1
Huntsville City Schools - Instructional Guide
2015 - 2016
Course: 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
QC I.A.2.a-c, e-g;
II.A.1.b
1. Distinguish between
precision and accuracy with
respect to experimental data.
Ch 3 in Pearson Chemistry;
SucessNetPlus platform
From Lab Manual:
10 days
2
Use Mathematics
and measurement in
science
appropriately.
ALCOS 1.
Differentiate among
pure substances,
mixtures, elements,
and compounds.
ALCOS 8. Distinguish
among endothermic
and exothermic
physical and
chemical changes.
(QC II.A.1.b;
II.B.1.d,e)
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. Explain density qualitatively
and solve density problems by
applying an understanding of
the concept of density.
7. Collect, organize, and
analyze data accurately and
use techniques and equipment
appropriately.
Lab -- Density Determination (1
day)
1. Distinguish between
intensive and extensive
properties of matter.
2. Contrast properties of
metals, nonmetals, and
metalloids.
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.
Ch 2, Ch 6 (metals) Ch 17 (heat), in
Pearson Chemistry; SuccessNetPlus
LTF: Foundation Lesson: Graphing
Skills-Line graph section only
Resources below from A+CR linkNature of Chemistry Unit
PowerPoints
SI units/Significant Figures Quiz
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
9 days
3
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
atomic structure,
including
photoelectric effect,
absorption and
emission spectra of
elements.
-Use the Periodic
Table to write
electron
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. Describe the historical
development of the modern
periodic table, including work
by Mendeleev and then
Moseley
7. Describe and explain the
organization of elements into
periods and groups in the
periodic table
Ch 4, 5, 6 in Pearson Chemistry;
SuccessNetPlus
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: Do’s and Don’ts of Periodic
Principles- teacher resource
15 days
1 day for
Benchmark
Review
1 day for
Benchmark
Assessment
4
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)
5
2nd Nine Weeks
Standard
“I Can” Statements
Resources
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)
1. Describe the characteristics
of ionic and covalent bonding
2. Describe the nature of the
chemical bond with respect to
valence electrons in bonding
atoms
3. Explain how ionic and
covalent compounds differ
4. Use Lewis dot diagrams to
represent bonding in covalent
compounds
5. Draw Lewis structures for
molecules and polyatomic
ions.
Ch 7, 8 Pearson Chemistry; SuccessNet
Plus
ALCOS 3. Utilize
electron
configuration, Lewis
dot structures, and
orbital notation to
write chemical
formulas.
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
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
Ch 9 in Pearson Chemistry;
SuccessNetPlus
8 days
**Ion Sheet
Regular Chemistry should not memorize
ions but use the Ion Sheet as a
reference page
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
ALCOS 6. Solve
stoichiometric
problems involving
relationships among
the number of
particles, moles, and
masses of reactants
1. Explain how conservation
laws form the basis for
balancing chemical reactions
and know what quantities are
conserved in physical and
chemical changes
Ch 11 in Pearson Chemistry;
SuccessNetPlus
20 days
2 days for
Benchmark
Review
7
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)
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
From A+CR link above- Chemical
Reactions Unit:
student activities, teacher demos,
assessments
Types of Reactions Lab (lab
manual)- modify for Chemistry
1 day for
Benchmark
Assessment
8
3rd Nine Weeks
Standard
“I Can” Statements
Resources
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
Ch 10 in Pearson Chemistry;
SuccessNetPlus
ALCOS 6. Solve
stoichiometric
problems involving
relationships among
the number of
1.Use chemical equations to
perform basic mole-mole,
mass-mass, and mass-mole
computations for chemical
reactions
Ch 3 (% error) and 12 in Pearson
Chemistry; SuccessNetPlus
Pacing
Recommendation
10 days
From A+CR from link aboveComposition Stoichiometry Unit:
Activities
PowerPoints
Chalk Talk activity
% Sugar in Gum (ASIM) in Unit 1 of
A+CR link
13 days
9
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)
2. Compute theoretical yield,
actual (experimental) yield,
and percent yield
3. Calculate percent error
From A+CR link above- Reaction
Stoichiometry unit:
Stoichiometry PowerPoint
Student homework
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
4. Use the kinetic molecular
theory to explain the states
Ch 13 and 7, 8 (IMFs, solids) in Pearson
Chemistry; SuccessNetPlus
From A+CR link above in States of
Matter unit:
Assessments, activities with graphs
LTF- Don’t Flip Your Lid Lab
9 days
10
and properties (i.e.,
microscopic and macroscopic)
of matter and phase changes
5. Compare the different types
of intermolecular forces.
6. Describe the unique
physical and chemical
properties of water resulting
from hydrogen bonding
7. Explain the relationship
between intermolecular
forces, boiling points, and
vapor pressure when
comparing differences in the
properties of pure substances
8. 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
Ch 13, 14 in Pearson Chemistry;
SuccessNetPlus
Cover the gas portion of Ch 13 and
sections 1 and 2 of Ch 14 in the 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
11
4. Predict boiling point
changes based on changes in
atmospheric pressure
12
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. 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.
3. Apply the mathematical
relationships that exist among
the volume, temperature,
pressure, and number of
particles in an ideal gas
Ch 14 in Pearson Chemistry;
SuccessNetPlus platform
ALCOS 4. Describe
solutions in terms of
energy changes,
solubility,
conductivity, and
concentration
1. Define solution, solute, and
solvent
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
Ch 15, 16 (solubility rules in Ch 11) in
Pearson Chemistry; SuccessNetPlus
ALCOS 5. Describe
the factors affecting
the solubility of a
solute in a given
solvent and its rate
of solution.
Resources
Pacing
Recommendation
8 days
From A+CR link above- States of
Matter Unit:
Guided reading note pages,
activities
10 days
From A+CR link:
http://www.apluscollegeready.org
/teachers
Solutions Unit- PowerPoint; notes;
homework; solubility curve;
assessments
13
(QC V.A.1.a-l;
V.A.2.a-c)
6. Describe the preparation
and properties of solutions
7. Describe the relationship
between temperature or
pressure and the solubility of
gases in liquids
8. Describe the relationship
between solvent character and
solute character and explain
miscibility
9. Apply the general rules of
solubility to aqueous salt
solutions
10. Describe the factors
affecting the solubility of a
solute in a given solvent and
its rate of solution
11. Describe qualitatively the
effect of adding solute on
freezing point, boiling point,
and vapor pressure of a
solvent
12. Define molality
13. Calculate changes in the
boiling point and freezing
point when nonvolatile,
nonelectrolyte solutes are
added to solvents
14. Predict the products of
double replacement reactions,
identify precipitates using
given solubility rules
Supersaturation Lab (Lab Manual)
14
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. Define the water constant,
Kw, and the pH scale
5. Describe characteristics of
strong and weak acids and
bases, and identify common
examples of both
6. Write and balance a simple
equation for a neutralization
reaction
7. Calculate hydrogen ion
concentration, hydroxide ion
concentration, pH, and pOH
for acidic or basic solutions
Ch 19 in Pearson Chemistry;
SuccessNetPlus
ALCOS 9. Distinguish
between chemical
and nuclear
reactions.
(QC V.E.a,b)
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
reactions and compare the
resulting radiation with regard
to penetrating ability
3. Calculate half-life of
radioactive isotopes.
Ch 25 in Pearson Chemistry;
SuccessNetPlus
10 days
From A+CR link- Acids and Bases
Unit:
Assessments, notes, activities
From A+CR link above: look in Unit
2 Structure of Matter
4 days
15
ALCOS 2. Describe
the structure of
carbon chains,
branched chains,
and rings.
(QC IV.B.3.e)
1. Describe the unique
features of bonding in carbon
compounds
2. Draw structural formulas
and their isomers along with
naming them using IUPAC
nomenclature.
Ch 22 in Pearson Chemistry;
SuccessNetPlus
ALCOS 8. Use
LeChatelier’s
Principle to explain
changes in physical
and chemical
equilibrium.
1. Apply Le Châtelier’s
principle to explain a variety
of changes in physical and
chemical equilibria
Ch 18 in Pearson Chemistry;
SuccessNetPlus
4 days
Molecular model kit for demos
2 days
2 days for
Exam Review