Download Honor`s Chemistry

Owosso High School
Honor’s Chemistry, Grade 10 - 12
Curriculum Map
September
Standards
 Michigan Merit
Curriculum
Content
Expectations for
Chemistry
C1.1A
C1.1C
C1.1E
C1.1g
C1.1h
C1.1i
C1.2E
C1.2f
C1.2h
C2.2B
P4.p1A
P4.p1B
P4.p1C
P4.p2A
P4.p2B
P4.p2C
P4.p2D
P5.p1A
C5.2B
C5.2C
C5.2d
C1.1B
October
November
December
January
 Michigan Merit
Curriculum Content
Expectations for
Chemistry
 Michigan Merit
Curriculum Content
Expectations for
Chemistry
 Michigan Merit
Curriculum Content
Expectations for
Chemistry
 Michigan Merit
Curriculum Content
Expectations for
Chemistry
C1.1B
C1.1D
C1.1E
C1.1g
C1.1i
C1.2h
C1.2i
C4.8A
C4.9A
C4.9b
C4.1OA
C4.10B
C4.10c
C4.10e
C1.1D
C1.1E
C1.2i
C2.4a
C2.4b
C2.4c
C2.4d
C4.8A
C4.8B
C4.8C
C4.8e
C4.8h
C4.8i
C4.10A
C4.10B
C4.8D
C4.8e
C4.8g
C4.9A
C4.9b
C4.9c
C4.10A
C4.10B
C5.5A
C5.4B
C2.2B
C3.3B
C4.3A
C4.3c
C4.3e
C4.3h
C4.3i
C4.8D
C4.8e
C4.8g
C4.9A
C4.9b
C4.10A
C5.5A
C5.4B
C5.5d
C5.5e
C4.8f
P2.p1A
P2.p1B
C2.1c
C2.2B
C3.2b
C3.3B
P4.p1A
P4.p1B
P4.p1C
C4.3A
C4.3B
C4.3c
C4.3f
C4.3g
C4.3h
C4.3i
C4.4B
P5.p1A
C5.4c
C5.4e
C5.5A
C5.5c
C5.5d
C5.5e
C4.3d
C4.2A
C4.2B
C4.2c
C4.2d
C5.4B
C5.7A
C4.2B
C4.2d
C5.2A
C5.2B
C5.7B
C4.1a
C4.1b
C4.1c
C4.6a
C4.6b
C5.2g
Course Content
 What is Chemistry
 Why study
Chemistry
 Careers with
Chemistry
 The scientific
Method
 Scientific laws
 Properties of matter
 States of matter
 Physical changes
 Classifying mixtures
 Separating mixtures
 Distinguishing
elements and
compounds
 Symbols and
formulas
 Changing reactants
to products
 Conservation of
mass
 Qualitative and
Quantitative
measurements
 Scientific notation
 Accuracy, precision,
and error
 Significant figures in
measurements
 Significant figures in
calculations
 SI units of length
 Units of volume
 Units of mass
 Determining density
 Specific gravity
 Measuring
temperature
 Temperature scales
 Conversion factors
 Converting units
 Dimensional analysis
 Early models of the
atom
 Electrons, protons,
and neutrons and
the structure of the
nuclear atom
 Atomic number
 Mass number
 Isotopes
 Atomic mass
 Development of the
periodic table
 The modern periodic
table
 The evolution of
atomic models
 The quantum
mechanical model
 Atomic orbitals
 Electron
configurations
 Exceptional electron
configurations
 Light and atomic
spectra
 The quantum
concept and the
photoelectric effect
 An explanation of
atomic spectra
 Classifying elements
by electron
configuration
 Trends in atomic
size
 Trends in ionization
energy
 Trends in ionic size
 Trends in
electronegativity
 Valence electrons
 Electron
configurations for
cations
 Electron
configurations for
anions
 Formation of ionic
compounds
 Properties of ionic
compounds
 Metallic bonds and
properties
 Crystalline structure
of metals
 Single covalent
bonds
 Double and triple
covalent bonds
 Coordinate covalent
bonds
 Exceptions to the
octet rule
 VSEPR theory
 Bond polarity
 Polar molecules
 Attraction between
molecules
 Intermolecular
attraction and
molecular properties
 Molecules and
molecular
compounds
 Ions and ionic
compounds
 Chemical formulas
 Molecular formulas
 Formula units
 The laws of definite
and multiple
proportions
 Monatomic ions
 Polyatomic ions
 Writing formulas for
binary ionic
compounds
 Naming binary ionic
compounds
 Ternary ionic
compounds
 Binary molecular
compounds
 Naming common
acids
 Word and chemical
equations
 Balancing chemical
equations
 Combination
reactions
 Decomposition
reactions
 Single-replacement
reactions
 Double replacement
reactions
 Combustion
reactions
 Predicting products
of chemical
reactions
 Net ionic equations
 Predicting the
formation of a
precipitate
 Final exam review
 The mole
 The number of
particles in a mole
 The mass of a mole
of an element
 The mass of a mole
of a compound
 The molar mass of a
substance
 The volume of a
mole of gas
 Calculating the
percent composition
of a compound
 Calculating empirical
formulas
 Calculating
molecular formulas
Skills Taught
 Define chemistry and
differentiate among
its traditional
divisions
 Describe the steps
involved in the
scientific method
 Distinguish between
a theory and a
scientific law
 Identify the
characteristics of
matter and
substances
 Differentiate among
the three states of
matter
 Define physical
property and list
several common
physical properties
of substances
 Categorize a sample
of matter as a
substance or a
mixture
 Distinguish between
homogeneous and
heterogeneous
samples of matter
 Explain the
difference between
an element and a
compound
 Differentiate
between physical
and chemical
changes in matter
 Apply the law of
conservation of
mass
 Distinguish between
quantitative and
qualitative
measurements
 Convert
measurements to
scientific notation
 Distinguish between
the accuracy,
precision, and error
of a measurement
 Identify the number
of significant figures
in a measurement
and in the result of a
calculation
 List SI units of
measurement and
common SI prefixes
 Distinguish between
the mass and weight
of an object
 Calculate the density
of an object from
experimental data
 Convert between
Celsius and Kelvin
 Summarize Dalton’s
atomic theory
 Distinguish among
protons, electrons,
and neutrons in
terms of relative
mass and charge
 Describe the
structure of an atom,
including the
location of the
protons, electrons,
and neutrons with
respect to the
nucleus
 Use the atomic
number and mass
number of an
element to subdivide
the atom into
numbers of protons,
electrons, and
neutrons
 Explain how isotopes
differ and why the
atomic masses of
elements are not
whole numbers
 Calculate the
average atomic
mass of an element
from isotope data
 Describe the origin
of the periodic table
 Identify the position
of groups, periods,
and the transition
metals in the
periodic table
 Explain the
significance of
quantized energies
of electrons as they
relate to the
quantum
mechanical model of
the atom
 Apply the Aufbau
principle, the Pauli
exclusion principle,
and Hund’s rule in
writing the electron
configurations of
elements
 Calculate the
wavelength,
frequency, or energy
of light, given two of
these values
 Explain the origin of
the atomic emission
spectrum of an
element
 Explain why you can
infer the properties
of an element based
on those of other
elements in the
 Use the periodic
table to infer the
number of valence
electrons in an atom
and draw its
electron dot
structure
 Describe the
formation of cations
from metals and
anions from
nonmetals
 List the
characteristics of an
ionic bond
 Use the
characteristics of
ionic compounds to
explain the electrical
conductivity of ionic
compounds when
melted and when in
aqueous solution
 Use the theory of
metallic bonds to
explain the physical
properties of metals
 Use electron dot
structures to show
the formation of
single, double, and
triple covalent bonds
 Describe and give
examples of
resonance
structures, and
exceptions to the
octet rule
 Use VSEPR theory
to predict the
shapes of simple
covalently bonded
molecules
 Use electronegativity
values to classify a
bond as nonpolar,
covalent, polar
covalent, or ionic
 Name and describe
the weak attractive
forces that hold
groups of molecules
together
 Distinguish between
ionic and molecular
compounds
 Define cation and
anion and relate
them to metal and
nonmetal
 Distinguish among
chemical formulas,
molecular formulas,
and formula units
 Use experimental
data to show that a
compound obeys
the law of definite
proportions
 Use the periodic
table to determine
the charge on an ion
 Define polyatomic
ion and give the
names and formulas
 Apply the rules for
naming and writing
formulas for
compounds
 Write equations
describing chemical
reactions using
appropriate symbols
 Write balanced
chemical equations
when given the
names or formulas
of the reactants and
products
 Identify a reaction as
combination,
decomposition,
single replacement,
double replacement,
or combustion
 Predict the products
of combination,
decomposition,
single-replacement,
double replacement,
and combustion
reactions
 Write and balance
net ionic equations
 Use solubility rules
to predict the solid
formed in a doublereplacement
reaction
 Describe how
Avogadro’s number
is related to a mole
of any substance
 Calculate the mass
of a mole of any
substance
 Use the molar mass
to convert between
mass and moles of
a substance
 Use the mole to
convert among
measurements of
mass, volume, and
number of particles
 Calculate the
percent composition
of a substance from
its chemical formula
and experimental
data
Honor’s Chemistry
Grade 10-12
February
Course Content
Standards
 Michigan Merit
Curriculum
Content
Expectations for
Chemistry
C5.2A
C5.2e
C5.2f
P2.p1A
P2.p1B
C2.1c
C2.2B
C2.2f
C3.3B
P4.p1A
P4.p1B
P4.p1C
C4.3A
C4.3B
C4.3c
C4.3i
C4.4a
P5.p1A
C5.4c
 Interpreting chemical
equations
 Stoichiometric
calculations
 Limiting reagents
 Calculating the
percent yield
 Kinetic theory of
gases
 Gas pressure
 Kinetic energy and
Kelvin temperature
 Kinetic theory of
liquids
 Evaporation
 Boiling point
 Kinetic theory of
solids
 Crystal structure and
unit cells
March
 Michigan Merit
Curriculum
Content
Expectations for
Chemistry
C2.2c
C4.5a
C4.5b
C4.5c
C4.4A
P2.p1A
P2.p1B
C2.1c
C2.2B
P3.p1A
C3.1d
C3.3B
C3.3c
P4.p1A
P4.p1B
P4.p2B
C4.3A
C4.3B
C4.3c
C4.3f
C4.3g
C4.4a
C4.4b
P5.p1A
C5.4c
C5.4d
C5.4e
C5.5c
 Describing a gas
 Factors affecting gas
pressure
 The gas laws
 Ideal gases
 Gas molecules:
mixtures and
movements
 Liquid water and its
properties
 Water vapor and ice
 Aqueous solutions
 Heterogeneous
aqueous systems
April
 Michigan Merit
Curriculum
Content
Expectations for
Chemistry
C3.4g
C4.6a
C4.7a
P2.p1A
P2.p1B
C2.1a
C2.1b
P3.p1A
C3.1a
C3.1b
C3.1c
C3.1d
P3.p2A
C3.4A
C3.4B
C3.4c
C3.4d
C5.4A
C5.4B
 Properties of
solutions
 Concentrations of
solutions
 Colligative properties
of solutions and
calculations
 The flow of energy –
heat
 Exothermic +
endother.
 Heat capac. + spec.
Ht.
 Calorimetry
 Thermochem.
Equation
 Heat in changes of
state
 Calculating heat
changes
May
 Michigan Merit
Curriculum
Content
Expectations for
Chemistry
C4.2A
C4.2B
C4.2c
C4.2d
C5.3c
C5.7A
C5.7C
C5.7D
C5.7g
C5.r7i
C5.7A
C5.7B
C5.7f
 Properties of acids
and bases
 Names + formulas of
acids and bases
 Hydrogen ions and
acidity
 The pH concept
 Acid – base theories
 Strengths of acids
and bases
 Neutralization
reactions
 Titration
 Equivalents and
Normality
June
 Michigan Merit
Curriculum
Content
Expectations for
Chemistry
C4.2A
C4.2B
C4.2c
C4.2d
C5.3c
C5.7A
C5.7C
C5.7D
C5.7g
C5.r7i
C5.7A
C5.7B
C5.7f
 Final exam review
over second
semester (which
includes much of
first semester, as
chemistry is
cumulative)
Skills Taught
 Changes of state
 Phase diagrams
 Sublimation
 Calculate the
amount of reactants
required or product
formed in a non
chemical process
 Interpret balanced
chemical equations
in terms of
interacting moles,
representative
particles, masses,
and gas volumes at
STP
 Use stoichiometric
principles to
calculate amounts of
reactants needed
and/or products
produced in
chemical reactions
 Calculate theoretical
yield, actual yield, or
percent yield given
appropriate
information.
 Describe the motion
of gases
 Interpret gas
pressure in terms of
kinetic energy
 Describe the nature
of liquids using
attractive forces
 Differentiate boiling
and evaporation
 Describe gas
particles properties
 Relate K temp. to KE
 Explain effects of
gas volume and
amount on pressure
 Infer effect of temp
on pressure
 State the gas laws
 Apply the gas laws
to problems
 Distinguish between
ideal and real gases
 State Avogadro’s
hypothesis, Dalton’s
law, and Graham’s
law
 Calculate moles,
masses, and
volumes of gases at
STP
 Calc. Part. Pressure
and effusion rates
 Describe Hydrogen
bonding in water
 Explain properties of
water
 Distinguish
electrolytes
 Compare solution
types
Authors: Jo Watling, Aaron Gillett
Created 10-23-08
 Identify dissolving
factors
 Solve problems in
solubility,
concentration, and
colligative properties
 Explain vapor
pressure and
colligative concepts
 Explain the
relationship between
energy and heat
 Distinguish between
heat capacity and
specific heat
 Construct heat
capacity equations
 Calculate heat
changes in chemical
+ physical Changes
 Classify the heat
changes in melting,
freezing, boiling,
condensing
 Calculate those heat
changes
 Apply Hess’s law
 Calc. heat changes
using standard
heats of formation
 List acid – base
properties
 Name acids and
bases from formulas
 Classify a solution as
acidic, basic or
neutral from
hydrogen or
hydroxide conc.
 Convert hydrogen
concentrations to pH
and hydroxide conc.
To pOH
 Compare and
contrast the acid –
base theories
 Identify conj. Acid –
base pairs
 Define strong acids
and bases
 Explain how acid –
base titration is used
to calc. the
concentration of an
acid or base
 Explain the concept
of equivalence in
neutralization
reactions
 Review of skills
taught during the
second semester (
see above )