AP CHEMISTY SYLLABUS
OVERVIEW OF AP CHEMISTRY COURSE
CLASS MATERIALS:
You will need to bring to class EACH day: textbook (“Chemistry“by Steven Zumdahl, 7th Ed), a 3ring binder, spiral notebook, calculator and a pencil or pen. A separate laboratory notebook is also
required. A TI-84+ graphing calculator is used extensively in class and it is suggested that you
purchase your own as the classroom set is not available for checkout.
COURSE DESCRIPTION:
This course meets 5 days a week for one 50 minute Period each day with lab days to extend for one
hour after or before school on an average of one day ever other week to allow additional time if
required by students. The A.P. Chemistry course is designed to be the equivalent of a General
Chemistry course taken in college. Upon completion of this course, students will be prepared to
take the AP Chemistry test. A score of 4 or 5 on the test COULD result in advanced placement or
General Chemistry credit upon entrance into college (depending on the institution). Students will
receive a sequentially planned A.P. Chemistry program designed by the College Board for A.P.
Chemistry classes. The course includes manipulation of materials, experimentation with written
labs, problem solving, class discussions, and lecture. By design, this course is more rigorous than
high school chemistry, because of the type of text used, topics covered, emphasis placed on
chemical calculations, formulation of principles, and the emphasis placed on labs and written
reports. It is strongly recommended that students take the Honors Chemistry course as a
prerequisite for this course because several of the required AP labs are integrated into that course.
EXPECTATIONS:
Do you want to learn? Will you do the work necessary to be prepared for class everyday? If so, then
you are in the right class! All of you have taken at least 3 science courses by now. Your academic
responsibilities will include doing ALL of the reading, problem sets, and most lab reports outside of
class. You will have at least one hour of homework every night. This is a college level course
and you will be treated as such. The more prepared you are to learn, the more you will. Each
chapter you will be given a calendar outlining due dates for your assignments and labs along with
test dates.
This is a very fast-paced class with fairly inflexible deadlines. Before the AP Examination in the
spring there will be 2 weekend optional review sessions where you will have the opportunity to
complete a full AP Exam under AP exam conditions. All students are required to take the actual AP
Chemistry exam to receive credit for the course. After the Exam in May, the remaining 2 - 2 ½
weeks of school will devoted to select special topics in chemistry.
BEHAVIOR:
As for behavior, RESPECT is the name of the game. If you can’t follow the rules, you can’t play
the game.
1) All students are expected to be in class on time and prepared to work.
2) Since this an advanced Lab course students may be working on various activities and labs
during the same period. Therefore, responsible and safe behavior will be expected at all
times. If a student has demonstrated that he / she can not conduct themselves in a
responsible manner he /she will be removed from the class permanently.
3) Students will work in small lab groups and will be expected to contribute to the groups’
work in an equitable manner or will be removed from the group and be required to complete
all lab work by themselves.
4) All students must continue to show a desire to work at an AP level or a parent conference
will be requested. If this meeting fails to produce the desired results the student will be
referred to the guidance office for further action.
5) All other school rules and policies will be adhered to and violations will result in appropriate
consequences as outlined by the student handbook.
EVALUATION:
Notebooks; SAVE ALL PAPERS! You may need them to verify a grade or for college
interviews. The papers should be arranged in chronological order. These papers will ultimately
serve as the basis for your science portfolio.
Labs and Demonstrations; You will perform the twenty two major labs that are
recommended for the AP Chemistry Course along with a few others that will enrich your
understanding of chemistry.. It is very important to be very detailed and thorough when conducting
a lab. You will be expected to follow a specific format when writing up the data from the
experiment in your lab report. Failure to adhere to lab safety and conduct rules results in immediate
removal from the lab and no credit. Different concepts and process skills will be assessed for each
lab along with appropriate lab conduct. Labs conducted in Honors Chemistry will be referenced in
this course. You will work in small lab groups where collaboration is expected but individual typed
lab reports are required. Although a satisfactory Lab report is required for each lab the lab score will
not be averaged into the final grade but will result in a grade letter reduction for each unacceptable
lab.
Lab Notebook; Since a typed lab report will be required for all labs, you will not need a
special laboratory notebook. A bound composition notebook will be required in the labs to record
lab notes and data. No loose sheets of paper to write notes on will be tolerated.
Text Problems & Practice Tests; You will be given nightly problems from the chapter and
daily assessments will be used to determine comprehension of the materials. All work is for your
benefit and your benefit only. Assigned Text problems will be representative of the rigor of the
questions expected on both the chapter test and the AP exam. The type of resources such as
calculators and reference charts will be limited by the rules for the AP exam. Appropriate past AP
tests questions are given the day before a chapter test for additional test preparation.
Late work; NO CREDIT IS GIVEN FOR LATE ASSIGNMENTS. If an assignment is
checked in class, it is due at that time, not at the end of the period. If the assignments are turned in
for me to grade, I must have it by the end of the day.
Tests & Quizzes; Tests will be given at the end of each chapter or unit. The test is composed
of multiple choice and free response questions from AP Released exams. They are timed and
scored in the same fashions as the AP Exam. There is usually a comparable retake test, but you are
required to come in and make corrections to your original test first to show you have a better
mastery of the material before retaking the test. During the second quarter, Ion quizzes will be
given twice a week. Reaction equation quizzes are given once a month starting the 2nd quarter
along with monthly Ion review quizzes. Expect the mathematical questions to be common, rigorous
and representative of the topic being covered. If you miss a test or need to take a retest, you will
make it up before or after school, NOT during class. Tests are worth 100% of the total grade with
retest scores totally replacing original scores.
Grading Scale; The grading scale is based on percent scores- NOT TOTAL POINTS! To
earn an A you must demonstrate 100 - 85% proficiency in completing the assignment, activity, lab,
or test. 84-70% is a B, 69-60% is a C, and 59-50% for a D. Quarters are weighted equally with the
midterm and final exam carrying the school’s prescribed weight. There is no extra credit!
COURSE OUTLINE
TEXT: Chemistry, Steven Zumdahl, Seventh Edition
LAB MANUALS: Chemistry with Calculators (Vernier, 2000)
Advanced Chemistry with Vernier, (2004)
PRACTICE BOOK: AP Chemistry Multiple Choice & Free Response Questions in Preparation for
the AP Chemistry Exam,
SUGGESTED AP REVIEW BOOKS:
(All are available at the Public Library or can purchased at any bookstore).
1. Kaplan. “Nice book supplement, but not good for weeks before test.”
2. Five Steps to a Five. “A cross between Kaplan and Princeton. There are errors in here.”
3. Princeton. “Minimal coverage. Gives basic ideas.”
Following each chapter is a list of required problems from the text.
Unit 1: ATOMIC STRUCTURE
Chapter 1: Chemical Foundations
Chapter 2: Atoms, Molecules, and Ions
Chapter 7: Atomic Structure and Periodicity
Unit 2: STOICHIOMETRY
Chapter 3: Stoichiometry
Chapter 4: Types of Chemical Reactions and Solution Stoichiometry
Unit 3: GASES AND THERMOCHEMISTRY
Chapter 5: Gases
Chapter 6: Thermochemistry
Unit 4: CHEMICAL BONDING
Chapter 8: Bonding
Chapter 9: Covalent Bonding: Orbitals;
Unit 5: LIQUIDS, SOLIDS, AND SOLUTIONS
Chapter 10: Liquids and Solids
Chapter 11: Properties of Solutions
Unit 6: KINETICS AND EQUILIBRIUM
Chapter 12: Chemical Kinetics
Chapter 13: Chemical Equilibrium;
Unit 7: ACIDS - BASES, AQUEOUS EQUILIBRIUM
Chapter 14: Acids and Bases
Chapter 15: Aqueous Equilibrium
Unit 8: ENTROPY, FREE ENERGY, AND ELECTROCHEMISTRY
Chapter 16: Spontaneity, Entropy, and Free Energy
Chapter 17: Electrochemistry
The following are assigned as reading during the AP Review days:
Unit 9: NUCLEAR CHEMISTRY
Chapter 21: The Nucleus: A Chemist’s View
Unit 10: ORGANIC AND BIOCHEMISTRY
Chapter 22: Organic Chemistry
Chapter 23: Biochemistry
Unit 11: REPRESENTATIVE ELEMENTS AND TRANSITION METALS
Chapter 18: The Representative Elements: Groups 1A through 4A
Chapter 19: The Representative Elements: Groups 5A through 8A
Chapter 20: Transition Metals and Coordination Chemistry
Required Supporting Labs
Unit 1: ATOMIC STRUCTURE
Labs: Hydrogen Spectrum-Balmer Series
Determining Avogadro’s number (Vernier Lab #31– Required AP Lab 21)
Electroplating ( Vernier Lab #21– Required AP Lab 21)
Alpha, Beta, and Gamma Radiation (Vernier Lab #27)
Radiation Shielding (Vernier Lab #28)
Unit 2: STOICHIOMETRY
Labs: The Determination of a Chemical Formula (Vernier Lab #1 – Required AP Lab 1)
The Determination of the Percent Water in a Compound (Vernier Lab #2 – Required AP Lab 2)
Determining the Mole Ratios in a Chemical Reaction (Vernier Lab # 9 – Required AP Lab 9)
The Syntheses of Alum (Vernier Lab #15A – Required AP Lab 15)
An Oxidation-Reduction Titration (Vernier # 8 – Required AP Lab 8)
Unit 3: GASES AND THERMOCHEMISTRY
Labs: Molecular Weight of a Volatile Liquid (Vernier Lab # 3– Required AP Lab 3)
The Molar Volume of a Gas (Vernier Lab #5– Required AP Lab 5)
Unit 4: CHEMICAL BONDING
Labs: Liquid Chromatography (Vernier Lab # 18– Required AP Lab 18)
Conductimetric Titration and Gravimetric Determination of a Precipitate (Vernier Lab # 16–
Required AP Lab 16)
Separation and Qualitative Analysis of Cations and Anions (Vernier Lab #14– Required AP Lab 14)
Unit 5: LIQUIDS, SOLIDS, AND SOLUTIONS
Labs: Using Freezing Point to Find Molecular Weight (Vernier Lab # 4– Required AP Lab 4)
Determining the Concentration of a Solution (Vernier Lab #17– Required AP Lab 17)
Unit 6: KINETICS AND EQUILIBRIUM
Labs: Rate Law Determination of the Crystal Violet Reaction (Vernier # 30)
The Determining of an Equilibrium Constant (Vernier Lab#10– Required AP Lab 10)
Decomposition of Hydrogen Perioxide (Vernier Lab # 12– Required AP Lab 12)
Unit 7: ACIDS - BASES, AQUEOUS EQUILIBRIUM
Labs: Standardization a Solution of Sodium Hydroxide (Vernier Lab #6– Required AP Lab 6)
Acid-Base Titration (Vernier Lab # 7– Required AP Lab 7)
Investigating Indicators (Vernier # 11– Required AP Lab 11)
Buffers (Vernier Lab # 19– Required AP Lab 19)
Unit 8: ENTROPY, FREE ENERGY, AND ELECTROCHEMISTRY
Lab: Determining the Enthalpy of a Chemical Reaction (Vernier Lab #13– Required AP Lab 13)
Electrochemistry: Voltaic Cells (Vernier Lab # 20– Required AP Lab 20)
The following are assigned as Labs during the AP Review days:
Unit 10: ORGANIC AND BIOCHEMISTRY
Lab: The Synthesis and Analysis of Aspirin (Vernier Lab #22– Required AP Lab 22)
The Making of Esters (Cebco Standard Publishing Lab 49)
Saponification (Cebco Standard Publishing Lab 49)
AP Chemistry Content Expectations
The following are the goals and expectations that will that will be achieved prior to the AP
Chemistry course completion.
I. TOPIC 1 Matter & Measurement
ALL students should;

Recall a definition of chemistry

Understand the process and stages of scientific (logical) problem solving

Recall the three states of matter, their general properties and the methods for their interconversion

Understand and recall definitions for physical and chemical change

Know the difference between elements, mixtures and compounds including the difference between
heterogeneous and homogeneous mixtures

Understand and be able to use scientific notation (standard form)

Recall and use SI units and prefixes

Be able to convert between units using the rules of significant figures

Understand the concept of derived units and use relationships relating to density

Recall the meaning of uncertainty and understand and be able to use the rules for determining
significant figures and rounding off on all calculations

Understand the differences between, and be able to apply, the concepts of accuracy and precision
II. TOPIC 2 Atoms, Ions & Nomenclature
ALL students should;

Recall a very brief history of Atomic Theory

Know and understand the five main aspects of Dalton's Atomic Theory

Recall some of the experiments that led to the identification of sub-atomic particles

Know the three particles that make up the atom and their relative charges, masses and positions in
the atom

Be able to use the Atomic # and Mass # of an isotope to calculate the numbers of protons, neutrons
and electrons present

Know what the term isotope means and be able to perform simple calculations relating to isotopic
data

Understand the phenomenon of radioactivity and the properties of radioactive particles and be able
to do half-life calculations

Be able to write nuclear equations

Recall some uses of radioactivity

Understand the term mass deficit

Be able to use neutron : proton ratio to make predictions about stability

Understand the terms nuclear fission and fusion

Understand, that in very general terms, radioactivity involves the rearrangement of the nucleus and
chemical reactions involve the rearrangement of electrons

Know the approximate locations of metals, non-metals and metalloids on the periodic table

Understand the meaning of the terms Molecule and Ion

Learn the lists of common anions ,cations and polyatomic ions

Know how to combine those anions and cations in the correct proportions to form ionic compounds
with no net charge

Be able to name binary ionic compounds of a metal and a non-metal

Be able to name binary molecular compounds of two non-metals

Be able to name simple binary acids

Be able to name ionic compounds containing polyatomic anions

Be able to name oxoacids and compounds containing oxoanions

Be able to name hydrated salts
III. TOPIC 3 Electronic Configuration
ALL students should;

Understand the Bohr model of the atom

Understand how line emission spectra are formed

Appreciate that the electron can be considered to have wave like properties as well as particle type
properties

Understand and do calculations using equations that relate the Energy, frequency, speed and
wavelength of waves including the Rydberg equation

Understand the concept of electrons in shells and the use of quantum numbers

Understand the use of the terms s, p, d and f and their use in orbital notation

Recall and understand the rules for filling orbitals and determining electronic configuration, including
the Pauli exclusion principle, Hund's rule of maximum multiplicity and notable exceptions

Be able to construct the electronic configuration of the elements using the s, p and d and f notation

Be able to construct the electronic configuration of the elements using the noble gas core and s, p, d
and f notation

Be able to construct the electronic configuration of simple ions (including d block ions)

Recall the shapes of the s, p and d orbitals

Recall that orbitals are electron probability maps

Be able to describe electronic configurations using the electrons in boxes notation

Recall the meanings of the terms paramagnetic, diamagnetic and isoelectronic
IV. TOPIC 4 Stoichiometry
ALL students should;

Be able to write chemical equations in words

Be able to write chemical equations using chemical formulae and chemical symbols (this requires
knowledge, and correct use of, chemical nomenclature)

Understand, and be able to use, state symbols as part of chemical equation writing

Be able to balance chemical equations

Understand why balancing chemical equations is important

Understand the concept of percentage by mass

Be able to calculate empirical formulae from percentage by mass data

Be able to convert empirical formulae to molecular formulae by using Molar Mass data

Understand and be able to apply the concept of the mole in chemical calculations (including the
application of Avogadro's number)

Be able to use combustion data to calculate empirical formulae of compounds

Understand the importance of, and be able to apply, the concept of stoichiometric coefficients
relating to reacting ratios

Know how to calculate the number of moles of a solid substance present in a reaction from data

Be able to perform calculations relating to molarity

Understand and be able to perform calculations relating to the Beer-Lambert law

Be able to perform calculations relating to dilution

Be able to perform calculations relating to molality

Be able to calculate the formulae of hydrated salts from experimental data

Understand, and be able to apply, the concept of a limiting reactant

Understand, and be able to apply, the concept of percentage yield
V. TOPIC 5 Qualitative & Quantitative Chemistry
ALL students should;

Understand that a reaction in aqueous solution is one that is carried out in water

Understand the terms electrolyte, weak electrolyte and non-electrolyte and be able to predict which
compounds fall into which category

Be able to calculate the individual ion concentrations when ionic compounds are dissolved in water

Understand the difference between, and be able to write, full, ionic and net ionic equations

Learn and be able to apply solubility rules

Be familiar with a limited number of colors associated with precipitates

Recall that an acid is a hydrogen ion donor

Recall that a base is a hydrogen ion acceptor

Understand how the degree of ionization/dissociation determines the strength of an acid and a base

Understand that in a neutralization reaction an acid and base react to form a salt and water

Learn some reactions that produce gases as products and the chemical tests for those gases

Understand that oxidation and reduction can be described in terms of loss and gain of electrons
respectively

Be able to find the oxidation number of an element within a compound

Become familiar with some common oxidizing and reducing agents and the half-equations that
represent their action

Understand and be able to recognize the different types of REDOX reaction. Namely synthesis
(combination), decomposition, combustion, single and double displacement (replacement) including
metal displacement, hydrogen displacement from water and acids and halogen displacement

Learn and be able to use the reactivity series as a tool for predicting displacement reactions

Understand the concept of disproportionation

Recall and understand the technique of titration

Be able to carry out simple quantitative moles calculations relating to REDOX titration data
VI. TOPIC 6 Gases
ALL students should;

Be able to convert between different units of pressure

Be able to convert between different units of temperature

Recall and be able to use Boyle's law in calculations

Recall and be able to use Charles' law in calculations

Recall and be able to use Gay-Lussac's law in calculations

Recall and be able to use Avogadro's law in calculations

Recall and be able to use the Combined gas law and the General gas law in calculations

Recall and be able to use the Ideal gas law in calculations

Understand and be able to use the van der Waals equation (modified ideal gas law) in calculations

Recall and be able to use Dalton's law of partial pressures in calculations

Recall the conditions that are used as standard in calculations

Be able to use molar gas volume in calculations

Understand the Kinetic theory as applied to gases

Understand the concept of, and be able to perform calculations involving, the root-mean-squarespeed of gases

Understand the terms effusion and diffusion and be able to perform calculations relating to those
concepts
VII. TOPIC 7 Periodicity
ALL students should;

Understand that regular, repeatable patterns occur across periods and within groups on the periodic
table

Appreciate that these patterns sometimes have notable exceptions

Recall and understand that the noble gases have full outer shells that represent stable electronic
configurations

Recall how, and understand why, group I, II, VI and VII elements achieve pseudo noble gas
electronic configurations

Recall the definition of ionization energy

Recall the definition of electron affinity

Recall and understand the variation in ionization energy and electron affinity when moving about the
periodic table

Be able to predict the group an element is in from ionization energy data

Understand and be able to apply the terms diamagnetic and paramagnetic

Recall how and why atomic and ionic size vary when moving about the periodic table

Understand how many physical properties change gradually when moving about the periodic table

Understand and recall the change in the specific chemical properties mentioned in TOPIC 7
VIII. TOPIC 8 Bonding
ALL students should;

Understand that when forming chemical bonds atoms are attempting to form more stable electronic
configurations

Understand the essential difference between intra and inter bonding

Understand the concept of ionic bonding and the nature of the ionic bond

Understand the concept of covalent bonding and nature of the covalent bond

Be able to draw Lewis structures

Understand the concept of resonance related to Lewis structures

Understand the concept of formal charge related to Lewis structures

Be able to predict the shape of, and bond angles in, simple molecules and ions using VSEPR theory

Understand the concept of the dative (co-ordinate) bond related to Lewis structures

Understand that ionic bonding and covalent bonding are at two ends of a sliding scale of bond type

Understand the concept of electronegativity

Understand that polarization caused by small highly charged cations leads to ionic compounds
exhibiting some covalent character

Understand that differences in electronegativity in covalent molecules causes dipoles and some ionic
character in covalent compounds

Understand when molecules exhibit polarity

Be able to predict the shapes of simple molecules and ions using Lewis structures

Understand the occurrence, relative strength and nature of dipole-dipole interactions, London
dispersion forces and hydrogen bonds

Understand how solid structure influences properties

Understand the nature of liquids

Understand the nature of sigma and pi bonds

Understand and be able to identify different types of orbital hybridization
IX. TOPIC 9 Thermochemistry
ALL students should;

Learn definitions that describe the systems studied in thermochemistry

Understand, be able to quote a definition and write suitable equations for standard enthalpy of
formation

Understand, be able to quote a definition and write suitable equations for standard enthalpy of
combustion

Understand and be able to use a Hess's law cycle or algebraic methods to calculate a given enthalpy
change

Understand and be able to use in calculations, average bond energy terms

Understand the meaning of the terms exothermic and endothermic

Understand and be able to apply the concept of entropy both in descriptive and calculation contexts

Understand and be able to apply the concept of Gibbs Free Energy both in descriptive and
calculation contexts

Understand and be able to apply the energetics of the ionic bond as described by the Born-Haber
cycle and associated calculations

Understand the role of charge density in determining some physical properties of ionic compounds
X. TOPIC 10 Transition Metal Basics
ALL students should;

Understand and be able to write electronic configurations of transition metals and their ions

Recall some colors of transition metals and understand when color occurs

Be able to recognize and name complex ions

Understand and be able to write equations for complex ion reactions (Ligand exchange &
Decomposition)
XI. TOPIC 11 Organic Basics
ALL students should;

Be able to name some simple aliphatic organic compounds

Understand and be able to write equations for some organic reactions (Combustion, Substitution,
Acid Base, Addition & Esterification) \
XII. TOPIC 12 Net Ionic Equation Writing
ALL students should;

Be able to write and balance net ionic equations for Double Replacement Reactions

Be able to write and balance net ionic equations for Simple REDOX Reactions

Be able to write and balance net ionic equations for Non-Simple REDOX Reactions

Be able to write and balance net ionic equations for Hydrolysis Reactions

Be able to write and balance net ionic equations for Complex Ion (Transition Metal) Reactions

Be able to write and balance net ionic equations for Organic Reactions

Be able to answer simple questions associated with the reactions in TOPIC 12
XIII. TOPIC 13 Equilibrium
ALL students should;

Understand the concept of dynamic equilibrium

Be able to write an expression in terms of concentrations for the equilibrium constant Kc given a
chemical equation

Understand that equilibria take a finite time to be achieved

Be able to calculate values for Kc and associated data from initial concentrations

Be able to write an expression in terms of partial pressures for the equilibrium constant Kp given a
chemical equation

Be able to calculate values for Kp and associated data from pressure data

Recall and understand Le Chatelier's Principle

Understand the application of Le Chatelier's Principle and be able to predict the shift in position of
equilibria and optimum conditions in reactions

Understand and be able to apply the relationship of Kc to Kp, the different formats of Kc (reciprocals
and roots) and the relationships in simultaneous equilibria

Understand and be able to apply to calculations, the concept of solubility product

Understand and be able to apply to calculations, the concept of common ion effect

Understand and be able to interpret phase diagrams

Understand and be able to interpret heating and cooling curves
XIV. TOPIC 14 Acids & Bases
ALL students should;

Be able to recall the Bronsted Lowry, Arrhenius and Lewis definitions of an acids and bases

Be able to identify acid base conjugate pairs

Recall the difference between strong and weak acids in terms of ionization

Be able to calculate pH of strong acids and strong bases

Be able to calculate pH of weak acids and weak bases using Ka and Kb

Recall a definition of Kw, the ionic product of water

Recall the definition of a buffer

Understand and how a buffer works

Be able to identify and calculate the pH of a buffer solution

Understand the techniques and procedures associated with titrations

Be able to sketch titration curves and be able to suggest a suitable indicator for a particular titration

Understand the hydrolysis of salts and the effect this has on pH

Understand the meaning of the term 'equivalence point'

Understand how indicators work
XV. TOPIC 15 Kinetics
ALL students should;

Be able to recall AND understand Collision Theory

Be able to recall AND understand how temperature, concentration, surface area and catalysts affect
a rate of reaction

Understand AND be able to interpret a Maxwell-Boltzmann distribution plot

Understand AND be able to interpret an energy profile plot

Be able to deduce orders, rate equations and rate constants (including units) from initial rate data

Understand the link between the rate determining (slow step) in a reaction mechanism and the rate
equation

Understand AND be able to interpret graphical data relating to rates
XVI. TOPIC 16 Electrochemistry
ALL students should;

Recall the definition of oxidation and reduction in terms of electrons

Understand and recall the definition of standard electrode potential

Understand and recall how to construct a cell diagram (line notation) and draw a diagram (picture) of
the apparatus needed

Recall the conditions that standard electrode potentials are measured under

Understand the nature and purpose of a salt bridge

Be able to predict the likelihood or otherwise of chemical reactions using standard electrode
potentials and understand how those predictions may not prove to be accurate

Understand and use the Nernst equation

Understand the relationship between Gibbs free energy, equilibrium constants and Ecell, and be able
to perform related calculations

Understand electrolysis and be able to perform quantitative calculations relating to it
XVII. TOPIC 17 Colligative Properties
ALL students should;

Understand the concept of vapor pressure

Be able to relate changes (both quantitative and qualitative) in vapor pressure to addition of nonvolatile solutes to solvents (Raoult's Law)

Understand and recall Raoult's Law in terms of ideal solutions of two volatile components AND
deviations from ideal behavior

Be able to recall and use equations relating to quantitative treatments of Boiling Point Elevation,
Freezing Point Depression, Osmotic Pressure and the van't Hoff factor