Revised 07.08.15
St Charles Parish Public Schools
Chemistry Curriculum Map 2015-16
Topic
Classroom Policies and
Procedures
Lab Safety & Equipment
First and Second Quarters
Chapter Outcomes
n/a

Chemistry is a Physical Science
(Section 1)
Matter and Its Properties
(Section 2)
1
Elements (Section 3)
Scientific Method (Section 1)
GLEs
2
Explain expectations and procedures in the
laboratory.
(F & PK)
 Identify laboratory safety procedures and choose
appropriate laboratory safety procedures given a lab
scenario.
(T & R)
Lab Teacher-made Assessment -- 1 day
 Define chemistry
 List examples of the branches of chemistry
 Compare and contrast basic research, applied
research, and technological development
 Distinguish between the physical properties and
chemical properties of matter.
 Classify changes of matter as physical or chemical.
 Explain the gas, liquid, and solid states in terms of
particles.
 Explain how the law of conservation of energy applies
to changes of matter.
 Distinguish between a mixture and a pure substance.
 Use a periodic table to name elements, given their
symbols.
 Use a periodic table to write the symbols of elements,
given their names.
 Describe the arrangement of the periodic table.
 List the characteristics that distinguish metals,
nonmetals, and metalloids.
Chapter 1 Teacher-made Assessment -- 1 day
 Describe the purpose of the scientific method.
Time Frame
1 Day
2 Days
1 Days
2 Days
SI.12
PS.14
PS.17
PS.31
2 Days
PS.1
2 Days
1
Revised 07.08.15
Units of Measurement (Section
2)
Using Scientific Measurements
(Section 3)
Measurements Lab
The Atom: From Philosophical
Idea to Scientific Theory (Section
1)
3
The Structure of the Atom
(Section 2)
 Distinguish between qualitative and quantitative
observations.
 Describe the differences between hypotheses,
theories, and models.
 Distinguish between a quantity, a unit, and a
measurement standard.
 Name and use SI units for length, mass, time,
volume, and density.
 Distinguish between mass and weight.
 Perform density calculations.
 Transform a statement of equality into a conversion
factor.
 Distinguish between accuracy and precision.
 Determine the number of significant figures in
measurements.
 Perform mathematical operations involving significant
figures.
 Convert measurements into scientific notation.
 Distinguish between inversely and directly proportional
relationships.

Chapter 2 Teacher-made Assessment -- 1 day
 Explain the law of conservation of mass, the law of
definite proportions, and the law of multiple
proportions.
 Summarize the five essential points of Dalton’s
atomic theory.
 Explain the relationship between Dalton’s atomic
theory and the law of conservation of mass, the law
of definite proportions, and the law of multiple
proportions.
 Summarize the observed properties of cathode rays
that led to the discovery of the electron.
 Summarize the experiment carried out by Rutherford
PS.2
PS.3
PS.4
SI.2
2 Days
1 Days
1 Day
1 Day
PS.4
PS.7
PS.8
PS.17
1 Day
2
Revised 07.08.15
Counting Atoms (Section 3)
Electron Configurations (Section
3)
4
and his co-workers that led to the discovery of the
nucleus.
 List the properties of protons, neutrons, and
electrons.
 Define atom.
 Explain what isotopes are.
 Define atomic number and mass number, and
describe how they apply to isotopes.
 Given the identity of a nuclide, determine its number of
protons, neutrons, and electrons.
 Define mole, Avogadro’s number, and molar mass,
and state how all three are related.
 Solve problems involving mass in grams, amount in
moles, and number of atoms of an element.
Chapter 3 Teacher-made Assessment -- 1 day
 List the total number of electrons needed to fully
occupy each main energy level.
 State the Aufbau principle, the Pauli exclusion
principle, and Hund’s rule.
 Describe the electron configurations for the atoms of
any element using orbital notation, electron
configuration notation, and, when appropriate, noblegas notation.
4 Days
2 Days
PS.8
PS.15
Flame Test Lab
1 Day
History of the Periodic Table
(Section 1)
5
Electron Configuration and the
Chapter 4 Teacher-made Assessment -- 1 day
 Explain the roles of Mendeleev and Moseley in the
development of the periodic table.
 Describe the modern periodic table.
 Explain how the periodic law can be used to predict
the physical and chemical properties of elements.
 Describe how the elements belonging to a group of
the periodic table are interrelated in terms of atomic
number.
 Describe the relationship between electrons in
1 Day
PS.13
PS.15
PS.16
PS.17
PS.22
1 Day
3
Revised 07.08.15
Periodic Table (Section 2)
Electron Configuration and
Periodic Properties (Section 3)
Introduction to Chemical Bonding
(Section 1)
Covalent Bonding and Molecular
Compounds (Section 2)
6
sublevels and the length of each period of the
periodic table.
 Locate and name the four blocks of the periodic table.
 Explain the reasons for these names.
 Discuss the relationship between group
configurations and group numbers.
 Describe the locations in the periodic table and the
general properties of the alkali metals, the alkalineearth metals, the halogens, and the noble gases.
 Define atomic and ionic radii, ionization energy,
electron affinity, and electronegativity.
 Compare the periodic trends of atomic radii, ionization
energy, and electronegativity, and state the reasons
for these variations.
 Define valence electrons, and state how many are
present in atoms of each main-group element.
 Compare the atomic radii, ionization energies, and
electronegativities of the d-block elements with those
of the main-group elements.
Chapter 5 Teacher-made Assessment -- 1 day
 Define chemical bond.
 Explain why most atoms form chemical bonds.
 Describe ionic and covalent bonding.
 Explain why most chemical bonding is neither purely
ionic nor purely covalent.
 Classify bonding type according to electronegativity
differences.
 Define molecule and molecular formula.
 Explain the relationships among potential energy,
distance between approaching atoms, bond length,
and bond energy.
 State the octet rule.
 List the six basic steps used in writing Lewis
structures.
2 Days
1 Day
PS.5
PS.9
PS.13
PS.16
PS.23
PS.24
PS.46
1 Day
4
Revised 07.08.15
Ionic Bonding and Ionic
Compounds (Section 3)
Chemical Names and Formulas
(Section 1)
Oxidation Numbers (Section 2)
7
Using Chemical Formulas
(Section 3)
 Explain how to determine
 Lewis structures for molecules containing single
bonds, multiple bonds, or both.
 Explain why scientists use resonance structures to
represent some molecules.
 Compare and contrast a chemical formula for a
molecular compound with one for an ionic compound.
 Discuss the arrangements of ions in crystals.
 Define lattice energy and explain its significance.
 List and compare the distinctive properties of ionic and
molecular compounds.
 Write the Lewis structure for a polyatomic ion given
the identity of the atoms combined and other
appropriate information.
Chapter 6 Teacher-made Assessment -- 1 day
 Explain the significance of a chemical formula.
 Determine the formula of an ionic compound formed
between two given ions.
 Name an ionic compound given its formula.
 Using prefixes, name a binary molecular compound
from its formula.
 Write the formula of a binary molecular compound
given its name.
 List the rules for assigning oxidation numbers.
 Give the oxidation number for each element in the
formula of a chemical compound.
 Name binary molecular compounds using oxidation
numbers and the Stock system.
 Calculate the formula mass or molar mass of any
given compound.
 Use molar mass to convert between mass in grams
and amount in moles of a chemical compound.
 Calculate the number of molecules, formula units, or
ions in a given molar amount of a chemical compound.
1 Day
1 Day
PS.5
PS.40
1 Day
2 Days
5
Revised 07.08.15
 Calculate the percentage composition of a given
chemical compound.
Chapter 7 Teacher-made Assessment -- 1 day
CUMULATIVE MIDTERM EXAM (CHAPTERS 1-7) -- 1 day
6
Revised 07.08.15
Topic
Describing Chemical Reactions
(Section 1)
Chemical Reactions Lab
Types of Chemical Reactions
(Section 2)
Third and Fourth Quarters
Chapter Outcomes
 List three observations that suggest that a chemical
reaction has taken place.
 List three requirements for a correctly written
chemical equation.
 Write a word equation and a formula equation for a
given chemical reaction.
 Balance a formula equation by inspection.
8
Introduction to Stoichiometry
(Section 1)
Ideal Stoichiometric Calculations
(Section 2)
9
 Define and give general equations for synthesis,
decomposition, single-displacement, and doubledisplacement reactions.
 Classify a reaction as a synthesis, decomposition,
single-displacement, double-displacement, or
combustion reaction.
 List three kinds of synthesis reactions and six kinds
of decomposition reactions.
 List four kinds of single-displacement reactions and
three kinds of double-displacement reactions.
 Predict the products of simple reactions given the
reactants.
Chapter 8 Teacher-made Assessment -- 1 day
 Define stoichiometry.
 Describe the importance of the mole ratio in
stoichiometric calculations.
 Write a mole ratio relating two substances in a
chemical equation.
 Calculate the amount in moles of a reactant or
product from the amount in moles of a different
reactant or product.
 Calculate the mass of a reactant or product from the
amount in moles of a different reactant or product.
 Calculate the amount in moles of a reactant or
GLEs
PS.7
PS.34
PS.35
PS.38
PS.45
Time Frame
1 Day
1 Day
2 Days
2 Day
PS.7
PS.41
PS.45
2 Days
7
Revised 07.08.15
product from the mass of a different reactant or
product.
 Calculate the mass of a reactant or product from the
mass
 of a different reactant or product.
 Describe a method for determining which of two
reactants is a limiting reactant.
 Calculate the amount in moles or mass in grams of a
product, given the amounts in moles or masses in
grams of two reactants, one of which is in excess.
 Distinguish between theoretical yield, actual yield, and
percentage yield.
 Calculate percentage yield, given the actual yield and
quantity of a reactant.

Limiting Reactants and
Percentage Yield (Section 3)
Limiting and Excess Reactant
Lab
Changes of State (Section 4)
10
Gases and Pressure (Section 1)
11
The Gas Laws (Section 2)
Chapter 9 Teacher-made Assessment -- 1 day
 Explain the relationship between equilibrium and
changes of state.
 Interpret phase diagrams.
 Explain what is meant by equilibrium vapor pressure.
 Describe the processes of boiling, freezing, melting,
and sublimation.
 Define pressure, give units of pressure, and describe
how pressure is measured.
 State the standard conditions of temperature and
pressure and convert units of pressure.
 Use Dalton’s law of partial pressures to calculate
partial pressures and total pressures.
 Use the kinetic-molecular theory to explain the
relationships between gas volume, temperature, and
pressure.
 Use Boyle’s law to calculate volume-pressure
changes at constant temperature.
2 Day
1 Day
1 Day
PS.46
1 Day
PS.29
2 Days
8
Revised 07.08.15
Gas Volumes and the Ideal Gas
Law (Section 3)
Types of Mixtures (Section 1)
The Solution Process (Section 2)
 Use Charles’s law to calculate volume-temperature
changes at constant pressure.
 Use Gay-Lussac’s law to calculate pressuretemperature changes at constant volume.
 Use the combined gas law to calculate volumetemperature-pressure changes.
 State the law of combining volumes.
 State Avogadro’s law and explain its significance.
 Define standard molar volume of a gas and use it to
calculate gas masses and volumes.
 State the ideal gas law.
 Using the ideal gas law, calculate pressure, volume,
temperature, or amount of gas when the other three
quantities are known. Reading Skill Builder
Chapter 10 & 11 Teacher-made Assessment -- 1 day
 Distinguish between heterogeneous and
homogeneous mixtures.
 List three different solute solvent combinations.
 Compare the properties of suspensions, colloids,
and solutions.
 Distinguish between electrolytes and
nonelectrolytes.
 List and explain three factors that affect the rate at
which a solid solute dissolves in a liquid solvent.
12
 Explain solution equilibrium, and distinguish among
saturated, unsaturated, and supersaturated
solutions.
 Explain the meaning of “like dissolves like” in terms
of polar and nonpolar substances.
 List the three interactions that contribute to the
enthalpy of solution, and explain how they combine
to cause dissolution to be exothermic orendothermic.
 Compare the effects of temperature and pressure on
solubility.
2 Days
1 Day
PS.14
PS.19
PS.20
1 Day
9
Revised 07.08.15
Concentration of Solutions
(Section 3)
Properties of Acids and Bases
(Section 1)
Acid-Base Theoriesm (Section 2)
14
Acid-Base Reactions (Section 3)
Aqueous Solutions and the
Concept of pH (Section 1)
15
 Given the mass of solute and volume of solvent,
calculate the concentration of a solution.
 Given the concentration of a solution, determine the
amount of solute in a given amount of solution.
 Given the concentration of a solution, determine the
amount of solution that contains a given amount of
solute.
Chapter 12 Teacher-made Assessment -- 1 day
 List five general properties of aqueous acids and
bases.
 Name common binary acids and oxyacids, given
their chemical formulas.
 List five acids commonly used in industry and the
laboratory, and give two properties of each.
 Define acid and base according to Arrhenius’s theory
of ionization.
 Explain the differences between strong and weak
acids and bases.
 Define and recognize Brønsted-Lowry acids and
bases.
 Define a Lewis acid and a Lewis base.
 Name compounds that are acids under the Lewis
definition but are not acids under the Brønsted-Lowry
definition.
 Describe a conjugate acid, a conjugate base, and an
amphoteric compound.
 Explain the process of neutralization.
 Define acid rain, give examples of compounds that
can cause acid rain, and describe effects of acid rain.
 Describe the self-ionization of water.
 Define pH, and give the pH of a neutral solution at
25°C.
 Explain and use the pH scale.
 Given [H3O+] or [OH−], find pH.
2 Days
1 Day
PS.7
PS.35
1 Day
2 Days
PS.4
PS.20
PS.31
PS.32
PS.33
1 Day
10
Revised 07.08.15
Determining pH and Titrations
(Section 2)
Titration Lab
Thermochemistry (Section 1)
Calorimeter Lab
Reaction Rates and Equilibrium
Oxidation-Reduction Reactions
Biochemistry
Nuclear Chemistry




Given pH, find [H3O+] or [OH−].
Describe how an acid-base indicator functions.
Explain how to carry out an acid-base titration.
Calculate the molarity of a solution from titration
data.

Chapter 14 & 15 Teacher-made Assessment -- 1 day
 Define temperature and state the units in which it is
measured.
 Define heat and state its units.
 Perform specific-heat calculations.
 Explain enthalpy change, enthalpy of reaction,
16
enthalpy of formation, and enthalpy of combustion.
 Solve problems involving enthalpies of reaction,
enthalpies of formation, and enthalpies of
combustion.

Chapter 16 Teacher-made Assessment -- 1 day
 Explain the five factors that influence reaction rates
Topic 1
on textbook pgs. 568-570 (Section 17.2)
(Chapters
 Explain chemical equilibrium (Section 18.1)
17 & 18)
 Explain LeChatelier’s principle (Section 18.2)
Topic 2  Define oxidation and reductions and give an
(Chapter
example of each reaction. (Section 19.1)
19)
 Determine the number of bond that carbon,
hydrogen, and oxygen can make.
Topic 3
 Distinguish among structures of alkanes, alkenes,
(Chapters
and alkynes (Section 22.2)
22 & 23)  Distinguish between structural characteristics of
hydrocarbons, carbohydrates, nucleic acids, and
proteins (Section 23.1)
Topic 4
 Describe the different types of radioactive decay
(Chapter
and their strength (Section 21.2)
2 Days
1 Day
2 Days
PS.30
PS.31
PS.44
1 Day
.5 Day
PS.37
.5 Day
PS.36
1 Day
PS.25
PS.26
PS.28
PS.45
PS.10
PS.11
1 Day
11
Revised 07.08.15
o Alpha Particle
o Beta Particle
o Gamma ray
 Solve half-life problems on pg. 689 (Section 21.2)
 Explain benefits of nuclear radiation on textbook pg.
695 (Section 21.3)
Topics 1-4 Teacher-made Assessment -- 1 day
CUMULATIVE FINAL EXAM (CHAPTERS 8-16 & 4 Topics) -- 1 day
21)
PS.12
PS.47
12