1
Huntsville City Schools - Instructional Guide
2015 - 2016
Course: Honors Chemistry Grades: 10-12
1st Nine Weeks
Standard
“I Can” Statements
Resources
Scientific Process
and Application
Skills
QC I.A.1.f
Safely use
laboratory
equipment and
techniques when
conducting scientific
investigations.
1. Identify the location and
function of safety equipment
in the lab.
2. Apply laboratory safety
rules.
3. Identify and properly use
laboratory equipment.
4. Obtain a score of 90 or
above on the Lab Safety Test.
5. Collect and organize data
accurately and use techniques
and equipment appropriately.
**See ion sheet note with Nomenclature
(chapter 6)
Pacing
Recommendation
7 days
http://www.apluscollegeready.org
/teachers
(Scroll down to Pre-AP Chemistry
link for resources)
In Nature of Chemistry Unit:
PPT: Lab Safety
PDF: Safety Contract/Rules
PPT: Lab Equipment
Lab safety Test
From Lab Manual:
Lab – Using Lab
Equipment/Techniques (2 days)
Scientific Process
and Application
Skills
1. Distinguish between
precision and accuracy with
respect to experimental data.
Ch 2 in Timberlake; in
MasteringChemistry.com- PPT:
Measurements
10 days
2
QC I.A.2.a-c, e-g;
II.A.1.b
Use Mathematics
and measurement in
science
appropriately.
ALCOS 1.
Differentiate among
pure substances,
mixtures, elements,
and compounds.
2. Use appropriate SI units
and convert between SI unit
prefixes.
3. Use the correct number of
significant figures in reporting
measurements in laboratory
and the results of calculations
4. Express numbers in
scientific notation when
appropriate
5. Solve for unknown
quantities by manipulating
variables
6. Use graphical,
mathematical, and/or
statistical models to express
patterns and relationships
inferred from sets of scientific
data
7. Explain density qualitatively
and solve density problems by
applying an understanding of
the concept of density.
8. Collect, organize, and
analyze data accurately and
use techniques and equipment
appropriately.
9. Interpret results and draw
conclusions as to the identity
of an unknown metal based on
its density.
1. Distinguish between
intensive and extensive
properties of matter.
2. Contrast properties of
metals, nonmetals, and
metalloids.
From Lab Manual:
Lab -- Density Determination (1
day)
LTF: Foundation Lesson: Graphing
Skills-Line graph section only
LTF: Dimensional Analysisproblems
Resources below from A+CR linkNature of Chemistry Unit
PowerPoints
SI units/Significant Figures Quiz
Ch 3 in Timberlake text;
MasteringChemistry.com
9 days
3
ALCOS 8. Distinguish
among endothermic
and exothermic
physical and
chemical changes.
(QC II.A.1.b;
II.B.1.d,e)
ALCOS 9. Identifying
atomic and
subatomic particles.
ALCOS 3.
Use the periodic
table to identify
periodic trends,
including atomic
radii, ionization
energy,
electronegativity,
and energy levels.
-Calculating the
number of protons,
neutrons, and
electrons in an
isotope.
-Utilizing benchmark
discoveries to
describe the
historical
development of
3. Distinguish between
homogeneous and
heterogeneous forms of
matter.
4. Describe physical and
chemical changes in terms of
endothermic and exothermic
processes.
5. Compare chemical and
physical properties of matter.
6. Differentiate between
chemical and physical changes
of matter.
7. Calculate temperature
change by using specific heat.
1. Compare characteristics of
isotopes of the same
elements.
2. Describe the crucial
contributions of scientists and
the critical experiments that
led to the development of the
modern atomic
model
3. Describe atomic orbitals (s,
p, d, f) and their basic shapes
4. Apply Hund’s rule and the
Aufbau process to specify the
electron configurations and
orbital notations of the
elements.
5. Describe characteristics of a
wave, such as wavelength,
frequency, energy, and speed.
6. Use electron configurations
of elements to explain the
trends and periodic properties.
Chemical and Physical Changes Lab
(Lab manual) Chemistry amend as
needed
From A+CR link- Nature of
Chemistry Unit:
PPT: Classification of Matter
PPT: properties and changes of
matter
Identification of an Unknown metal
as a teacher Demo
Assessments
Ch 4, 5 in Timberlake text;
MasteringChemistry.com
From A+CR link- Structure of
Matter Unit:
PPT: History of PT
PPT: Chemical Families
PPT: Atomic structure
PPT: Wave-particle nature
PPT: orbital notation
PPT: Periodic Trends
Flame Test Lab (Lab manual)
LTF: Electron Configuration, orbit
al notation and quantum numbers
LTF: Do’s and Don’ts of Periodic
Principles- teacher resource
15 days
1 day for
Benchmark
Review
1 day for
Benchmark
Assessment
4
atomic structure,
including
photoelectric effect,
absorption and
emission spectra of
elements.
-Use the Periodic
Table to write
electron
configurations and
orbital notations.
ALCOS 1. Contrast
properties of metals,
nonmetals, and
metalloids.
(QC II.A.2.c;
IV.B.1.a-f;
IV.B.2.a-g)
7. Describe the historical
development of the modern
periodic table, including work
by Mendeleev and then
Moseley
8. Describe and explain the
organization of elements into
periods and groups in the
periodic table
5
2nd Nine Weeks
Standard
ALCOS 6.
Solve stoichiometric
problems involving
relationships among
the number of
particles, moles, and
masses of reactants
and products in a
chemical reaction.
Predicting covalent
and ionic bond
types.
(QC IV.B.3.a-d)
ALCOS 3. Utilize
electron
configuration, Lewis
dot structures, and
orbital notation to
write chemical
formulas.
“I Can” Statements
1. Describe the characteristics
of ionic and covalent bonding
2. Explain ionic stability,
recognize typical ionic
configurations, and predict
ionic configurations for
elements (e.g., electron
configurations, Lewis dot
models)
3. Describe the nature of the
chemical bond with respect to
valence electrons in bonding
atoms
4. Explain how ionic and
covalent compounds differ
5. Use Lewis dot diagrams to
represent bonding in covalent
compounds
6. Draw Lewis structures for
molecules and polyatomic
ions, including those that must
be represented by a set of
resonance
structures
7. Use VSEPR theory to explain
geometries of molecules and
polyatomic ions
Resources
Ch 10 sections 1-3 in Timberlake
text;
MasteringChemistry.com
From A+CR link above- Bonding
and Nomenclature Unit:
Chemical Bonding PowerPoint
LTF: Molecular Geometry
Covalent Molecules Lab (Lab
Manual)
[Intermolecular Forces will be
covered with States of Matter
during 2nd semester]
Pacing
Recommendation
9 days
6
8. Describe how orbital
hybridization models relate to
molecular geometry
9. Describe the relationship
between molecular polarity
and bond polarity
ALCOS 6. Solve
stoichiometric
problems involving
relationships among
the number of
particles, moles, and
masses of reactants
and products in a
chemical reaction.
Identifying the
nomenclature of
ionic compounds,
binary compounds,
and acids.
(QC III.A.1.a-d;
IV.B.3.a,d)
1. Distinguish between
chemical symbols, empirical
formulas, molecular formulas,
and structural formulas
2. Interpret the information
conveyed by chemical
formulas for numbers of atoms
of each element represented
3. Use the names, formulas,
and charges of commonly
referenced polyatomic ions
4. Provide the interconversion
of molecular formulas,
structural formulas, and
names, including common
binary and ternary acids
Ch 6 in Timberlake text;
Masteringchemistry.com
**Ion Sheet (We encourage Honors
students to start learning ions
many weeks before the topic is
taught. One strategy is for students
to make notecards and take quizzes
over several weeks prior to this
chapter.)
From A+CR linkBonding/Nomenclature unit:
student activities
LTF: Chemical Nomenclature
Lesson- Use templates to as group
activity. HW- Table C
Quality Core- module 14- student
nomenclature practice
8 days
7
ALCOS 6. Solve
stoichiometric
problems involving
relationships among
the number of
particles, moles, and
masses of reactants
and products in a
chemical reaction.
Classifying chemical
reactions. Assign
oxidation numbers
for individual atoms
of monatomic and
polyatomic ions.
(QC II.B.1.a;
III.A.3.a-h; V.D.a-c)
1. Explain how conservation
laws form the basis for
balancing chemical reactions
and know what quantities are
conserved in physical and
chemical changes
2. Write and balance chemical
equations, given the names of
reactants and products
3. Describe what is
represented, on a molecular
and molar level, by chemical
equations
4. Use the appropriate
symbols for state (i.e., solid,
liquid, gaseous, aqueous) and
reaction direction when
writing chemical
equations
5. Classify chemical reactions
as being synthesis,
decomposition, single
replacement, or double
replacement reactions
6. Predict the products of
synthesis, combustion, and
decomposition reactions and
write balanced equations for
these reactions
7. Predict products of single
replacement reactions, using
the activity series, and write
balanced equations for these
reactions
8. Predict the products of
double replacement reactions,
and write balanced equations
for these reactions
Ch 8 in Timberlake text;
Masteringchemistry.com and
activity series is in Ch 15 p.534.
From A+CR link above- Chemical
Reactions Unit:
student activities, teacher demos,
assessments
Suggestion: Give a test on 4 types
of reactions and separate quiz or
test on redox
Types of Reactions Lab (lab
manual)- modify for Chemistry
LTF- OIL RIG lesson
20 days
2 days for
Benchmark
Review
1 day for
Benchmark
Assessment
8
9. Define redox reaction,
oxidation, and reduction.
10. Assign oxidation numbers
to reaction species.
11. Identify what is oxidized
and reduced.
12. Balance a redox reaction
using the half reaction
method.
9
3rd Nine Weeks
Standard
“I Can” Statements
ALCOS 6. Solve
stoichiometric
problems involving
relationships among
the number of
particles, moles, and
masses of reactants
and products in a
chemical reaction.
Solve problems
involving
relationships among
number of particles,
moles, and masses
of atoms in
compounds.
(QC III.A.2.a,b;
III.A.1.e,f)
1. Explain the meaning of mole
and Avogadro’s number
2. Interconvert between mass,
moles, and number of particles
3. Distinguish between
formula mass, empirical mass,
molecular mass, gram
molecular mass, and gram
formula mass.
4. Calculate the percent
composition of a substance,
given its formula or masses of
each component element in a
sample
5. Determine the empirical
formulas and molecular
formulas of compounds, given
percent composition data or
mass composition data
6. Determine percent
composition experimentally
and derive empirical formulas
from the data (e.g., for
hydrates)
ALCOS 6. Solve
stoichiometric
problems involving
relationships among
1.Use chemical equations to
perform basic mole-mole,
mass-mass, and mass-mole
Resources
Ch 7 in Timberlake text;
Masteringchemistry.com
Pacing
Recommendation
10 days
From A+CR from link aboveComposition Stoichiometry Unit:
Activities
PowerPoints
Chalk Talk activity
Labquestion.pptx in Reaction
Stoichiometry unit.
% Sugar in Gum (ASIM) in Unit 1 of
A+CR link
Ch 9 in Timberlake text;
Masteringchemistry.com
13 days
10
the number of
particles, moles, and
masses of reactants
and products in a
chemical reaction.
Solve stoichiometric
problems involving
relationships
between reactants
and products in a
chemical reaction.
(QC III.A.3.j-l)
computations for chemical
reactions
2. Identify limiting reagents
and use this information when
solving reaction stoichiometry
problems
3. Compute theoretical yield,
actual (experimental) yield,
and percent yield
4. Calculate percent error and
analyze experimental errors
that affect percent error
5. Calculate the heat of
reaction for a given chemical
reaction when given
calorimetric data.
ALCOS 5. Use the
kinetic molecular
theory to explain
states of matter and
phase changes.
(QC II.B.1.b,c;
IV.A.1.a; IV.A.2.a;
IV.B.3.f-k)
1.Describe how matter is
classified by state of matter
and by composition
2. Describe the phase and
energy changes associated
with boiling/condensing,
melting/freezing, sublimation,
and crystallization.
3. Describe differences
between solids, liquids, and
gases at the atomic and
molecular levels
From A+CR link above- Reaction
Stoichiometry unit:
Stoichiometry PowerPoint
Student homework
LTF- Exploring Molar Relationships
Ch 10 in Timberlake Text (already
completed sections 1-3) Teach
section 4 (IMFs) and 5 (Solids and
Liquids- this section is VERY lacking
in details-MUST supplement for
properties of solids and liquids)
Ch 11 pages 367-368- for Vapor
Pressure and Boiling Point
From A+CR link above in States of
Matter unit:
Assessments, activities with graphs
9 days
11
4. Use the kinetic molecular
theory to explain the states
and properties (i.e.,
microscopic and macroscopic)
of matter and phase changes
5. Compare the different types
of intermolecular forces.
6. Explain and provide
examples for dipole moments,
bond polarity, and hydrogen
bonding
7. Describe the unique
physical and chemical
properties of water resulting
from hydrogen bonding
8. Explain the relationship
between intermolecular
forces, boiling points, and
vapor pressure when
comparing differences in the
properties of pure substances
9. Classify solids as ionic,
molecular, metallic, or
network
ALCOS 7. Explain the
behavior of ideal
gases in terms of
pressure, volume,
temperature, and
number of particles
using the gas laws.
(QC II.B.2.a-d)
1. Define gas pressure and the
various pressure units (e.g.,
torr, kilopascals, mm Hg,
atmospheres)
2. Describe the use and
operation of mercury
barometers and manometers
to find atmospheric pressure
or relative gas pressures
3. Define the gas laws given
by Boyle, Charles, Gay-Lussac,
and Dalton and solve problems
based on these laws
LTF- Don’t Flip Your Lid Lab
Ch 11 in Timberlake Text;
Masteringchemistry.com
Sections 1-6 are covered during 3rd
9 weeks.
From A+CR link above- States of
Matter Unit:
Guided reading note pages,
activities
LTF- Boyle’s Law and Practice using
Gas Laws
8 days
1 day for
Benchmark
Review
1 day for
Benchmark
Assessment
12
4. Use the kinetic-molecular
theory as a basis for
explaining gas pressure,
Avogadro’s hypothesis, and
Boyle’s/Charles’s laws
5. Predict boiling point
changes based on changes in
atmospheric pressure
13
4th Nine Weeks
Standard
“I Can” Statements
ALCOS 7. Explain the
behavior of ideal
gases in terms of
pressure, volume,
temperature, and
number of particles
using the gas laws.
(QC II.B.2.e,f;
II.B.3.a-e)
1. Explain the basis for
gaseous diffusion and
effusion.
2. Describe Avogadro’s
hypothesis and use it to solve
stoichiometric problems
3. Explain the difference
between an ideal and real gas,
the assumptions made about
an ideal gas, and what
conditions favor ideal behavior
for a real gas.
4. Apply the mathematical
relationships that exist among
the volume, temperature,
pressure, and number of
particles in an ideal gas
5. Compute gas density when
given molar mass,
temperature, and pressure
6. Apply the ideal gas law to
determine the molar volume of
a volatile compound
7. Solve gas stoichiometry
problems at standard and
nonstandard conditions.
1. Define solution, solute, and
solvent
ALCOS 4. Describe
solutions in terms of
energy changes,
Resources
Ch 11, sections 7-10 in Timberlake
Text; Masteringchemistry.com
Pacing
Recommendation
8 days
From A+CR link above- States of
Matter Unit:
Guided reading note pages,
activities
Molar Volume of a Gas Lab- Lab
manual
10 days
14
solubility,
conductivity, and
concentration
ALCOS 5. Describe
the factors affecting
the solubility of a
solute in a given
solvent and its rate
of solution.
(QC V.A.1.a-l;
V.A.2.a-c)
2. Compare properties of
suspensions, colloids, and true
solutions
3. Define the terms saturated,
unsaturated, supersaturated,
dilute, and concentrated as
they pertain to solutions
4. Give examples of solid,
liquid, or gas medium
solutions
5. Define and calculate the
molarity of a solution
6. Define and calculate the
percent composition of a
solution (percent by mass and
mole fraction).
7. Describe the preparation
and properties of solutions
8. Solve stoichiometry
calculations based on
reactions involving aqueous
solutions
9. Describe the relationship
between temperature or
pressure and the solubility of
gases in liquids
10. Describe the relationship
between solvent character and
solute character and explain
miscibility
11. Apply the general rules of
solubility to aqueous salt
solutions
12. Describe the factors
affecting the solubility of a
solute in a given solvent and
its rate of solution
Ch 12 in Timberlake text (skip
Osmotic pressure); PowerPoints in
masteringchemistry.com
(Mole fraction is not in the text- can
use LTF lesson “solution basics” for
info)
From A+CR link:
http://www.apluscollegeready.org
/teachers
Solutions Unit-Better list of
solubility rules than in Timberlake
text; PowerPoint; notes;
homework; solubility curve;
assessments
LTF- Colligative Properties
Supersaturation Lab (Lab Manual)
15
13. Describe qualitatively the
effect of adding solute on
freezing point, boiling point,
and vapor pressure of a
solvent
14. Define molality and mole
fraction
15. Calculate changes in the
boiling point and freezing
point when nonvolatile,
nonelectrolyte solutes are
added to solvents
16. Predict the products of
double replacement reactions,
identify precipitates using
given solubility rules, and
write balanced equations for
these reactions
17. Write net ionic equations,
identifying spectator ions, and
the net ionic equation.
ALCOS 4. Describe
acids and bases in
terms of strength,
concentration, pH,
and neutralization
reactions.
(QC III.A.1.d;
V.B.1.h)
1. Describe the nature and
interactions of acids and bases
2. Describe the hydronium ion
and the concept of
amphoterism
3. Describe Arrhenius and
Brønsted-Lowry acids and
bases; identify conjugate acids
and bases in reactions
4. Relate solvent interaction to
the formation of acidic and
basic solutions
5. Define the water constant,
Kw, and the pH scale
6. Describe characteristics of
strong and weak acids and
Ch 14 in Timberlake Text;
masteringchemistry.com
From Ch 13 refer to writing
equilibrium expressions
From A+CR link- Acids and Bases
Unit:
Assessments, notes, activities
Titration Lab- Lab Manual
10 days
16
ALCOS 9. Distinguish
between chemical
and nuclear
reactions.
(QC V.E.a,b)
bases, and identify common
examples of both
7. Write and balance a simple
equation for a neutralization
reaction
8. Calculate hydrogen ion
concentration, hydroxide ion
concentration, pH, and pOH
for acidic or basic solutions
9. Explain how the acid-base
indicators work
10. Define percent ionization,
Ka, and Kb and explain how
they relate to acid/base
strength
11. Conduct a titration
experiment in order to
determine the concentration
of an acid or base solution
12. Qualitatively understand
the behavior of a buffer and
explain why buffer solutions
maintain pH upon dilution
13. Explain the law of mass
action and write equilibrium
law expressions for chemical
equilibria.
14. Define percent ionization,
Ka, Kb and explain how they
relate to acid/base strength.
1. Describe alpha, beta, and
gamma decay, carbon-14
dating, and fission and fusion
2. Write appropriate equations
for nuclear decay reactions,
using particle balance;
describe how the nucleus
changes during these
From A+CR link above: look in Unit
2 Structure of Matter
4 days
17
ALCOS 2. Describe
the structure of
carbon chains,
branched chains,
and rings.
(QC IV.B.3.e)
ALCOS 8. Use
LeChatelier’s
Principle to explain
changes in physical
and chemical
equilibrium.
ALCOS 8. Distinguish
among endothermic
and exothermic
physical and
chemical changes.
ALCOS 5. Use the
kinetic theory to
explain chemical
reactions.
(QC V.B.1.a-f)
reactions and compare the
resulting radiation with regard
to penetrating ability
3. Calculate half-life of
radioactive isotopes.
1. Describe the unique
features of bonding in carbon
compounds
2. Draw structural formulas
and their isomers along with
naming them using IUPAC
nomenclature.
1.Explain the collision theory
of reactions
2. Analyze factors (e.g.,
temperature, nature of
reactants) affecting reaction
rates in relation to the kinetic
theory
3. Relate reaction mechanism,
rate-determining step,
activated complex, heat of
reaction, and activation
energy to reaction kinetics
4. Interpret potential energy
diagrams for chemical
reactions
5. Describe the conditions that
define equilibrium systems on
a dynamic molecular level and
on a static macroscopic scale
6. Apply Le Châtelier’s
principle to explain a variety
of changes in physical and
chemical equilibria
Ch 17 (section 1) in Timberlake
text; masterchemistry.com
4 days
Molecular model kit for demos
Ch 13 (sections 1,2,5) in
Timberlake text;
masteringchemistry.com
From A+CR link:
Look under “AP Lite” unit.
Enthalpykineticslechatelier.ppt
Kinetics begins at slide 12
2 days
2 days for
Exam Review
18