Download Chemistry Curriculum Map - Belle Vernon Area School District

Accelerated and General Chemistry Curriculum Map
Course Understandings
Essential Questions
Students will understand:
~Chemistry is the study of
matter and the changes it
undergoes.
+What are the differences
between pure substances
and mixtures?
~Atomic theory is the
foundation for the study
of chemistry.
+In what ways has the
theory of the atom changed
over time due to
technological
improvements?
~The nature of science
depends on the ability to
conduct scientific
experiments with
reproducible results.
+What are the processes in
place so that scientific
research is accurate and
reproducible?
~The metric system is the
basis of measurement in
the scientific community.
+How is the metric system
used to express scientific
values and constants?
Assessments
First Quarter
Diagnostic – Math pretest (Given before
chapter 1), Metric System Pretest (Given
before chapter 2), Scientific method
knowledge pretest (Given before chapter
3). Each posttest given after end of
chapter.
Benchmark – Study Island Pretest (Given
during Chapter 1), Physical and Chemical
Properties Test (Given during Chapter 2),
Atoms Test (Given during Chapter 3)
Formative Assessments – Ch 1 Quiz, Ch 1
Test, Ch 2 Quiz, Ch 2 Test, Ch 3 Quiz, Ch 3
Test. Informal assessments will also be
done during in class assignments,
homework, and laboratory activities.
Summative Assessments – Quarterly
Assessment #1
Course Knowledge/Skills
Standard: 3.2.C.A1 – Differentiate between physical
properties and chemical properties
Anchor: CHEM.A.1.1 – Identify and describe how
observable and measureable properties can be used to
classify and describe matter and energy.
Eligible Content: CHEM.A.1.1.2 – Classify observations as
qualitative and/or quantative.
Standard: 3.2.C.A1 – Differentiate between pure substances
and mixtures; differentiate between heterogeneous and
homogeneous mixtures
Anchor: CHEM. A.1.2 – Compare the properties of mixtures
Eligible Content
 CHEM.A.1.2.1 – Compare properties of solutions
containing ionic or molecular solutes (e.g.,
dissolving, dissociating).
 CHEM.A.1.2.2 – Differentiate between
homogeneous and heterogeneous mixtures (e.g.,
how such mixtures can be separated).
 CHEM.A.1.2.3 – Describe how factors (e.g.,
temperature, concentration, surface area) can affect
solubility.
Anchor: CHEM. A.2.1 – Explain how atomic theory serves
as the basis for the study of matter
Eligible Content
 CHEM.A.2.1.1 – Describe the evolution of the atomic
theory leading to the current model of the atom
based on the works of Dalton, Thomson, Rutherford,
and Bohr.
 CHEM.A.2.1.2 – Differentiate between the mass
number of an isotope and the average atomic mass
of an element.
Anchor: CHEM.B.1.2 – Apply the mole concept to the
composition of matter
Eligible Content CHEM.B.1.2.2 – Apply the law of definite
proportions to the classification of elements and compounds
as pure substances
Standard: 3.2.C.A3 – Describe the three normal states of
matter in terms of energy, particle motion, and phase
transitions
Anchor: CHEM. A.1.1. – Identify and describe how
observable and measureable properties can be used to
classify and describe matter and energy.
Eligible Content CHEM. A.1.1.3 – Utilize significant
figures to communicate the uncertainty in a quantative
observation.
Standard: 3.2.C.A4 – Predict how combinations of
substances can result in physical and/or chemical changes.
Anchor: CHEM.B.1.1 – Explain how the mole is a
fundamental unit of chemistry.
Eligible Content: CHEM.B.1.1.1 – Apply the mole concept
to representative particles (e.g., counting, determining mass
of atoms, ions, molecules, and/or formula units).
Standard: 3.2.C.A5 – Models – Recognize discoveries from
Dalton (atomic theory), Thomson (the electron), Rutherford
(the nucleus), and Bohr (planetary model of the atom) and
understand how each discovery leads to modern theory.
Anchor: CHEM.A.1.1 Identify and describe how observable
and measurable properties can be used to classify and
describe matter and energy.
Eligible Content: CHEM.A.1.1.1 – Classify physical or
chemical changes within a system in terms of matter and/or
energy.
Standard 3.2.C.A5 – Describe Rutherford’s “gold foil”
experiment that lead to the discovery of the nuclear atom.
Identify the major components (protons, neutrons, and
electrons) of the nuclear atom and explain how they
interact.
Anchor: CHEM.A.2.1 – Explain how atomic theory serves s
the basis for the study of matter.
Eligible Content: CHEM. A.2.1.1 – Describe the evolution
of atomic theory leading to the current model of the atom
based on the works of Dalton, Thomson, Rutherford, and
Bohr.
Students will understand:
~Chemical bonding occurs
as a result of attractive
forces between particles.
+What factors determine
the types of chemical bonds
that form between
particles?
~Periodic trends in the
properties of atoms allow
for the prediction of
physical and chemical
properties.
+How does the distribution
of electrons in atoms affect
the formation of a
compound?
~Changes in matter are
accompanied by changes
in energy
+ How are changes in matter
accompanied by changes in
energy?
Second Quarter
Diagnostic – Pretest on “The Periodic
Table” (Given before Chapter 4), Pretest
on “Bond Types” (Given before Chapter
5), Pretest on “Common Compounds”
and Naming (Given before Chapter 5).
Each posttest given after end of chapter.
Benchmark – Study Island: Systems,
Models, and Patterns (given During
Chapter 4), Energy Transformations
(Given During Chapter 5), Energy Environmental Consequences (Given
During Chapter 6)
Formative Assessment – Ch 4 Quiz, Ch 4
Test, Ch 5 Quiz, Ch 5 Test, Ch 6 Quiz, Ch 6
Test. Informal assessments will also be
done during in class assignments,
homework, and laboratory activities.
Summative Assessment – Quarterly
Assessment #2
Standard: 3.1.C.A2 – Describe how changes in energy affect
the rate of chemical reactions.
Standard: 3.2.C.A1 – Explain the relationship of an elements
position on the periodic table to its atomic number,
ionization energy, electro-negativity, atomic size, and
classification of elements.
Anchor: CHEM.A.2.1 – Explain how atomic theory serves as
the basis for the study of matter.
Eligible Content: CHEM.A.2.1.2 – Differentiate between
the mass number of an isotope and the average atomic mass
of an element.
Anchor: CHEM.A.2.3 – Explain how periodic trends in the
properties of atoms allow for the prediction of physical and
chemical properties.
Eligible Content: CHEM.A.2.3.2 – Explain how the
periodicity of chemical properties led to the arrangement of
elements on the periodic table.
Standard: 3.2.C.A1 – Use electro-negativity to explain the
difference between polar and non-polar covalent bonds.
Anchor: CHEM.A.2.3 – Explain how periodic trends in the
properties of atoms allow for the prediction of physical and
chemical properties.
Eligible Content: CHEM.A.2.3.3 – Compare and/or predict
the properties (e.g., electron affinity, ionization energy,
chemical reactivity, electronegativity, atomic radius> of
selected elements by using their locations on the periodic
table and known trends.
Anchor: CHEM.B.2.3 – Explain how atoms form chemical
bonds.
Eligible Content: CHEM.B.1.3.2 – Classify a bond as being
polar covalent, non-polar covalent, or ionic.
Standard: 3.2.C.A2 – Compare the electron configurations
for the first twenty elements of the periodic table.
Anchor: CHEM.A.2.2 – Describe the behavior of electrons
in atoms.
Eligible Content: CHEM.A.2.2.1 – Predict the ground state
electronic configurations and/or orbital diagram for a given
atom or ion.
Standard: 3.2.C.A2 – Relate the position of an element on
the periodic table to its electron configuration and compare
its reactivity to the reactivity of other elements in the table.
Anchor: CHEM.A.2.2 – Describe the behavior of electrons
in atoms.
Eligible Content: CHEM.A.2.2.2 – Predict characteristics
of an atom or an ion based on its location on the periodic
table (e.g., number of valence electrons, potential types of
bonds, reactivity.
Anchor: CHEM.A.2.2 – Describe the behavior of electrons
in atoms.
Eligible Content: CHEM.A.2.2.4 – Relate the existence of
quantized energy levels to atomic emission spectra.
Standard: 3.2.C.A2 – Explain how atoms combine to form
compounds through both ionic and covalent bonding.
Anchor: CHEM.A.1.1 – Identify and describe how
observable and measureable properties can be used to
classify and describe matter and energy.
Eligible Content: CHEM.A.1.1.4 – Relate the physical
properties of matter to its atomic or molecular structure.
Anchor: CHEM.B.1.3 – Explain how atoms for chemical
bonds.
Eligible Content: CHEM.B.1.3.1 – Explain how atoms
combine to form compounds through ionic and covalent
bonding.
Standard: 3.2.C.A2 – Predict chemical formulas based on the
number of valence electrons.
Anchor: CHEM.A.1.1 – Identify and describe how
observable and measureable properties can be used to
classify and describe matter and energy.
Eligible Content: CHEM.A.1.1.5 – Apply systematic set of
rules (IUPAC) for naming compounds and writing chemical
formulas (e.g., binary covalent binary ionic, ionic compounds
containing polyatomic ions).
Standard: 3.2.C.A2 – Draw Lewis dot structures for simple
molecules and ionic compounds.
Anchor: CHEM.A.2.2 – Describe the behavior of electrons
in atoms.
Eligible Content: CHEM.A.2.2.3 – Explain the relationship
between the electron configurations and the atomic
structure of a given atom or ion (e.g., energy levels and/or
orbitals with electrons, distribution of electrons in orbitals,
shapes of orbitals).
Anchor: CHEM.B.1.3 – Explain how atoms form chemical
bonds.
Eligible Content: CHEM.B.1.3.3 – Use illustrations to
predict the polarity of a molecule.
Anchor: CHEM.B.1.4 – Explain how models can be used to
represent bonding.
Eligible Content: CHEM.B.1.4.1 – Recognize and describe
different types of models that can be used to illustrate the
bonds that hold atoms together in a compound (e.g.,
computer models, ball-and-stick models, graphical models,
solid-sphere models, structural formulas, skeletal formulas,
Lewis dot structures).
Eligible Content: CHEM.B.1.4.2 – Utilize Lewis dot
structures to predict the structure and bonding in simple
compounds.
Standard: 3.2.C.A2 – Predict the chemical formulas for
simple ionic and molecular compounds.
Anchor: CHEM.A.1.1 – Identify and describe how
observable and measureable properties can be used to
classify and describe matter and energy.
Eligible Content: CHEM.A.1.1.5 – Apply systematic set of
rules (IUPAC) for naming compounds and writing chemical
formulas (e.g., binary covalent binary ionic, ionic compounds
containing polyatomic ions).
Standard: 3.2.C.B3 – Describe the Law of Conservation of
Energy.
Standard: 3.2.C.B3 – Explain the difference between an
endothermic process and an exothermic process.
Students will understand:
~The mole is the SI unit
for amount of a substance
and is used extensively in
chemistry.
~Chemical reactions are
predictable.
~ According to the law of
conservation of matter,
the mass of the products
in a chemical reaction is
equal to the mass of the
reactants. The amounts
of reactants and products
involved in a chemical
reaction can be predicted
using mole relationships.
Common chemical
reactions can be
categorized as synthesis,
decomposition, single
replacement, double
replacement, or
combustion.
~ A chemical reaction will
proceed until equilibrium
is reached or until a
limiting reactant is
exhausted. Dimensional
analysis is a mathematical
technique that can be
used to express
stoichiometric
+How is the mole used for
counting atoms?
+What factors identify the
types of chemical reactions?
+According to the collision
theory, what factors affect
the rate of a chemical
reaction?
+How do stoichiometric
ratios relate reactants to
products in a chemical
reaction?
Third Quarter
Diagnostic – Pretest on “Common
Reactions” (Given before Chapter 8).
Each posttest given after end of chapter.
Benchmark – Study Island: Impact of
Scientific Knowledge (Given during
Chapter 7), Chemical Reactions test
(Given During Chapter 8), Nature of
Science (Given during Chapter 9).
Formative Assessment – Ch 7 Quiz, Ch 7
Test, Ch 8 Quiz, Ch 8 Test, Ch 9 Quiz, Ch 9
Test. Informal assessments will also be
done during in class assignments,
homework, and laboratory activities.
Summative Assessment – Quarterly
Assessment #3
Standard: 3.2.C.A2 – Use the mole concept to determine
number of particles and molar mass for elements and
compounds.
Anchor: CHEM.B.1.1 – Explain how the mole is a
fundamental unit of chemistry.
Eligible Content: CHEM.B.1.1.1 – Apply the mole concept
to representative particles (e.g., counting, determining mass
of atoms, ions, molecules, and/or formula units).
Standard: 3.2.C.A2 – Determine percent compositions,
empirical formulas, and molecular formulas.
Anchor: CHEM.B.1.2 – Apply the mole concept to the
composition of matter.
Eligible Content: CHEM.B.1.2.1 – Determine the
empirical and molecular formulas of compounds.
Eligible Content: CHEM.B.1.2.3 – Relate the percent
composition and mass of each element present in a
compound.
Standard: 3.2.C.A4 – Predict how combinations of
substances can result in physical and/or chemical changes.
Standard: 3.2.C.A4 – Interpret and apply the Laws of
Conservation of Mass, Constant Composition (Definite
Proportions), and Multiple Proportions.
Anchor: CHEM.B.1.2 – Apply the mole concept to the
composition of matter
Eligible Content CHEM.B.1.2.2 – Apply the law of definite
proportions to the classification of elements and compounds
as pure substances
Standard: 3.2.C.A4 – Balance chemical equations by applying
the Law of Conservation of Mass.
Anchor: CHEM.B.2.1 – Predict what happens during a
relationships.
chemical reaction.
Eligible Content: CHEM. B.2.1.5 – Balance chemical
equations by applying the Law of Conservation of Matter.
Standard: 3.2.C.A4 – Classify chemical reactions as synthesis
(combination), decomposition, single displacement
(replacement), double displacement, and combustion.
Anchor: CHEM.B.2.1 – Predict what happens during a
chemical reaction.
Eligible Content:
 CHEM. B.2.1.3 – Classify reactions as synthesis,
decomposition, single replacement, double
replacement, or combustion.
 CHEM.B.2.1.4 – Predict products of simple chemical
reactions (e.g., synthesis, decomposition, single
replacement, double replacement, combustion).
Standard: 3.2.C.A4 – Use stoichiometry to predict quantative
relationships in a chemical reaction.
Anchor: CHEM.B.2.1 – Predict what happens during a
chemical reaction.
Eligible Content:
 CHEM. B.2.1.1 – Describe the roles of limiting and
excess reactants in chemical reactions.
 CHEM.B.2.1.2 – Use stoichiometric relationships to
calculate the amounts of reactants and products
involved in a chemical reaction.
Students will understand:
~ The physical properties
of compounds reflect the
nature of the interactions
among molecules. These
interactions are
+Considering matter in the
gaseous form, what
relationship exists between
the volume, temperature,
and pressure of the
particles?
Fourth Quarter
Diagnostic – Pretest on “Gases” (Given
before Chapter 11). Each posttest given
after end of chapter.
Benchmark – Study Island: Changes in
Systems (Given during Chapter 10),
Standard: 3.2.C.A3 – Identify the three main types of
radioactive decay and compare their properties.
Standard: 3.2.C.A3 – Describe the process of radioactive
decay by using nuclear equations and explain the concept of
half-life for an isotope.
determined by the
structure of the molecule
including the constituent
atoms. Gases can be
measured and described
by four properties:
number of particle,
pressure, temperature,
and volume.
~ The rate at which one
atom/molecule reacts
with another
atom/molecule is
influenced greatly by the
concentrations of the
reactants the reaction, the
rate of collisions between
molecules, and by the
energy needed for
atoms/molecules to react
individually or with one
another.
+ How do gas laws predict
changes in temperature,
pressure, or volume of an
ideal gas?
+ What are the four major
methods of calculating the
concentration of a solution
and how do they differ?
+ What three factors can
make the "equilibrium
position" shift?
Experimental Design (Given during
Chapter 11), Gas Behavior (Given during
Chapter 12)
Formative Assessment – Ch 10 Quiz, Ch
10 Test, Ch 11 Quiz, Ch 11 Test, Ch 12
Quiz, Ch 12 Test. Informal assessments
will also be done during in class
assignments, homework, and laboratory
activities.
Summative Assessment – Quarterly
Assessment #4
Standard: 3.2.C.A3 – Compare and contrast nuclear fission
and fusion.
Standard: 3.2.C.B2 – Explore the natural tendency for
systems to move in a direction of disorder or randomness
(entropy).
Standard: 3.2.C.A3 – Describe the three normal states of
matter in terms of energy, particle motion, and phase
transitions
Anchor: CHEM.B.2.2 – Explain how the kinetic molecular
theory relates to the behavior of gases.
Eligible Content:
 CHEM. B.2.2.1 – Utilize mathematical relationships
to predict changes in the number of particles, the
temperature, the pressure, and the volume in a
gaseous system (i.e., Boyle’s Law, Charles’s Law,
Dalton’s Law of partial pressures, the combined gas
law, and the ideal gas law).
 CHEM.B.2.2.2 – Predict the amounts of reactants
and products involved in a chemical reaction using
molar volume of a gas at STP.
Standard: 3.2.C.A1 – Differentiate between pure substances
and mixtures; differentiate between heterogeneous and
homogeneous mixtures
Anchor: CHEM. A.1.2 – Compare the properties of mixtures
Eligible Content
 CHEM.A.1.2.1 – Compare properties of solutions
containing ionic or molecular solutes (e.g.,
dissolving, dissociating).
 CHEM.A.1.2.2 – Differentiate between
homogeneous and heterogeneous mixtures (e.g.,
how such mixtures can be separated).
 CHEM.A.1.2.3 – Describe how factors (e.g.,
temperature, concentration, surface area) can affect
solubility.
 CHEM.A.1.2.4 – Describe various ways that
concentration can be expressed and calculated (e.g.,

molarity, percent by mass, percent by volume).
CHEM.A.1.2.5 – Describe how chemical bonding can
affect whether a substance dissolves in a given
liquid.