.8.A.1 Explain that all matter is made of atoms, and give examples of common elements
5.2.8.A.2 Analyze and explain the implications of the statement “all substances are composed of
elements.”
5.2.6.B.1 Compare the properties of reactants with the properties of the products when two or more
substances are combined and reaction
5.2.8.B.1 Explain, using an understanding of the concept of chemical change, why the mass of reactants
and the mass of products
5.2.12.B.3 Balance chemical equations by applying the law of conservation of mass.
Motivation:
Development:
Chemical Bonding Chapter 8 power point presentation
Summary/Assessment:
Homework 57 all,58 all,59,61,63,66,67,68,69,70,71&72(fgh),73,75,98,99
Riar: A.P Chemistry
UNIT 6:Chemical Bonding Chapter 8&9&10
Learning Objectives:
 Students will be able to:
Define, compare and contrast, classify, differentiate, put in order, predict using, identify correct
and incorrect examples of, identify correct and incorrect interpretations of, identify correct and
incorrect applications of…the following terms:
Molecular geometry, Valence-Shell-Electron-Pair-Repulsion (VSEPR) Model, single bonds,
multiple bond ,double bonds, triple bond , lone pairs non-bonding pairs, dipole moment, valence
bond theory overlapping , hybridization, sigma bond , pi bond






Go into detail about the Valence-Shell-Electron-Pair-Repulsion (VSEPR) Model
Go into details about the rules of thumb for electron pair repulsion
Explain why multiple bonds take up more "space" than single bonds
Apply the three rules to minimize electron pair repulsion in a structure
Predict and describe the geometry of compounds with two, three, or four pairs of
electrons on the central atom, draw the most correct structure for them, and explain why
that structure is the most correct using the VSEPR model
Predict and describe the geometry of compounds with five or six pairs of electrons on the
central atom, draw the most correct structure for them, and explain why that structure is
the most correct using the VSEPR model
NJCCC standards addressed:
5.2.12.A.5 Describe the process by which solutes dissolve in solvents.
5.2.2.A.1 Sort and describe objects based on the materials of which they are made and their physical
properties.
5.2.8.A.1 Explain that all matter is made of atoms, and give examples of common elements
5.2.8.A.2 Analyze and explain the implications of the statement “all substances are composed of
elements.”
5.2.6.B.1 Compare the properties of reactants with the properties of the products when two or more
substances are combined and reaction
5.2.8.B.1 Explain, using an understanding of the concept of chemical change, why the mass of reactants
and the mass of products
5.2.12.B.3 Balance chemical equations by applying the law of conservation of mass.
Motivation:
Development:
Chemical Bonding Chapter 9 power point presentation
Summary/Assessment:
Homework
73,77&8 ,79&83,85(cd) ,87,89,100,103,109,111,112(c),113
Riar: A.P Chemistry
UNIT 6:Chemical Bonding Chapter 8&9&10
Learning Objectives:
 Students will be able to: Define, compare and contrast, classify, differentiate, put in
order, predict using, identify correct and incorrect examples of, identify correct and
incorrect interpretations of, identify correct and incorrect applications of…the
following terms:
 Molecular geometry , Valence-Shell-Electron-Pair-Repulsion (VSEPR) Model,
single bonds, multiple bond ,double bonds, triple bond , lone pairs non-bonding
pairs, dipole moment, valence bond theory overlapping , hybridization, sigma bond ,
pi bond







Go into detail about the Valence-Shell-Electron-Pair-Repulsion (VSEPR) Model
Go into details about the rules of thumb for electron pair repulsion
Explain why multiple bonds take up more "space" than single bonds
Apply the three rules to minimize electron pair repulsion in a structure
Predict and describe the geometry of compounds with two, three, or four pairs of
electrons on the central atom, draw the most correct structure for them, and explain why
that structure is the most correct using the VSEPR model
Predict and describe the geometry of compounds with five or six pairs of electrons on the
central atom, draw the most correct structure for them, and explain why that structure is
the most correct using the VSEPR model Describe the relationship between dipole
moment and a bond’s polarity
Relate dipole moment and molecular geometry for binary molecular compounds and
predict whether or not a binary molecular compound would be expected to have a zero
net dipole moment on the basis of its geometry
NJCCC standards addressed:
5.2.12.A.5 Describe the process by which solutes dissolve in solvents.
5.2.2.A.1 Sort and describe objects based on the materials of which they are made and their physical
properties.
5.2.8.A.1 Explain that all matter is made of atoms, and give examples of common elements
5.2.8.A.2 Analyze and explain the implications of the statement “all substances are composed of
elements.”
5.2.6.B.1 Compare the properties of reactants with the properties of the products when two or more
substances are combined and reaction
5.2.8.B.1 Explain, using an understanding of the concept of chemical change, why the mass of reactants
and the mass of products
5.2.12.B.3 Balance chemical equations by applying the law of conservation of mass.
Motivation:
Development:
Chemical Bonding Chapter 9 power point presentation
Summary/Assessment:
Homework: 9,11,13,23(fgjkm)25,26,27,28,29,51,53,54(ab),61
Riar: A.P Chemistry
UNIT 6: Chemical Bonding Chapter 8&9&10
Learning Objectives:

Students will be able to:
Define, compare and contrast, classify, differentiate, put in order, predict using, identify correct
and incorrect examples of, identify correct and incorrect interpretations of, identify correct and
incorrect applications of…the following terms:
Molecular geometry , Valence-Shell-Electron-Pair-Repulsion (VSEPR) Model, single bonds,
multiple bond ,double bonds, triple bond , lone pairs non-bonding pairs, dipole moment, valence
bond theory overlapping , hybridization, sigma bond , pi bond






Describe the relationship between dipole moment and a bond’s polarity
Relate dipole moment and molecular geometry for binary molecular compounds and
predict whether or not a binary molecular compound would be expected to have a zero
net dipole moment on the basis of its geometry
Go into detail about valence bond theory
Go into detail about how promotion and hybridization explain bond formation and bond
strength
Go into detail using valence bond theory to describe multiple bonding
Predict the hybridization in a compound or bond
NJCCC standards addressed:
5.2.12.A.5 Describe the process by which solutes dissolve in solvents.
5.2.2.A.1 Sort and describe objects based on the materials of which they are made and their physical
properties.
5.2.8.A.1 Explain that all matter is made of atoms, and give examples of common elements
5.2.8.A.2 Analyze and explain the implications of the statement “all substances are composed of
elements.”
5.2.6.B.1 Compare the properties of reactants with the properties of the products when two or more
substances are combined and reaction
5.2.8.B.1 Explain, using an understanding of the concept of chemical change, why the mass of reactants
and the mass of products
5.2.12.B.3 Balance chemical equations by applying the law of conservation of mass.
Motivation:
Development:
Chemical Bonding Chapter 9 power point presentation
Summary/Assessment:
Homework 29, 31, 33, 35, 85,98
Riar: A.P Chemistry
UNIT 7: Solutions Chapter 10
Learning Objectives:
 Students will be able to:
 Define, compare and contrast, classify, differentiate, put in order, predict using,
identify correct and incorrect examples of, identify correct and incorrect
interpretations of, identify correct and incorrect applications of…the following terms:
 Be able to explain why ionic interactions, hydrogen bonds, and dipole-dipole
interactions are electrostatic interactions
 Be able to describe, compare and contrast the types of intermolecular forces
 Be able to describe the two factors that affect dispersion forces and be able to predict
relative strength of dispersion forces for substances from their formula and/or
structure
 Be able to describe hydrogen bonds and be able to predict whether or not hydrogen
bonds will exist and the relative strength of hydrogen bonding for substances from
their formula and/or structure
 Be able to identify which intermolecular forces are present in substance from their
formula and/or structure
 Explain the relationship between intermolecular forces and the five mentioned
properties of liquids
 Be able to describe how the structure of each of the four types of solids explains their
physical properties
NJCCC standards addressed:
5.2.12.A.5 Describe the process by which solutes dissolve in solvents.
5.2.2.A.1 Sort and describe objects based on the materials of which they are made and their physical
properties.
5.2.8.A.1 Explain that all matter is made of atoms, and give examples of common elements
5.2.8.A.2 Analyze and explain the implications of the statement “all substances are composed of
elements.”
5.2.6.B.1 Compare the properties of reactants with the properties of the products when two or more
substances are combined and reaction
5.2.8.B.1 Explain, using an understanding of the concept of chemical change, why the mass of reactants
and the mass of products
5.2.12.B.3 Balance chemical equations by applying the law of conservation of mass.
Motivation:
Development:
Liquids and Solids Chapter 10 power point presentation
Summary/Assessment:
Homework
Homework 29, 31, 33, 35, 85,98, 83,75,77,79,84
Riar: A.P Chemistry
UNIT 7: Solutions Chapter 10
Learning Objectives:
 Students will be able to:
 Define, compare and contrast, classify, differentiate, put in order, predict using,
identify correct and incorrect examples of, identify correct and incorrect
interpretations of, identify correct and incorrect applications of…the following terms:
heat of vaporization ,vapor pressure, boiling point ,melting, freezing, vaporization
condensation, sublimation, deposition ,heat of fusion – standard enthalpy of fusion, heat
of vaporization – standard enthalpy of vaporization, volatility, equilibrium vapor
pressure, Clausius-Clapeyron equation, phase diagram ,triple point, critical point, critical
temperature ,critical pressure , Heating curve
NJCCC standards addressed:
5.2.12.A.5 Describe the process by which solutes dissolve in solvents.
5.2.2.A.1 Sort and describe objects based on the materials of which they are made and their physical
properties.
5.2.8.A.1 Explain that all matter is made of atoms, and give examples of common elements
5.2.8.A.2 Analyze and explain the implications of the statement “all substances are composed of
elements.”
5.2.6.B.1 Compare the properties of reactants with the properties of the products when two or more
substances are combined and reaction
5.2.8.B.1 Explain, using an understanding of the concept of chemical change, why the mass of reactants
and the mass of products
5.2.12.B.3 Balance chemical equations by applying the law of conservation of mass.
Motivation:
Development:
Liquids and Solids Chapter 10 power point presentation
Summary/Assessment:
Homework
Review for Part-I Chemical Bonding Chapter 8,9&10 Test
Part-I Chemical Bonding Chapter 8,9 &10 Test Take home Part-II Chemical Bonding
Chapter 8, 9&10 Test due
Riar: A.P Chemistry
UNIT 7: Solutions Chapter 11
Learning Objectives:
 Students will be able to:
Define, compare and contrast, classify, differentiate, put in order, predict using, identify correct
and incorrect examples of, identify correct and incorrect interpretations of, identify correct and
incorrect applications of…the following terms:
Solution, crystallization, soluble, insoluble, miscible , immiscible, solubility, saturated solution,
unsaturated solution, supersaturated solution, molarity, mass percentage of solute, molality,
mole fraction, Henry’s Law






Compare and contrast, and give examples of the three types of solutions based on state
Describe the solution process in terms of free energy
Describe the solution process in terms of the three processes involved in the formation of
a solution
Describe the solution process in terms of enthalpy changes, entropy changes, whether a
solution will form or not, and whether the solution process will be exothermic or
endothermic
Explain the application of enthalpy changes and entropy changes to the rule, “Like
dissolves like.”
Describe the effects of temperature and pressure on solubility and apply that to the
solubility of solids and gases
NJCCC standards addressed:
5.2.12.A.5 Describe the process by which solutes dissolve in solvents.
5.2.2.A.1 Sort and describe objects based on the materials of which they are made and their physical
properties.
5.2.8.A.1 Explain that all matter is made of atoms, and give examples of common elements
5.2.8.A.2 Analyze and explain the implications of the statement “all substances are composed of
elements.”
5.2.6.B.1 Compare the properties of reactants with the properties of the products when two or more
substances are combined and reaction
5.2.8.B.1 Explain, using an understanding of the concept of chemical change, why the mass of reactants
and the mass of products
5.2.12.B.3 Balance chemical equations by applying the law of conservation of mass.
Motivation:
Development:
Solutions Chapter 11 power point presentation
Summary/Assessment:
Homework
27,29, 30 (a-d),31,32,79
Riar: A.P Chemistry
UNIT 7: Solutions Chapter 11
Learning Objectives:
 Students will be able to:
Define, compare and contrast, classify, differentiate, put in order, predict using, identify correct
and incorrect examples of, identify correct and incorrect interpretations of, identify correct and
incorrect applications of…the following terms:
Solution, crystallization, soluble, insoluble, miscible , immiscible, solubility, saturated solution,
unsaturated solution, supers Work Henry’s Law problems








Define molarity and describe how to make a solution of a given molarity
Define mass percentage of solute and describe how to make a solution of a given mass
percentage of solute
Define molality and describe how to make a solution of a given molality
Define mole fraction and describe how to make a solution of a given mole fraction
Convert percent to mole fraction
Convert molality and mole fraction
Convert molality and molarity
Saturated solution, molarity, mass percentage of solute, molality, mole fraction,
Henry’s Law
NJCCC standards addressed:
5.2.12.A.5 Describe the process by which solutes dissolve in solvents.
5.2.2.A.1 Sort and describe objects based on the materials of which they are made and their physical
properties.
5.2.8.A.1 Explain that all matter is made of atoms, and give examples of common elements
5.2.8.A.2 Analyze and explain the implications of the statement “all substances are composed of
elements.”
5.2.6.B.1 Compare the properties of reactants with the properties of the products when two or more
substances are combined and reaction
5.2.8.B.1 Explain, using an understanding of the concept of chemical change, why the mass of reactants
and the mass of products
5.2.12.B.3 Balance chemical equations by applying the law of conservation of mass.
Motivation:
Development:
Solutions Chapter 11 power point presentation
Summary/Assessment:
Homework
27,29, 30 (a-d),31,32,79, 35,38,39,41,43
Riar: A.P Chemistry
UNIT 7: Solutions Chapter 10& 11
Learning Objectives:

Students will be able to:
Define, compare and contrast, classify, differentiate, put in order, predict using, identify correct
and incorrect examples of, identify correct and incorrect interpretations of, identify correct and
incorrect applications of…the following terms:
colligative property, vapor pressure lowering, Raoult’s Law, boiling point elevation,
freezing point depression, osmosis, osmotic pressure ,van’t Hoff factor





Do vapor pressure lowering and Raoult’s Law problems
Do boiling point elevation problems
Do freezing point depression problems
Use freezing point depression to determine molecular weight and molecular formula
Do osmotic pressure problems
 Work colligative property problems for ionic solutions
NJCCC standards addressed:
5.2.12.A.5 Describe the process by which solutes dissolve in solvents.
5.2.2.A.1 Sort and describe objects based on the materials of which they are made and their physical
properties.
5.2.8.A.1 Explain that all matter is made of atoms, and give examples of common elements
5.2.8.A.2 Analyze and explain the implications of the statement “all substances are composed of
elements.”
5.2.6.B.1 Compare the properties of reactants with the properties of the products when two or more
substances are combined and reaction
5.2.8.B.1 Explain, using an understanding of the concept of chemical change, why the mass of reactants
and the mass of products
5.2.12.B.3 Balance chemical equations by applying the law of conservation of mass.
Motivation:
Development:
Solutions Chapter 11 power point presentation
Summary/Assessment:
Homework
47,49,51,55,56,57,58
Riar: A.P Chemistry
UNIT 7: Solutions Chapter 11
Learning Objectives:
 Students will be able to:
 Determine Freezing temperature of a pure solvent, Lauric Acid
 Determine Freezing temperature of a mixture of lauric Acid and benzoic acid
 Calculate the freezing point depression of the mixture
 Calculate the molecular weight of benzoic acid.
NJCCC standards addressed:
5.2.12.A.5 Describe the process by which solutes dissolve in solvents.
5.2.2.A.1 Sort and describe objects based on the materials of which they are made and their physical
properties.
5.2.8.A.1 Explain that all matter is made of atoms, and give examples of common elements
5.2.8.A.2 Analyze and explain the implications of the statement “all substances are composed of
elements.”
5.2.6.B.1 Compare the properties of reactants with the properties of the products when two or more
substances are combined and reaction
5.2.8.B.1 Explain, using an understanding of the concept of chemical change, why the mass of reactants
and the mass of products
5.2.12.B.3 Balance chemical equations by applying the law of conservation of mass.
Motivation:
ASK STUDENTS HOW CAN THE MOLECULAR WEIGHT OF AN UNKNOWN SOLUTE
BE DETERMINED BY USING FREEZING POINT DEPRESSION
Development:
Students will perform the procedure of the Using freezing point depression to find molecular
weight lab
Students will use their collect data to calculate the molecular mass of the unknown solute
Students will plot a graph of their collected data to determine the freezing temperature of a
mixture of lauric Acid and benzoic acid
Students will calculate the freezing point depression of the mixture
Summary/Assessment:
Discuss Lab results and compare class results
Homework
Complete lab write up due
Riar: A.P Chemistry
UNIT 7: Solutions Chapter 11
Learning Objectives:

Students will be able to:
Define, compare and contrast, classify, differentiate, put in order, predict using, identify correct
and incorrect examples of, identify correct and incorrect interpretations of, identify correct and
incorrect applications of…the following terms:
colligative property, vapor pressure lowering, Raoult’s Law, boiling point elevation,
freezing point depression, osmosis, osmotic pressure ,van’t Hoff factor






Do vapor pressure lowering and Raoult’s Law problems
Do boiling point elevation problems
Do freezing point depression problems
Use freezing point depression to determine molecular weight and molecular formula
Do osmotic pressure problems
Work colligative property problems for ionic solutions
NJCCC standards addressed:
5.2.12.A.5 Describe the process by which solutes dissolve in solvents.
5.2.2.A.1 Sort and describe objects based on the materials of which they are made and their physical
properties.
5.2.8.A.1 Explain that all matter is made of atoms, and give examples of common elements
5.2.8.A.2 Analyze and explain the implications of the statement “all substances are composed of
elements.”
5.2.6.B.1 Compare the properties of reactants with the properties of the products when two or more
substances are combined and reaction
5.2.8.B.1 Explain, using an understanding of the concept of chemical change, why the mass of reactants
and the mass of products
5.2.12.B.3 Balance chemical equations by applying the law of conservation of mass.
Motivation:
Development:
Solutions Chapter 11 power point presentation
Summary/Assessment:
Homework
59,61,62,63,64,65,66,71,72,73,85
Riar: A.P Chemistry
UNIT 7: Solutions Chapter 11
Learning Objectives:

Students will be able to:
Define, compare and contrast, classify, differentiate, put in order, predict using, identify correct
and incorrect examples of, identify correct and incorrect interpretations of, identify correct and
incorrect applications of…the following terms:
colligative property, vapor pressure lowering, Raoult’s Law, boiling point elevation,
freezing point depression, osmosis, osmotic pressure ,van’t Hoff factor






Do vapor pressure lowering and Raoult’s Law problems
Do boiling point elevation problems
Do freezing point depression problems
Use freezing point depression to determine molecular weight and molecular formula
Do osmotic pressure problems
Work colligative property problems for ionic solutions
NJCCC standards addressed:
5.2.12.A.5 Describe the process by which solutes dissolve in solvents.
5.2.2.A.1 Sort and describe objects based on the materials of which they are made and their physical
properties.
5.2.8.A.1 Explain that all matter is made of atoms, and give examples of common elements
5.2.8.A.2 Analyze and explain the implications of the statement “all substances are composed of
elements.”
5.2.6.B.1 Compare the properties of reactants with the properties of the products when two or more
substances are combined and reaction
5.2.8.B.1 Explain, using an understanding of the concept of chemical change, why the mass of reactants
and the mass of products
5.2.12.B.3 Balance chemical equations by applying the law of conservation of mass.
Motivation:
Development:
Solutions Chapter 11 power point presentation
Summary/Assessment:
Homework
Take Home solutions test due
Review for Solutions Test
Riar: A.P Chemistry
UNIT 8: Kinetics Chapter 12
Learning Objectives:







Students will be able to:
Define chemical kinetics, reaction rate, average rate, instantaneous rate, rate constant,
rate law, reaction order
Analyze and apply the factors that affect reaction rate
Relate the rate of disappearance of a reactant and the rate of appearance of a product
from the balanced equation
Determine the average reaction rate from concentration measurements at specific
times
Give the reaction order with respect to each reactant and give the overall reaction
order for a reaction when given its rate law
Determine the rate law from initial concentrations and initial rates
NJCCC standards addressed:
5.2.12.A.5 Describe the process by which solutes dissolve in solvents.
5.2.2.A.1 Sort and describe objects based on the materials of which they are made and their physical
properties.
5.2.8.A.1 Explain that all matter is made of atoms, and give examples of common elements
5.2.8.A.2 Analyze and explain the implications of the statement “all substances are composed of
elements.”
5.2.6.B.1 Compare the properties of reactants with the properties of the products when two or more
substances are combined and reaction
5.2.8.B.1 Explain, using an understanding of the concept of chemical change, why the mass of reactants
and the mass of products
5.2.12.B.3 Balance chemical equations by applying the law of conservation of mass.
Motivation:
ASK STUDENTS –WHAT ARE SPONTANEOUS REACTIONS?
HOW DO WE MEASURE THE RATE OF A REACTION?
Development:
Kinetics Chapter 12 Power point
Summary/Assessment:
Homework
Section 1 – 19, 20, 21, 22, 23, 25, 27, 63, 71
Riar: A.P Chemistry
UNIT 8: Kinetics Chapter 12
Learning Objectives:







Students will be able to:
Define catalyst, inhibitor, homogeneous catalysis, heterogeneous catalysis,
enzyme catalysis, active site ,substrate
Analyze and apply the factors that affect reaction rate
Relate the rate of disappearance of a reactant and the rate of appearance of a product
from the balanced equation
Determine the average reaction rate from concentration measurements at specific
times
Give the reaction order with respect to each reactant and give the overall reaction
order for a reaction when given its rate law
Determine the rate law from initial concentrations and initial rates
NJCCC standards addressed:
5.2.12.A.5 Describe the process by which solutes dissolve in solvents.
5.2.2.A.1 Sort and describe objects based on the materials of which they are made and their physical
properties.
5.2.8.A.1 Explain that all matter is made of atoms, and give examples of common elements
5.2.8.A.2 Analyze and explain the implications of the statement “all substances are composed of
elements.”
5.2.6.B.1 Compare the properties of reactants with the properties of the products when two or more
substances are combined and reaction
5.2.8.B.1 Explain, using an understanding of the concept of chemical change, why the mass of reactants
and the mass of products
5.2.12.B.3 Balance chemical equations by applying the law of conservation of mass.
Motivation:
ASK STUDENTS –WHAT ARE SPONTANEOUS REACTIONS?
HOW DO WE MEASURE THE RATE OF A REACTION?
Development:
Kinetics Chapter 12 Power point
Summary/Assessment:
Homework
Section 1 – 19, 20, 21, 22, 23, 25, 27, 63, 71
Riar: A.P Chemistry
UNIT 8: Kinetics Chapter 12
Learning Objectives:





Students will be able to:
Define chemical kinetics, reaction rate, average rate, instantaneous rate, rate constant,
rate law, reaction order, half life
Work rate problems using concentration-time laws for both first order and second
order reactions
Calculate half-lives for both first order and second order reactions
Use graphing to determine the order of a reaction
NJCCC standards addressed:
5.2.12.A.5 Describe the process by which solutes dissolve in solvents.
5.2.2.A.1 Sort and describe objects based on the materials of which they are made and their physical
properties.
5.2.8.A.1 Explain that all matter is made of atoms, and give examples of common elements
5.2.8.A.2 Analyze and explain the implications of the statement “all substances are composed of
elements.”
5.2.6.B.1 Compare the properties of reactants with the properties of the products when two or more
substances are combined and reaction
5.2.8.B.1 Explain, using an understanding of the concept of chemical change, why the mass of reactants
and the mass of products
5.2.12.B.3 Balance chemical equations by applying the law of conservation of mass.
Motivation:
ASK STUDENTS –WHAT ARE SPONTANEOUS REACTIONS?
HOW DO WE MEASURE THE RATE OF A REACTION?
Development:
Kinetics Chapter 12 Power point
Summary/Assessment:
Homework
Section 2 – 29,30,31,32,33,35,37,38,39,41,43,65,73
Riar: A.P Chemistry
UNIT 8: Kinetics Chapter 12
Learning Objectives:





Students will be able to:
Define chemical kinetics, reaction rate, average rate, instantaneous rate, rate constant,
rate law, reaction order, half life
Work rate problems using concentration-time laws for both first order and second
order reactions
Calculate half-lives for both first order and second order reactions
Use graphing to determine the order of a reaction
NJCCC standards addressed:
5.2.12.A.5 Describe the process by which solutes dissolve in solvents.
5.2.2.A.1 Sort and describe objects based on the materials of which they are made and their physical
properties.
5.2.8.A.1 Explain that all matter is made of atoms, and give examples of common elements
5.2.8.A.2 Analyze and explain the implications of the statement “all substances are composed of
elements.”
5.2.6.B.1 Compare the properties of reactants with the properties of the products when two or more
substances are combined and reaction
5.2.8.B.1 Explain, using an understanding of the concept of chemical change, why the mass of reactants
and the mass of products
5.2.12.B.3 Balance chemical equations by applying the law of conservation of mass.
Motivation:
ASK STUDENTS –WHAT ARE SPONTANEOUS REACTIONS?
HOW DO WE MEASURE THE RATE OF A REACTION?
Development:
Kinetics Chapter 12 Power point
Summary/Assessment:
Homework
Section 2 – 29,30,31,32,33,35,37,38,39,41,43,65,73
Riar: A.P Chemistry
UNIT 8: Kinetics Chapter 12
Learning Objectives:







Students will be able to:
Define -reaction mechanism, elementary step, reaction intermediate
molecularity, unimolecular, bimolecular, termolecular
Describe reaction mechanisms in terms of elementary steps, reaction intermediates,
and molecularity
Write the overall balanced equation from the mechanism
Write rate laws for elementary steps
Write rate laws from mechanisms
Determine the rate-determining step from the rate law
NJCCC standards addressed:
5.2.12.A.5 Describe the process by which solutes dissolve in solvents.
5.2.2.A.1 Sort and describe objects based on the materials of which they are made and their physical
properties.
5.2.8.A.1 Explain that all matter is made of atoms, and give examples of common elements
5.2.8.A.2 Analyze and explain the implications of the statement “all substances are composed of
elements.”
5.2.6.B.1 Compare the properties of reactants with the properties of the products when two or more
substances are combined and reaction
5.2.8.B.1 Explain, using an understanding of the concept of chemical change, why the mass of reactants
and the mass of products
5.2.12.B.3 Balance chemical equations by applying the law of conservation of mass.
Motivation:
ASK STUDENTS –WHAT ARE SPONTANEOUS REACTIONS?
HOW DO WE MEASURE THE RATE OF A REACTION?
Development:
Kinetics Chapter 12 Power point
Summary/Assessment:
Homework
Section 3 – 45,47,48, 68, 69, 74
Riar: A.P Chemistry
UNIT 8: Kinetics Chapter 12
Learning Objectives:







Students will be able to:
Define - collision theory, activation energy ,activated complex collision theory,
Arrhenius equation
Use collision theory and energy considerations to explain reactions and reaction rates
Explain reactions and reaction rates using potential energy profiles, including
activation energy and the activated complex
Use collision theory and energy considerations to explain the effect of temperature,
surface area, concentration, and the presence or absence of a catalyst on reaction rates
Use the Arrhenius equation to describe the relationship among activation energy,
temperature, frequency of collisions, and the rate law constant and to calculate these
values
Describe the nature of a catalyst and catalysis, including enzyme catalysis
NJCCC standards addressed:
5.2.12.A.5 Describe the process by which solutes dissolve in solvents.
5.2.2.A.1 Sort and describe objects based on the materials of which they are made and their physical
properties.
5.2.8.A.1 Explain that all matter is made of atoms, and give examples of common elements
5.2.8.A.2 Analyze and explain the implications of the statement “all substances are composed of
elements.”
5.2.6.B.1 Compare the properties of reactants with the properties of the products when two or more
substances are combined and reaction
5.2.8.B.1 Explain, using an understanding of the concept of chemical change, why the mass of reactants
and the mass of products
5.2.12.B.3 Balance chemical equations by applying the law of conservation of mass.
Motivation:
ASK STUDENTS –WHAT ARE SPONTANEOUS REACTIONS?
HOW DO WE MEASURE THE RATE OF A REACTION?
Development:
Kinetics Chapter 12 Power point
Summary/Assessment:
Homework
Review Kinetics
Kinetics take home test due
Riar: A.P Chemistry
UNIT 8: Kinetics Chapter 12
Learning Objectives:







Students will be able to:
Define chemical kinetics, reaction rate, average rate, instantaneous rate, rate constant,
rate law, reaction order
Analyze and apply the factors that affect reaction rate
Relate the rate of disappearance of a reactant and the rate of appearance of a product
from the balanced equation
Determine the average reaction rate from concentration measurements at specific
times
Give the reaction order with respect to each reactant and give the overall reaction
order for a reaction when given its rate law
Determine the rate law from initial concentrations and initial rates
NJCCC standards addressed:
5.2.12.A.5 Describe the process by which solutes dissolve in solvents.
5.2.2.A.1 Sort and describe objects based on the materials of which they are made and their physical
properties.
5.2.8.A.1 Explain that all matter is made of atoms, and give examples of common elements
5.2.8.A.2 Analyze and explain the implications of the statement “all substances are composed of
elements.”
5.2.6.B.1 Compare the properties of reactants with the properties of the products when two or more
substances are combined and reaction
5.2.8.B.1 Explain, using an understanding of the concept of chemical change, why the mass of reactants
and the mass of products
5.2.12.B.3 Balance chemical equations by applying the law of conservation of mass.
Motivation:
ASK STUDENTS –WHAT ARE SPONTANEOUS REACTIONS?
HOW DO WE MEASURE THE RATE OF A REACTION?
Development:
Kinetics Chapter 12 Power point
Summary/Assessment:
Homework
Kinetics take home test due Kinetics Test
Midterm Review
Riar: A.P Chemistry
UNIT 9: Equilibrium Chapter 13
Learning Objectives:
 Students will be able to:
 Define reversible reaction, forward reaction, reverse reaction, chemical
equilibrium, dynamic equilibrium, equilibrium position
 Use the equilibrium position of a reaction to determine whether products or
reactants are favored in a reversible reaction
 Write equilibrium constant expressions for homogeneous equilibria, in terms of
partial pressures where all species are gaseous, and for heterogeneous equilibria
 Calculate equilibrium constants from equilibrium concentrations
 Calculate equilibrium constants from stoichiometry
NJCCC standards addressed:
5.2.12.A.5 Describe the process by which solutes dissolve in solvents.
5.2.2.A.1 Sort and describe objects based on the materials of which they are made and their physical
properties.
5.2.8.A.1 Explain that all matter is made of atoms, and give examples of common elements
5.2.8.A.2 Analyze and explain the implications of the statement “all substances are composed of
elements.”
5.2.6.B.1 Compare the properties of reactants with the properties of the products when two or more
substances are combined and reaction
5.2.8.B.1 Explain, using an understanding of the concept of chemical change, why the mass of reactants
and the mass of products
5.2.12.B.3 Balance chemical equations by applying the law of conservation of mass.
Motivation:
ASK STUDENTS – WHAT IS STATE OF EQUILIBRIUM?
WHAT IS DYNAMIC EQUILIBRIUM?
Development:
Equilibrium Chapter 13 Power point
Summary/Assessment:
Homework
Section 1 – 19,21,23,25,27,29,32,33,35,67
Riar: A.P Chemistry
UNIT 9: Equilibrium Chapter 13
Learning Objectives:
 Students will be able to:
 Define I.C.E. (Initial-Change-Equilibrium) table, equilibrium constant (Kc),
homogeneous equilibrium, heterogeneous equilibrium, reaction quotient
(Qc),LeChatelier’s Principle ,catalyst
 Use the equilibrium position of a reaction to determine whether products or
reactants are favored in a reversible reaction
 Apply stoichiometry to equilibrium mixtures
 Set up an I.C.E. (Initial-Change-Equilibrium) table
 Use the magnitude of the equilibrium constant to determine whether the
equilibrium lies to the right or left, and whether products or reactants are favored
 Calculate equilibrium constants from stoichiometry
 Predict the direction of a reaction from the reaction quotient
 Calculate one equilibrium concentration given the others and the equilibrium
constant
 Calculate equilibrium concentrations from initial concentrations and the
equilibrium constant
NJCCC standards addressed:
5.2.12.A.5 Describe the process by which solutes dissolve in solvents.
5.2.2.A.1 Sort and describe objects based on the materials of which they are made and their physical
properties.
5.2.8.A.1 Explain that all matter is made of atoms, and give examples of common elements
5.2.8.A.2 Analyze and explain the implications of the statement “all substances are composed of
elements.”
5.2.6.B.1 Compare the properties of reactants with the properties of the products when two or more
substances are combined and reaction
5.2.8.B.1 Explain, using an understanding of the concept of chemical change, why the mass of reactants
and the mass of products
5.2.12.B.3 Balance chemical equations by applying the law of conservation of mass.
Motivation:
ASK STUDENTS – WHAT IS STATE OF EQUILIBRIUM?
WHAT IS DYNAMIC EQUILIBRIUM?
Development:
Equilibrium Chapter 13 Power point
Summary/Assessment:
Homework
Section 2 – 37,39,40,41,43,45,47,51,53,55,56,57,68,69,71,72,73,77,79,80,81,82,83
Riar: A.P Chemistry
UNIT 9: Equilibrium Chapter 13
Learning Objectives:
 Students will be able to:
 Define I.C.E. (Initial-Change-Equilibrium) table, equilibrium constant (Kc),
homogeneous equilibrium, heterogeneous equilibrium, reaction quotient
(Qc),LeChatelier’s Principle ,catalyst
 Use the equilibrium position of a reaction to determine whether products or
reactants are favored in a reversible reaction
 Apply stoichiometry to equilibrium mixtures
 Set up an I.C.E. (Initial-Change-Equilibrium) table
 Use the magnitude of the equilibrium constant to determine whether the
equilibrium lies to the right or left, and whether products or reactants are favored
 Calculate equilibrium constants from stoichiometry
 Predict the direction of a reaction from the reaction quotient
 Calculate one equilibrium concentration given the others and the equilibrium
constant
 Calculate equilibrium concentrations from initial concentrations and the
equilibrium constant
NJCCC standards addressed:
5.2.12.A.5 Describe the process by which solutes dissolve in solvents.
5.2.2.A.1 Sort and describe objects based on the materials of which they are made and their physical
properties.
5.2.8.A.1 Explain that all matter is made of atoms, and give examples of common elements
5.2.8.A.2 Analyze and explain the implications of the statement “all substances are composed of
elements.”
5.2.6.B.1 Compare the properties of reactants with the properties of the products when two or more
substances are combined and reaction
5.2.8.B.1 Explain, using an understanding of the concept of chemical change, why the mass of reactants
and the mass of products
5.2.12.B.3 Balance chemical equations by applying the law of conservation of mass.
Motivation:
ASK STUDENTS – WHAT IS STATE OF EQUILIBRIUM?
WHAT IS DYNAMIC EQUILIBRIUM?
Development:
Equilibrium Chapter 13 Power point
Summary/Assessment:
Homework
Section 2 – 37,39,40,41,43,45,47,51,53,55,56,57,68,69,71,72,73,77,79,80,81,82,83
Riar: A.P Chemistry
UNIT 9: Equilibrium Chapter 13
Learning Objectives:
 Students will be able to:
 Define I.C.E. (Initial-Change-Equilibrium) table, equilibrium constant (Kc),
homogeneous equilibrium, heterogeneous equilibrium, reaction quotient
(Qc),LeChatelier’s Principle ,catalyst
 Use the equilibrium position of a reaction to determine whether products or
reactants are favored in a reversible reaction
 Apply stoichiometry to equilibrium mixtures
 Set up an I.C.E. (Initial-Change-Equilibrium) table
 Use the magnitude of the equilibrium constant to determine whether the
equilibrium lies to the right or left, and whether products or reactants are favored
 Calculate equilibrium constants from stoichiometry
 Predict the direction of a reaction from the reaction quotient
 Calculate one equilibrium concentration given the others and the equilibrium
constant
 Calculate equilibrium concentrations from initial concentrations and the
equilibrium constant
NJCCC standards addressed:
5.2.12.A.5 Describe the process by which solutes dissolve in solvents.
5.2.2.A.1 Sort and describe objects based on the materials of which they are made and their physical
properties.
5.2.8.A.1 Explain that all matter is made of atoms, and give examples of common elements
5.2.8.A.2 Analyze and explain the implications of the statement “all substances are composed of
elements.”
5.2.6.B.1 Compare the properties of reactants with the properties of the products when two or more
substances are combined and reaction
5.2.8.B.1 Explain, using an understanding of the concept of chemical change, why the mass of reactants
and the mass of products
5.2.12.B.3 Balance chemical equations by applying the law of conservation of mass.
Motivation:
ASK STUDENTS – WHAT IS STATE OF EQUILIBRIUM?
WHAT IS DYNAMIC EQUILIBRIUM?
Development:
Equilibrium Chapter 13 Power point
Summary/Assessment:
Homework
Section 2 – 37,39,40,41,43,45,47,51,53,55,56,57,68,69,71,72,73,77,79,80,81,82,83
Riar: A.P Chemistry
UNIT 9: Equilibrium Chapter 13
Learning Objectives:
 Students will be able to:
 Apply LeChatelier’s Principle to changes in concentration, changes in
temperature, and changes in pressure
 Explain how catalysts work and their effect on activation energy, rate of reaction,
the composition of a reaction mixture, the value of the equilibrium constant, and the
rate at which equilibrium is reached
NJCCC standards addressed:
5.2.12.A.5 Describe the process by which solutes dissolve in solvents.
5.2.2.A.1 Sort and describe objects based on the materials of which they are made and their physical
properties.
5.2.8.A.1 Explain that all matter is made of atoms, and give examples of common elements
5.2.8.A.2 Analyze and explain the implications of the statement “all substances are composed of
elements.”
5.2.6.B.1 Compare the properties of reactants with the properties of the products when two or more
substances are combined and reaction
5.2.8.B.1 Explain, using an understanding of the concept of chemical change, why the mass of reactants
and the mass of products
5.2.12.B.3 Balance chemical equations by applying the law of conservation of mass.
Motivation:
ASK STUDENTS – WHAT IS STATE OF EQUILIBRIUM?
WHAT IS DYNAMIC EQUILIBRIUM?
Development:
Equilibrium Chapter 13 Power point
Summary/Assessment:
Homework
Section 3 – 59,61,63,65,66,75,74
Additional Problems from old A.P Exams
Test Equilibrium
Riar: A.P Chemistry
UNIT 10: Acids & Bases Chapter 14
Learning Objectives:
 Students will be able to:
 Define acid, base ,Arrhenius acid, Arrhenius base, strong acid, weak base,
Brønstead-Lowry acid, Brønstead-Lowry base, conjugate acid, conjugate base, Lewis
acid, Lewis base, autoionization, pH, pOH
 Identify the properties of acids and bases
 Identify strong acids and strong bases
 Describe the unique quality of the hydrogen ion in water that makes it different
from all other aqueous cations
 Discuss the evidence for the Arrhenius theory
 Discuss the drawbacks to the Arrhenius theory, how the Brønstead-Lowry
concept developed as a result of these drawbacks Write the formulas for conjugate
acids and conjugate bases
 Identify conjugate acids and bases
NJCCC standards addressed:
5.2.12.A.5 Describe the process by which solutes dissolve in solvents.
5.2.2.A.1 Sort and describe objects based on the materials of which they are made and their physical
properties.
5.2.8.A.1 Explain that all matter is made of atoms, and give examples of common elements
5.2.8.A.2 Analyze and explain the implications of the statement “all substances are composed of
elements.”
5.2.6.B.1 Compare the properties of reactants with the properties of the products when two or more
substances are combined and reaction
5.2.8.B.1 Explain, using an understanding of the concept of chemical change, why the mass of reactants
and the mass of products
5.2.12.B.3 Balance chemical equations by applying the law of conservation of mass.
Motivation:
ASK STUDENTS – WHAT ARE ACIDS AND BASES
WHAT ARE SOME PROPERTIES OF ACIDS AND BASES?
Development:
Acids And Bases Chapter 14 Power point
Summary/Assessment
Homework
Section 2 – 25, 26 , 27, 29,31, 32, 33, 34, 13
Riar: A.P Chemistry
UNIT 10: Acids & Bases Chapter 14
Learning Objectives:
 Students will be able to:
 Define acid, base ,Arrhenius acid, Arrhenius base, strong acid, weak base,
Brønstead-Lowry acid, Brønstead-Lowry base, conjugate acid, conjugate base, Lewis
acid, Lewis base, autoionization, ion-product constant for water
pH, pOH
 Give the relationship between [H+] and Arrhenius definitions of acids and bases
 Calculate the concentrations of H+ and OH for aqueous solutions of strong acids
or strong bases
 Give the relationship between pH and pOH and Arrhenius definitions of acids and
bases
 Calculate pH and pOH from molar concentrations
 Calculate [H+] and [OH] from pH and pOH
NJCCC standards addressed:
5.2.12.A.5 Describe the process by which solutes dissolve in solvents.
5.2.2.A.1 Sort and describe objects based on the materials of which they are made and their physical
properties.
5.2.8.A.1 Explain that all matter is made of atoms, and give examples of common elements
5.2.8.A.2 Analyze and explain the implications of the statement “all substances are composed of
elements.”
5.2.6.B.1 Compare the properties of reactants with the properties of the products when two or more
substances are combined and reaction
5.2.8.B.1 Explain, using an understanding of the concept of chemical change, why the mass of reactants
and the mass of products
5.2.12.B.3 Balance chemical equations by applying the law of conservation of mass.
Motivation:
ASK STUDENTS – WHAT ARE ACIDS AND BASES?
WHAT ARE SOME PROPERTIES OF ACIDS AND BASES?
Development:
Acids And Bases Chapter 14 Power point
Summary/Assessment:
Homework
Section 3– 35,36,37,38,40,41,43,45,47,49,50,51
Riar: A.P Chemistry
UNIT 10: Acids & Bases Chapter 14
Learning Objectives:
 Students will be able to:
 Define acid, base ,Arrhenius acid, Arrhenius base, strong acid, weak base,
Brønstead-Lowry acid, Brønstead-Lowry base, conjugate acid, conjugate base, Lewis
acid, Lewis base, autoionization, ion-product constant for water
pH, pOH
 Use the approximation method for calculating the concentrations of species in a
weak acid solution using Ka
 Use the quadratic formula to calculate the concentrations of species in a weak
acid solution using Ka
 Calculate Ka using pH
 Calculate percent ionization for a weak acid given the initial concentration and the
pH or given the initial concentration and the Ka
 Calculate pH of weak acids from their % dissociation
 Understand the table of relative strengths of acids and Bases
NJCCC standards addressed:
5.2.12.A.5 Describe the process by which solutes dissolve in solvents.
5.2.2.A.1 Sort and describe objects based on the materials of which they are made and their physical
properties.
5.2.8.A.1 Explain that all matter is made of atoms, and give examples of common elements
5.2.8.A.2 Analyze and explain the implications of the statement “all substances are composed of
elements.”
5.2.6.B.1 Compare the properties of reactants with the properties of the products when two or more
substances are combined and reaction
5.2.8.B.1 Explain, using an understanding of the concept of chemical change, why the mass of reactants
and the mass of products
5.2.12.B.3 Balance chemical equations by applying the law of conservation of mass.
Motivation:
ASK STUDENTS – WHAT ARE ACIDS AND BASES?
WHAT ARE SOME PROPERTIES OF ACIDS AND BASES?
Development:
Acids And Bases Chapter 14 Power point
Summary/Assessment:
Homework
Section 4– 53,55,57,58,59,61,63,65,66,67,69,71,73,74,131,144,145
Riar: A.P Chemistry
UNIT 10: Acids & Bases Chapter 14
Learning Objectives:
 Students will be able to:
 Define acid, base ,Arrhenius acid, Arrhenius base, strong acid, weak base,
Brønstead-Lowry acid, Brønstead-Lowry base, conjugate acid, conjugate base, Lewis
acid, Lewis base, autoionization, ion-product constant for water
pH, pOH
 Calculate pH of strong Bases
 Use the approximation method for calculating the concentrations of species in a
weak base solution using Kb
 Use the quadratic formula to calculate the concentrations of species in a weak
base solution using Kb
 Use the relative strengths of acids and bases to predict whether reactants or
products are favored for a reaction
 Calculate the Kb for the conjugate base of an acid
NJCCC standards addressed:
5.2.12.A.5 Describe the process by which solutes dissolve in solvents.
5.2.2.A.1 Sort and describe objects based on the materials of which they are made and their physical
properties.
5.2.8.A.1 Explain that all matter is made of atoms, and give examples of common elements
5.2.8.A.2 Analyze and explain the implications of the statement “all substances are composed of
elements.”
5.2.6.B.1 Compare the properties of reactants with the properties of the products when two or more
substances are combined and reaction
5.2.8.B.1 Explain, using an understanding of the concept of chemical change, why the mass of reactants
and the mass of products
5.2.12.B.3 Balance chemical equations by applying the law of conservation of mass.
Motivation:
ASK STUDENTS – WHAT ARE ACIDS AND BASES?
WHAT ARE SOME PROPERTIES OF ACIDS AND BASES?
Development:
Acids And Bases Chapter 14 Power point
Summary/Assessment:
Homework
Section 5 – 75,76,77,78,79,80,81,83,84,85,87,89,95
Riar: A.P Chemistry
UNIT 10: Acids & Bases Chapter 14
Learning Objectives:
 Students will be able to:
 Define acid ionization constant – Ka, percent ionization, base ionization constant –
Kb, conjugate acid, conjugate base, salt hydrolysis
 Calculate [H+] and pH for polyprotic acids
 Use bond strength and bond polarity to explain the trend in acid strength for
binary acids
 Use electronegativity and the number of O atoms bonded to the central atom to
explain the trend in acid strength for oxyacids
 Explain the trend in acid strength for polyprotic acids and their corresponding
acid anions
 Use salt hydrolysis to predict whether a salt solution will be acidic, basic, or
neutral
 Calculate the pH of salt solutions
 Explain the common ion effect
 Perform calculations involving the common ion effect
NJCCC standards addressed:
5.2.12.A.5 Describe the process by which solutes dissolve in solvents.
5.2.2.A.1 Sort and describe objects based on the materials of which they are made and their physical
properties.
5.2.8.A.1 Explain that all matter is made of atoms, and give examples of common elements
5.2.8.A.2 Analyze and explain the implications of the statement “all substances are composed of
elements.”
5.2.6.B.1 Compare the properties of reactants with the properties of the products when two or more
substances are combined and reaction
5.2.8.B.1 Explain, using an understanding of the concept of chemical change, why the mass of reactants
and the mass of products
5.2.12.B.3 Balance chemical equations by applying the law of conservation of mass.
Motivation:
ASK STUDENTS – WHAT ARE ACIDS AND BASES?
WHAT ARE SOME PROPERTIES OF ACIDS AND BASES?
Development:
Acids And Bases Chapter 14 Power point
Summary/Assessment:
Homework
A.P Exam Acid / Base Free response questions
TEST ACIDS AND BASES
Riar: A.P Chemistry
UNIT 11: Acids & Bases Equilibria Chapter 15PartI
Learning Objectives:












Students will be able to:
Define common ion effect, buffer (or buffered solution) ,Henderson-Hasselbalch
equation, acid-base titration, equivalence point, end point, indicator, titration curve
Explain the common ion effect
Perform calculations involving the common ion effect
Perform calculations involving the common ion effect
Describe how to make a buffer
Explain how a buffer works
Identify solutions that are buffers and those that are not
Derive the Henderson-Hasselbalch equation
Calculate the pH of the initial buffer solution
Calculate the pH of a buffer solution after the addition of acid or base to that solution
Perform the calculations for making a buffer solution of a specified pH
NJCCC standards addressed:
5.2.12.A.5 Describe the process by which solutes dissolve in solvents.
5.2.2.A.1 Sort and describe objects based on the materials of which they are made and their physical
properties.
5.2.8.A.1 Explain that all matter is made of atoms, and give examples of common elements
5.2.8.A.2 Analyze and explain the implications of the statement “all substances are composed of
elements.”
5.2.6.B.1 Compare the properties of reactants with the properties of the products when two or more
substances are combined and reaction
5.2.8.B.1 Explain, using an understanding of the concept of chemical change, why the mass of reactants
and the mass of products
5.2.12.B.3 Balance chemical equations by applying the law of conservation of mass.
Motivation:
ASK STUDENTS – WHAT IS A COMMON ION?
WHAT ARE BUFFERS?
Development:
Acids And Bases Chapter 15 Power point
Summary/Assessment:
Homework
Section 1- 21,22,23,25,27,29,31,33,35,37
Riar: A.P Chemistry
UNIT 11: Acids & Bases Equilibria Chapter 15PartI
Learning Objectives:












Students will be able to:
Define common ion effect, buffer (or buffered solution) ,Henderson-Hasselbalch
equation, acid-base titration, equivalence point, end point, indicator, titration curve
Explain the common ion effect
Perform calculations involving the common ion effect
Perform calculations involving the common ion effect
Describe how to make a buffer
Explain how a buffer works
Identify solutions that are buffers and those that are not
Derive the Henderson-Hasselbalch equation
Calculate the pH of the initial buffer solution
Calculate the pH of a buffer solution after the addition of acid or base to that solution
Perform the calculations for making a buffer solution of a specified pH
NJCCC standards addressed:
5.2.12.A.5 Describe the process by which solutes dissolve in solvents.
5.2.2.A.1 Sort and describe objects based on the materials of which they are made and their physical
properties.
5.2.8.A.1 Explain that all matter is made of atoms, and give examples of common elements
5.2.8.A.2 Analyze and explain the implications of the statement “all substances are composed of
elements.”
5.2.6.B.1 Compare the properties of reactants with the properties of the products when two or more
substances are combined and reaction
5.2.8.B.1 Explain, using an understanding of the concept of chemical change, why the mass of reactants
and the mass of products
5.2.12.B.3 Balance chemical equations by applying the law of conservation of mass.
Motivation:
ASK STUDENTS – WHAT ARE BUFFERS?
Development:
Acids And Bases Chapter 15 Power point
Summary/Assessment:
Homework
Section 2- 41,43,45,46,47,48,50,51,52,53,54,113,114,115,116
Riar: A.P Chemistry
UNIT 11: Acids & Bases Equilibria Chapter 15PartI
Learning Objectives:





Students will be able to:
Define common ion effect, buffer (or buffered solution) ,Henderson-Hasselbalch
equation, acid-base titration, equivalence point, end point, indicator, titration curve
Describe and explain the shape of the three types of titration curves as well as
explaining the pH of the equivalence point
Calculate the pH after the addition of a given amount of acid or base in a titration
Calculate the pH at the equivalence point for a titration
NJCCC standards addressed:
5.2.12.A.5 Describe the process by which solutes dissolve in solvents.
5.2.2.A.1 Sort and describe objects based on the materials of which they are made and their physical
properties.
5.2.8.A.1 Explain that all matter is made of atoms, and give examples of common elements
5.2.8.A.2 Analyze and explain the implications of the statement “all substances are composed of
elements.”
5.2.6.B.1 Compare the properties of reactants with the properties of the products when two or more
substances are combined and reaction
5.2.8.B.1 Explain, using an understanding of the concept of chemical change, why the mass of reactants
and the mass of products
5.2.12.B.3 Balance chemical equations by applying the law of conservation of mass.
Motivation:
ASK STUDENTS – WHAT IS A TITRATION?
WHAT IS EQUIVALENCE POINT?
WHAT IS AN END POINT?
Development:
Acids And Bases Chapter 15 Power point
Summary/Assessment:
Homework
Section 3- 55,56,57,59,61,63,65,68,118,119,121,126
Riar: A.P Chemistry
UNIT 11: Acids & Bases Equilibria Chapter 15PartI
Learning Objectives:





Students will be able to:
Define common ion effect, buffer (or buffered solution) ,Henderson-Hasselbalch
equation, acid-base titration, equivalence point, end point, indicator, titration curve
Describe and explain the shape of the three types of titration curves as well as
explaining the pH of the equivalence point
Calculate the pH after the addition of a given amount of acid or base in a titration
Calculate the pH at the equivalence point for a titration
NJCCC standards addressed:
5.2.12.A.5 Describe the process by which solutes dissolve in solvents.
5.2.2.A.1 Sort and describe objects based on the materials of which they are made and their physical
properties.
5.2.8.A.1 Explain that all matter is made of atoms, and give examples of common elements
5.2.8.A.2 Analyze and explain the implications of the statement “all substances are composed of
elements.”
5.2.6.B.1 Compare the properties of reactants with the properties of the products when two or more
substances are combined and reaction
5.2.8.B.1 Explain, using an understanding of the concept of chemical change, why the mass of reactants
and the mass of products
5.2.12.B.3 Balance chemical equations by applying the law of conservation of mass.
Motivation:
ASK STUDENTS – WHAT IS A TITRATION?
WHAT IS EQUIVALENCE POINT?
WHAT IS AN END POINT?
Development:
Acids And Bases Chapter 15 Power point
Summary/Assessment:
Homework
Section 3- 55,56,57,59,61,63,65,68,118,119,121,126
Riar: A.P Chemistry
UNIT 11: Acids & Bases Equilibria Chapter 15PartI
Learning Objectives:





Students will be able to:
Define common ion effect, buffer (or buffered solution) ,Henderson-Hasselbalch
equation, acid-base titration, equivalence point, end point, indicator, titration curve
Describe and explain the shape of the three types of titration curves as well as
explaining the pH of the equivalence point
Calculate the pH after the addition of a given amount of acid or base in a titration
Calculate the pH at the equivalence point for a titration
NJCCC standards addressed:
5.2.12.A.5 Describe the process by which solutes dissolve in solvents.
5.2.2.A.1 Sort and describe objects based on the materials of which they are made and their physical
properties.
5.2.8.A.1 Explain that all matter is made of atoms, and give examples of common elements
5.2.8.A.2 Analyze and explain the implications of the statement “all substances are composed of
elements.”
5.2.6.B.1 Compare the properties of reactants with the properties of the products when two or more
substances are combined and reaction
5.2.8.B.1 Explain, using an understanding of the concept of chemical change, why the mass of reactants
and the mass of products
5.2.12.B.3 Balance chemical equations by applying the law of conservation of mass.
Motivation:
ASK STUDENTS – WHAT IS A TITRATION?
WHAT IS EQUIVALENCE POINT?
WHAT IS AN END POINT?
Development:
Acids And Bases Chapter 15 Power point
Summary/Assessment:
Homework
Section 4 – 69,70,71,73,75,77,122,132
Riar: A.P Chemistry
UNIT 11: Acids & Bases Equilibria Chapter 15PartI
Learning Objectives:





Students will be able to:
Define common ion effect, buffer (or buffered solution) ,Henderson-Hasselbalch
equation, acid-base titration, equivalence point, end point, indicator, titration curve
Describe and explain the shape of the three types of titration curves as well as
explaining the pH of the equivalence point
Calculate the pH after the addition of a given amount of acid or base in a titration
Calculate the pH at the equivalence point for a titration
NJCCC standards addressed:
5.2.12.A.5 Describe the process by which solutes dissolve in solvents.
5.2.2.A.1 Sort and describe objects based on the materials of which they are made and their physical
properties.
5.2.8.A.1 Explain that all matter is made of atoms, and give examples of common elements
5.2.8.A.2 Analyze and explain the implications of the statement “all substances are composed of
elements.”
5.2.6.B.1 Compare the properties of reactants with the properties of the products when two or more
substances are combined and reaction
5.2.8.B.1 Explain, using an understanding of the concept of chemical change, why the mass of reactants
and the mass of products
5.2.12.B.3 Balance chemical equations by applying the law of conservation of mass.
Motivation:
ASK STUDENTS – WHAT IS A TITRATION?
WHAT IS EQUIVALENCE POINT?
WHAT IS AN END POINT?
Development:
Acids And Bases Chapter 15 Power point
Summary/Assessment:
Homework
Review for the test
Free response questions
TEST CHAPTER ACID BASE EQUILIBRIA
Riar: A.P Chemistry
UNIT 11: Acids & Bases Equilibria Chapter 15 PartII
Learning Objectives:











Students will be able to: solubility product constant, solubility, molar solubility,
common ion effect, ion product, formation constant – complexes, dissociation
constant – complexes
Write solubility product constant (Ksp) expressions
Determine the Ksp from the solubility of a substance
Determine the solubility of a substance from its Ksp
Perform solubility calculations involving the common ion effect
Write ion product (Qc) expressions
Use ion products to predict precipitation
Recognize when the solubility of a substance will be affected by the pH
Given a set of substances, state which substances will be more soluble in acidic
solutions than in water
Perform equilibrium calculations for the formation of a complex
Calculate the solubility of a slightly soluble salt in a solution of the complex ion
NJCCC standards addressed:
5.2.12.A.5 Describe the process by which solutes dissolve in solvents.
5.2.2.A.1 Sort and describe objects based on the materials of which they are made and their physical
properties.
5.2.8.A.1 Explain that all matter is made of atoms, and give examples of common elements
5.2.8.A.2 Analyze and explain the implications of the statement “all substances are composed of
elements.”
5.2.6.B.1 Compare the properties of reactants with the properties of the products when two or more
substances are combined and reaction
5.2.8.B.1 Explain, using an understanding of the concept of chemical change, why the mass of reactants
and the mass of products
5.2.12.B.3 Balance chemical equations by applying the law of conservation of mass.
Motivation:
ASK STUDENTS –
Development:
Acids And Bases Chapter 15 Power point
Summary/Assessment:
Homework
Section 1- 79,81,83,85,87,89,93,95, 97,98,99,100,101,123,126,
Riar: A.P Chemistry
UNIT 11: Acids & Bases Equilibria Chapter 15
Learning Objectives:











Students will be able to: solubility product constant, solubility, molar solubility,
common ion effect, ion product, formation constant – complexes, dissociation
constant – complexes
Write solubility product constant (Ksp) expressions
Determine the Ksp from the solubility of a substance
Determine the solubility of a substance from its Ksp
Perform solubility calculations involving the common ion effect
Write ion product (Qc) expressions
Use ion products to predict precipitation
Recognize when the solubility of a substance will be affected by the pH
Given a set of substances, state which substances will be more soluble in acidic
solutions than in water
Perform equilibrium calculations for the formation of a complex
Calculate the solubility of a slightly soluble salt in a solution of the complex ion
NJCCC standards addressed:
5.2.12.A.5 Describe the process by which solutes dissolve in solvents.
5.2.2.A.1 Sort and describe objects based on the materials of which they are made and their physical
properties.
5.2.8.A.1 Explain that all matter is made of atoms, and give examples of common elements
5.2.8.A.2 Analyze and explain the implications of the statement “all substances are composed of
elements.”
5.2.6.B.1 Compare the properties of reactants with the properties of the products when two or more
substances are combined and reaction
5.2.8.B.1 Explain, using an understanding of the concept of chemical change, why the mass of reactants
and the mass of products
5.2.12.B.3 Balance chemical equations by applying the law of conservation of mass.
Motivation:
ASK STUDENTS –
Development:
Acids And Bases Chapter 15 Power point
Summary/Assessment:
Homework
103,104,105,106,107,108,109,110,111,112
Riar: A.P Chemistry
UNIT 11: Acids & Bases Equilibria Chapter 15 part II
Learning Objectives:











Students will be able to: solubility product constant, solubility, molar solubility,
common ion effect, ion product, formation constant – complexes, dissociation
constant – complexes
Write solubility product constant (Ksp) expressions
Determine the Ksp from the solubility of a substance
Determine the solubility of a substance from its Ksp
Perform solubility calculations involving the common ion effect
Write ion product (Qc) expressions
Use ion products to predict precipitation
Recognize when the solubility of a substance will be affected by the pH
Given a set of substances, state which substances will be more soluble in acidic
solutions than in water
Perform equilibrium calculations for the formation of a complex
Calculate the solubility of a slightly soluble salt in a solution of the complex ion
NJCCC standards addressed:
5.2.12.A.5 Describe the process by which solutes dissolve in solvents.
5.2.2.A.1 Sort and describe objects based on the materials of which they are made and their physical
properties.
5.2.8.A.1 Explain that all matter is made of atoms, and give examples of common elements
5.2.8.A.2 Analyze and explain the implications of the statement “all substances are composed of
elements.”
5.2.6.B.1 Compare the properties of reactants with the properties of the products when two or more
substances are combined and reaction
5.2.8.B.1 Explain, using an understanding of the concept of chemical change, why the mass of reactants
and the mass of products
5.2.12.B.3 Balance chemical equations by applying the law of conservation of mass.
Motivation:
ASK STUDENTS –
Development:
Acids And Bases Chapter 15 Power point
Summary/Assessment:
Homework
Take home test due
Riar: A.P Chemistry
UNIT 11: Thermodynamics (Spontaneity & Entropy) Chapter 16
Learning Objectives:
Students will be able to Define, compare and contrast, classify, differentiate, put in order, predict
using, identify correct and incorrect examples of, identify correct and incorrect interpretations of,
identify correct and incorrect applications of…the following terms:
First Law of Thermodynamics, spontaneous processes, nonspontaneous processes, entropy,
Second Law of Thermodynamics, microstate, Third Law of Thermodynamics, absolute entropy,
standard entropy, standard state, standard entropy of reaction, Gibbs free energy, standard free
energy change of a reaction
standard free energy of formation, thermodynamic equilibrium constant







Give a molecular interpretation of entropy
Relate entropy and disorder
Relate entropy and temperature
Apply qualitative rules for comparing entropy
Use heat capacity to calculate entropy
Predict the sign of the standard entropy of a reaction
Calculate the standard entropy of reaction
NJCCC standards addressed:
5.2.12.A.5 Describe the process by which solutes dissolve in solvents.
5.2.2.A.1 Sort and describe objects based on the materials of which they are made and their physical
properties.
5.2.8.A.1 Explain that all matter is made of atoms, and give examples of common elements
5.2.8.A.2 Analyze and explain the implications of the statement “all substances are composed of
elements.”
5.2.6.B.1 Compare the properties of reactants with the properties of the products when two or more
substances are combined and reaction
5.2.8.B.1 Explain, using an understanding of the concept of chemical change, why the mass of reactants
and the mass of products
5.2.12.B.3 Balance chemical equations by applying the law of conservation of mass.
Motivation:
ASK STUDENTS – WHAT ARE SPONTANEOUS PROCESSES ?
WHAT IS ENTROPY?
Development:
Thermodynamics Chapter 16Power point
Summary/Assessment:
Homework
Section 1 – Spontaneity and Entropy
17,18,21,23,25,27,28,29,31,32,33,34,35,36,37,67
Riar: A.P Chemistry
UNIT 11: Thermodynamics (Spontaneity & Entropy) Chapter 16
Learning Objectives:
Students will be able to Define, compare and contrast, classify, differentiate, put in order, predict
using, identify correct and incorrect examples of, identify correct and incorrect interpretations of,
identify correct and incorrect applications of…the following terms:
First Law of Thermodynamics, spontaneous processes, nonspontaneous processes, entropy,
Second Law of Thermodynamics, microstate, Third Law of Thermodynamics, absolute entropy,
standard entropy, standard state, standard entropy of reaction, Gibbs free energy, standard free
energy change of a reaction
standard free energy of formation, thermodynamic equilibrium constant







Give a molecular interpretation of entropy
Relate entropy and disorder
Relate entropy and temperature
Apply qualitative rules for comparing entropy
Use heat capacity to calculate entropy
Predict the sign of the standard entropy of a reaction
Calculate the standard entropy of reaction
NJCCC standards addressed:
5.2.12.A.5 Describe the process by which solutes dissolve in solvents.
5.2.2.A.1 Sort and describe objects based on the materials of which they are made and their physical
properties.
5.2.8.A.1 Explain that all matter is made of atoms, and give examples of common elements
5.2.8.A.2 Analyze and explain the implications of the statement “all substances are composed of
elements.”
5.2.6.B.1 Compare the properties of reactants with the properties of the products when two or more
substances are combined and reaction
5.2.8.B.1 Explain, using an understanding of the concept of chemical change, why the mass of reactants
and the mass of products
5.2.12.B.3 Balance chemical equations by applying the law of conservation of mass.
Motivation:
ASK STUDENTS – WHAT ARE SPONTANEOUS PROCESSES ?
WHAT IS ENTROPY?
Development:
Thermodynamics Chapter 16Power point
Summary/Assessment:
Homework
Section 2 – Calculations ΔS, ΔH and ΔG
Riar: A.P Chemistry
UNIT 11: Thermodynamics (Spontaneity & Entropy) Chapter 16
Learning Objectives:
Students will be able to Define, compare and contrast, classify, differentiate, put in order, predict
using, identify correct and incorrect examples of, identify correct and incorrect interpretations of,
identify correct and incorrect applications of…the following terms:
First Law of Thermodynamics, spontaneous processes, nonspontaneous processes, entropy,
Second Law of Thermodynamics, microstate, Third Law of Thermodynamics, absolute entropy,
standard entropy, standard state, standard entropy of reaction, Gibbs free energy, standard free
energy change of a reaction
standard free energy of formation, thermodynamic equilibrium constant
 Describe the effect of temperature on free energy
 Compare the enthalpy term and the entropy term in the Gibbs free energy equation at various
temperatures
 Apply the rules of thumb regarding the signs of H, S, G and spontaneity
 calculate free energy changes from standard enthalpy and standard entropy
 calculate standard free energy from standard free energies of formation
 Calculate K from G
NJCCC standards addressed:
5.2.12.A.5 Describe the process by which solutes dissolve in solvents.
5.2.2.A.1 Sort and describe objects based on the materials of which they are made and their physical
properties.
5.2.8.A.1 Explain that all matter is made of atoms, and give examples of common elements
5.2.8.A.2 Analyze and explain the implications of the statement “all substances are composed of
elements.”
5.2.6.B.1 Compare the properties of reactants with the properties of the products when two or more
substances are combined and reaction
5.2.8.B.1 Explain, using an understanding of the concept of chemical change, why the mass of reactants
and the mass of products
5.2.12.B.3 Balance chemical equations by applying the law of conservation of mass.
Motivation:
ASK STUDENTS – WHAT ARE SPONTANEOUS PROCESSES?
WHAT IS ENTROPY?
Development:
Thermodynamics Chapter 16 Power point
Summary/Assessment:
Homework
Section 3 – Equilibrium
55,57,58,59,60,61,63,65,66,72,73,74,75
Riar: A.P Chemistry
UNIT 11: Thermodynamics (Spontaneity & Entropy) Chapter 16
Learning Objectives:
Students will be able to Define, compare and contrast, classify, differentiate, put in order, predict
using, identify correct and incorrect examples of, identify correct and incorrect interpretations of,
identify correct and incorrect applications of…the following terms:
First Law of Thermodynamics, spontaneous processes, nonspontaneous processes, entropy,
Second Law of Thermodynamics, microstate, Third Law of Thermodynamics, absolute entropy,
standard entropy, standard state, standard entropy of reaction, Gibbs free energy, standard free
energy change of a reaction
standard free energy of formation, thermodynamic equilibrium constant
 Describe the effect of temperature on free energy
 Compare the enthalpy term and the entropy term in the Gibbs free energy equation at various
temperatures
 Apply the rules of thumb regarding the signs of H, S, G and spontaneity
 calculate free energy changes from standard enthalpy and standard entropy
 calculate standard free energy from standard free energies of formation
 Calculate K from G
NJCCC standards addressed:
5.2.12.A.5 Describe the process by which solutes dissolve in solvents.
5.2.2.A.1 Sort and describe objects based on the materials of which they are made and their physical
properties.
5.2.8.A.1 Explain that all matter is made of atoms, and give examples of common elements
5.2.8.A.2 Analyze and explain the implications of the statement “all substances are composed of
elements.”
5.2.6.B.1 Compare the properties of reactants with the properties of the products when two or more
substances are combined and reaction
5.2.8.B.1 Explain, using an understanding of the concept of chemical change, why the mass of reactants
and the mass of products
5.2.12.B.3 Balance chemical equations by applying the law of conservation of mass.
Motivation:
ASK STUDENTS – WHAT ARE SPONTANEOUS PROCESSES?
WHAT IS ENTROPY?
Development:
Thermodynamics Chapter 16 Power point
Summary/Assessment:
Homework
Section 3- Equilibrium
76,77, 78, 79, 81 ,83, 84, 85
Riar: A.P Chemistry
UNIT 11: Thermodynamics (Spontaneity & Entropy) Chapter 16
Learning Objectives:
Students will be able to:
 Describe the effect of temperature on free energy
 Compare the enthalpy term and the entropy term in the Gibbs free energy equation at various
temperatures
 Apply the rules of thumb regarding the signs of H, S, G and spontaneity
 calculate free energy changes from standard enthalpy and standard entropy
 calculate standard free energy from standard free energies of formation
 Calculate K from G
NJCCC standards addressed:
5.2.12.A.5 Describe the process by which solutes dissolve in solvents.
5.2.2.A.1 Sort and describe objects based on the materials of which they are made and their physical
properties.
5.2.8.A.1 Explain that all matter is made of atoms, and give examples of common elements
5.2.8.A.2 Analyze and explain the implications of the statement “all substances are composed of
elements.”
5.2.6.B.1 Compare the properties of reactants with the properties of the products when two or more
substances are combined and reaction
5.2.8.B.1 Explain, using an understanding of the concept of chemical change, why the mass of reactants
and the mass of products
5.2.12.B.3 Balance chemical equations by applying the law of conservation of mass.
Motivation:
ASK STUDENTS – WHAT ARE SPONTANEOUS PROCESSES?
WHAT IS ENTROPY?
Development:
Thermodynamics Chapter 16 Power point
Summary/Assessment:
Homework
A.P Free response Questions – Take home
Riar: A.P Chemistry
UNIT 12: Electrochemistry Chapter 17
Learning Objectives:
Students will be able to Define, compare and contrast, classify, differentiate, put in order, predict
using, identify correct and incorrect examples of, identify correct and incorrect interpretations of,
identify correct and incorrect applications of…the following terms:
redox reaction, oxidation number, half-reaction, oxidation, reduction, electrochemical cell
,voltaic cell, also called a galvanic cell ,electrolytic cell ,half-cell ,salt bridge ,anode ,cathode
cell reaction ,potential difference ,electromotive force ,standard electrode potential (E) ,standard
hydrogen electrode (SHE) ,reduction potential ,oxidation potential ,standard reduction potential
Left-Right-Below Diagonal Rule ,standard cell emf ’s (Ecell) ,volt ,coulomb ,joule ,Faraday’s
constant ,free-energy-Faraday equation ,Nernst equation ,reaction quotient ,electrolysis,
electrolytic cell ,electroplating ,redox titration








Describe the construction of voltaic cells
Compare and contrast anodes and cathodes
Draw and label a voltaic cell
Use cell notation for voltaic cells
Determine the strengths of oxidizing and reducing agents
Put a list of species in order of increasing strength as an oxidizing agent or reducing agent
Predict the direction of spontaneity from standard electrode potentials
Write reactions in the direction of spontaneity using the “Left-Right-Below Diagonal
Rule”
NJCCC standards addressed:
5.2.12.A.5 Describe the process by which solutes dissolve in solvents.
5.2.2.A.1 Sort and describe objects based on the materials of which they are made and their physical
properties.
5.2.8.A.1 Explain that all matter is made of atoms, and give examples of common elements
5.2.8.A.2 Analyze and explain the implications of the statement “all substances are composed of
elements.”
5.2.6.B.1 Compare the properties of reactants with the properties of the products when two or more
substances are combined and reaction
5.2.8.B.1 Explain, using an understanding of the concept of chemical change, why the mass of reactants
and the mass of products
5.2.12.B.3 Balance chemical equations by applying the law of conservation of mass.
Motivation:
ASK STUDENTS – HOW CAN CHEMICAL ENERGY BE CONVERTED TO ELECTRICAL
ENERGY?
WHAT IS AN GALVANIC CELL?
Development:
Thermodynamics Chapter 17 Power point
Summary/Assessment:
Homework
Section 1 Galvanic Cells
25,33,35,47,49.51,52,53,99,100,101,107
Riar: A.P Chemistry
UNIT 12: Electrochemistry Chapter 17
Learning Objectives:
Students will be able to Define, compare and contrast, classify, differentiate, put in order, predict
using, identify correct and incorrect examples of, identify correct and incorrect interpretations of,
identify correct and incorrect applications of…the following terms:
redox reaction, oxidation number, half-reaction, oxidation, reduction, electrochemical cell
,voltaic cell, also called a galvanic cell ,electrolytic cell ,half-cell ,salt bridge ,anode ,cathode
cell reaction ,potential difference ,electromotive force ,standard electrode potential (E) ,standard
hydrogen electrode (SHE) ,reduction potential ,oxidation potential ,standard reduction potential
Left-Right-Below Diagonal Rule ,standard cell emf ’s (Ecell) ,volt ,coulomb ,joule ,Faraday’s
constant ,free-energy-Faraday equation ,Nernst equation ,reaction quotient ,electrolysis,
electrolytic cell ,electroplating ,redox titration









Describe the construction of voltaic cells
Compare and contrast anodes and cathodes
Draw and label a voltaic cell
Use cell notation for voltaic cells
Use the Left-Right-Below Diagonal Rule to determine spontaneity for reactions already
given
Combine half-reactions to determine standard cell emf ’s (Ecell)
Write cell reactions
Calculate free-energy changes from emf ’s
Calculate emf’s from free-energy changes
NJCCC standards addressed:
5.2.12.A.5 Describe the process by which solutes dissolve in solvents.
5.2.2.A.1 Sort and describe objects based on the materials of which they are made and their physical
properties.
5.2.8.A.1 Explain that all matter is made of atoms, and give examples of common elements
5.2.8.A.2 Analyze and explain the implications of the statement “all substances are composed of
elements.”
5.2.6.B.1 Compare the properties of reactants with the properties of the products when two or more
substances are combined and reaction
5.2.8.B.1 Explain, using an understanding of the concept of chemical change, why the mass of reactants
and the mass of products
5.2.12.B.3 Balance chemical equations by applying the law of conservation of mass.
Motivation:
ASK STUDENTS – HOW CAN CHEMICAL ENERGY BE CONVERTED TO ELECTRICAL
ENERGY?
WHAT IS AN GALVANIC CELL?
Development:
Thermodynamics Chapter 17 Power point
Summary/Assessment:
Homework
Section 2 & 3 Calculations cell potential, ΔG and Nernst Equation
39,41, 43, 403, 108, 109, 110, 113
55,59,61,63,67,68,71,72,75,77,114
Riar: A.P Chemistry
UNIT 12: Electrochemistry Chapter 17
Learning Objectives:
Students will be able to Define, compare and contrast, classify, differentiate, put in order, predict
using, identify correct and incorrect examples of, identify correct and incorrect interpretations of,
identify correct and incorrect applications of…the following terms:
redox reaction, oxidation number, half-reaction, oxidation, reduction, electrochemical cell
,voltaic cell, also called a galvanic cell ,electrolytic cell ,half-cell ,salt bridge ,anode ,cathode
cell reaction ,potential difference ,electromotive force ,standard electrode potential (E) ,standard
hydrogen electrode (SHE) ,reduction potential ,oxidation potential ,standard reduction potential
Left-Right-Below Diagonal Rule ,standard cell emf ’s (Ecell) ,volt ,coulomb ,joule ,Faraday’s
constant ,free-energy-Faraday equation ,Nernst equation ,reaction quotient ,electrolysis,
electrolytic cell ,electroplating ,redox titration











Combine half-reactions to determine standard cell emf ’s (Ecell)
Write cell reactions
Calculate free-energy changes from emf ’s
Calculate emf’s from free-energy changes
Calculate the equilibrium constant from emf ’s
Calculate Ecell under nonstandard conditions
Describe the electrolysis of various substances
Describe the electroplating of metals
Calculate stoichiometry problems involving electrolysis
Describe the similarities between acid-base titrations and redox titrations
Discuss the key points to redox titrations
NJCCC standards addressed:
5.2.12.A.5 Describe the process by which solutes dissolve in solvents.
5.2.2.A.1 Sort and describe objects based on the materials of which they are made and their physical
properties.
5.2.8.A.1 Explain that all matter is made of atoms, and give examples of common elements
5.2.8.A.2 Analyze and explain the implications of the statement “all substances are composed of
elements.”
5.2.6.B.1 Compare the properties of reactants with the properties of the products when two or more
substances are combined and reaction
5.2.8.B.1 Explain, using an understanding of the concept of chemical change, why the mass of reactants
and the mass of products
5.2.12.B.3 Balance chemical equations by applying the law of conservation of mass.
Motivation:
ASK STUDENTS – HOW CAN CHEMICAL ENERGY BE CONVERTED TO ELECTRICAL
ENERGY?
WHAT IS AN GALVANIC CELL?
Development:
Thermodynamics Chapter 17 Power point
Summary/Assessment:
Homework
Section 4 Electrolysis
79,81,83,85,86,87,89,94,95,98,111,116
Riar: A.P Chemistry
UNIT 12: Electrochemistry Chapter 17
Learning Objectives:
Students will be able to Define, compare and contrast, classify, differentiate, put in order, predict
using, identify correct and incorrect examples of, identify correct and incorrect interpretations of,
identify correct and incorrect applications of…the following terms:
redox reaction, oxidation number, half-reaction, oxidation, reduction, electrochemical cell
,voltaic cell, also called a galvanic cell ,electrolytic cell ,half-cell ,salt bridge ,anode ,cathode
cell reaction ,potential difference ,electromotive force ,standard electrode potential (E) ,standard
hydrogen electrode (SHE) ,reduction potential ,oxidation potential ,standard reduction potential
Left-Right-Below Diagonal Rule ,standard cell emf ’s (Ecell) ,volt ,coulomb ,joule ,Faraday’s
constant ,free-energy-Faraday equation ,Nernst equation ,reaction quotient ,electrolysis,
electrolytic cell ,electroplating ,redox titration











Combine half-reactions to determine standard cell emf ’s (Ecell)
Write cell reactions
Calculate free-energy changes from emf ’s
Calculate emf’s from free-energy changes
Calculate the equilibrium constant from emf ’s
Calculate Ecell under nonstandard conditions
Describe the electrolysis of various substances
Describe the electroplating of metals
Calculate stoichiometry problems involving electrolysis
Describe the similarities between acid-base titrations and redox titrations
Discuss the key points to redox titrations
NJCCC standards addressed:
5.2.12.A.5 Describe the process by which solutes dissolve in solvents.
5.2.2.A.1 Sort and describe objects based on the materials of which they are made and their physical
properties.
5.2.8.A.1 Explain that all matter is made of atoms, and give examples of common elements
5.2.8.A.2 Analyze and explain the implications of the statement “all substances are composed of
elements.”
5.2.6.B.1 Compare the properties of reactants with the properties of the products when two or more
substances are combined and reaction
5.2.8.B.1 Explain, using an understanding of the concept of chemical change, why the mass of reactants
and the mass of products
5.2.12.B.3 Balance chemical equations by applying the law of conservation of mass.
Motivation:
ASK STUDENTS – HOW CAN CHEMICAL ENERGY BE CONVERTED TO ELECTRICAL
ENERGY?
WHAT IS AN GALVANIC CELL?
Development:
Thermodynamics Chapter 17 Power point
Summary/Assessment:
Homework
A.P Free response Questions – Take home
Review For the A.P Exam May 2
UNIT 13: Final AP CHEMISTRY PROJECT
End of the year project: Guidelines
Learning Objectives:
The objective of this project is to allow students to explore aspects of Chemistry you haven’t yet
experienced. Specifically, research based experimentation, lab design, data analysis, and (most
importantly) science education. You and your partner will be assigned a Lab experiment to
explore the problem, conduct your experiment, analyze your data, and finally teach the
experiment to the entire class. You will be assessed in two ways: First, I will grade your lab’s
procedure and analysis. Then, you will be graded by me and the rest of the class on the quality of
your lesson. This one project represents the majority (50%) of your 4th quarter grade and ALL of
you final exam grade.
NJCCC standards addressed:
5.2.12.A.5 Describe the process by which solutes dissolve in solvents.
5.2.2.A.1 Sort and describe objects based on the materials of which they are made and their physical
properties.
5.2.8.A.1 Explain that all matter is made of atoms, and give examples of common elements
5.2.8.A.2 Analyze and explain the implications of the statement “all substances are composed of
elements.”
5.2.6.B.1 Compare the properties of reactants with the properties of the products when two or more
substances are combined and reaction
5.2.8.B.1 Explain, using an understanding of the concept of chemical change, why the mass of reactants
and the mass of products
5.2.12.B.3 Balance chemical equations by applying the law of conservation of mass.
Motivation:
Development:
Each Group will :
1) Try out the experiment and modify it if necessary to get it working. This means that you must
prepare all solutions and get all the equipment needed. You may have to learn additional theory
and use other sources to get more information. THE LAB MUST WORK. Perform the
experiment sufficient number of times so that you understand what you are doing and so that you
have enough consistent data to allow your group to reach a conclusion. A single run generally
means nothing.
Summary/Assessment:
1) Prepare a written Lab write –up for distribution to the class. The write up should contain the
experiment’s purpose an introduction, a procedure, a data table and a place to do the calculations.
You also need some form of activity for the class to do. It could be asset of questions or an
overall theory statement so that each individual in the rest of the class is responsible for doing
something which shows that they have learned something. Make copies of the lab write up for
the class.
2) Students will be prepared on the due date to teach the lesson in which all members of the
group teach the lab’s principles and concepts and how the experiment was done. You may want
to show the experimental set up and how the experiment was conducted and data was collected.
You will need to take the class through calculations and the final result. This presentation will
require at least a class period and may require more time. It must be rehearsed with Mrs. Riar at
least two days before the Final presentation.
3) Each group will turn in complete set of teacher notes describing how to make all of the
solutions, showing all of your experimental data and your calculations and graphs as well as your
results
Every group is the teacher for every aspect of their experiment. Both members of the group are
expected to share all parts of this lab experiment equally.
Homework
Proposed Presentation dates Assigned Experiments:
 Group 1 Complex ion Ag(NH3)2
 Group 2 Avogadro’s
 Group 3 Redox
 Group 4 Ksp of PbCl2
Presentation date June 1st
Presentation date June 2nd
Presentation date June 6th
Presentation date June 7th
May 7th onwards:
Before students make any solutions they will do the calculations and show all the
calculations
Make solutions and do the experiment. Calculate results. Repeat the experiment to refine
their technique and get improved results and additional data.