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Accelerated Chemistry 2003-2004 Curriculum Plan
Text: Chemistry: Connections to Our Changing World, LeMay, et al., 2002
Topic
Scientific
Processes
Mathematical
applications
Safety
Energy & Matter
Chapter 2
Atomic Structure
Chapters 3 and 24
Electron
Configuration
Chapter 4
Periodic Table
Chapters 5 and 6
Skills
NJCCS
Critical thinking and analysis; Collaboration, peer review;
Inquiry and problem solving; observation and data collection,
inference
Critical thinking and analysis; Collaboration, peer review;
Inquiry and problem solving. Graphing, use of ESA (equation
– substitution – answer) methodology, data analysis, statistics.
Understand Accuracy, Precision / Uncertainty, Dimensional
Analysis, Significant Figures, Exponents, SI (Metric)
relationships and conversions
Understand and agree to lab safety rules; identify and know
how to use safety equipment
Understand: Definitions, the Laws of Conservation of Energy
and of Conservation of Matter, Temperature scales and
conversions, Chemical and physical changes, Classifying
Matter, Chemical and physical properties
Understand the evolution of atomic models, Components of
atomic structure (electrons, protons, and neutrons, including
location, relative mass and relative electric charge). Define
isotopes and use isotope notation, Write nuclear equations to
represent types of nuclear changes, Define half-life and solve
related problems including carbon dating, Distinguish between
nuclear and chemical reactions using atomic mass units,
Understand that the strong nuclear force holds the nucleus
together, Recognize biological effects of radiation, Define
fission and fusion and write nuclear equations to represent
each, Understand the basic components of a nuclear reactor
Describe the relationships among wavelength, frequency,
velocity and energy, Recognize that the speed of light is a
constant and the value of that constant, Describe the regions of
the electromagnetic radiation (EMR) spectrum, Relate the line
spectrum of hydrogen to the EMR spectrum and to other
atoms, Distinguish between quantized and continuous
systems, Describe the Bohr atomic model and its limitations,
Contrast the quantum mechanic model to other previous
atomic models, Write electron configurations using the
Aufbau Principle, Hund’s Rule, and the Pauli Exclusion
Principle
Identify groups / families and periods, Identify the
representative families and the similarities and differences in
their electron configurations, Use periodic patterns and trends
to organize elements within a period or group
5.1.A
5.1.B
5.4.A
5.3.A
5.3.B
5.3.D
5.1.C.1
5.7.A
5.7.A.1
5.7.A.2
5.7.A.6
5.7.A.3
5.7.A.8
5.7.A.5
September 2, 2003
Page 1 of 4
Topic
Chemical
Formulas and
Chemical Bonding
Chapter 7
Molecular Shapes
Chapter 8
Chemical
Reactions and
Equations
Chapter 9
The Mole,
introduction to
Stoichiometry
Chapter 10
Stoichiometry and
Limiting Reactants
Chapter 11
Skills
NJCCS
Distinguish between ionic and covalent chemical bonding,
5.7.A.4
Identify general properties of ionic compounds and of
5.7.A.7
covalent compounds, Use electron dot diagrams to represent
ionic and covalent bonding in formula units and molecules,
Recognize types of ions: cation and anion, monatomic and
polyatomic, Write formulas for and name ionic compounds,
Write formulas for and name covalent compounds,
Distinguish between molecular and empirical formulas,
Describe and illustrate multiple covalent bonds, Describe the
cause of polar and nonpolar covalent bonds and identify
molecules containing each, Apply electronegativity concepts
to predict the type of chemical bond between two atoms
Use Ball and Stick models to construct simple molecules,
5.7.A.7
Draw and describe the shape of simple molecules, Apply the
VSEPR (valence-shell electron pair repulsion) Theory to
explain hybrid orbitals, Identify Intermolecular Attractive
Forces (IMAF) (revisited in chapter 14)
Writing unbalanced formula equations when given a word
5.7.B
equation, Writing a balanced equation when given and
unbalanced formula equation, Writing a balanced equation
when given a word equation, Correctly use all four state
symbols, Classifying equations as synthesis, decomposition,
single replacement, double displacement, and combustion
reactions, Classifying reactions as acid/base, redox (oxidationreduction), precipitation
Define a mole in terms of Avogadro’s number, Define a mole
5.7.A
in terms of molar mass, Convert between number of moles,
mass, and number of particles, Describe molar volume of a
gas (that one mole of any ideal gas occupies 22.4 L at
Standard temperature and pressure - STP), Use molar volume
of a gas at STP to convert between number of particles, mass,
and number of moles, Calculate percent composition from a
chemical formula, Use percent composition to determine
empirical formula, Differentiate molecular and empirical
formulas, Find the empirical formula associated with a
molecular formula, Find a molecular formula given a molar
mass and an empirical formula
Define stoichiometry, Use stoichiometry to make conversions
5.7.B
using balanced chemical equations: moles A  moles B, mass
A  moles B, moles A  mass, mass A  mass B,
Define the concept of a limiting reactant in terms of chemical
reactions and everyday applications, Make any of the above
conversions using limiting reactants, Hypothetical situations:
calculate how much of the excess reactant was left over, how
much more of a product could have been produced, how much
more limiting reactant would need to be added, etc.
September 2, 2003
Page 2 of 4
Topic
Skills
NJCCS
Thermochemistry,
Thermodynamics
and Kinetics
Distinguish exothermic and endothermic reactions, Define
enthalpy, change in enthalpy and how they are used in
equations, Define standard conditions for standard enthalpy
change and its notation, State Hess’s law, Use Hess’s law to
find Ho for a reaction, Describe the process of calorimetry,
Define rate of reaction, Identify intermediate products of a
reaction, Describe a rate law for a chemical reaction, Describe
collision theory and relate how it describes the reaction rate,
Describe the factors that affect reaction rate in terms of
collision theory, Explain the concept of activation energy and
activated complex, Define entropy, Describe an increase in the
entropy of the universe as a driving force (2nd law of
thermodynamics), Create and recognize an energy diagram for
an exothermic or endothermic reaction, including EA, Ho,
enthalpy of products and enthalpy of reactants, Use the Gibbs
free energy equation (G = H - TS) to calculate G.
Decide whether a reaction is spontaneous if only the sign of
Ho and S are given
Describe the kinetic molecular theory (KMT) and use the
KMT to describe the behavior of gases, Describe changes in
pressure, temperature and volume on a molecular level in
terms of the KMT, Define gas pressure and describe its
measurement, State and use the gas laws to predict properties
of ideal gases both quantitatively and qualitatively:
PV = nRT, PV = k, V/T = k, V/n = k. PTOT = Pa + Pb …
Compare ideal and real gas behavior and predict how
changing temperature, pressure, and volume can cause a gas to
deviate from ideal behavior, Calculate gas density, Use molar
volume of a gas to calculate quantities of mass or particles
(Review from Ch 10)
Use the kinetic molecular theory (KMT) to describe the
behavior of solids, liquids, and gases on a molecular level,
Describe three different intermolecular forces (IMF):
hydrogen bonds, dipole-dipole interactions, and London
dispersion forces, Recognize that intermolecular forces only
affect molecular substances, and recognize IMF as one of four
types of categories of bonding, which also includes covalent
network interactions, metallic bonding, and ionic bonding,
Describe the six changes of state (melting, freezing, boiling,
condensing, sublimation, deposition), Describe the features of
a heating curve, Distinguish heat of fusion and heat of
vaporization and use each in calculations, Identify the features
of a phase diagram, Use a phase diagram to predict how a
change in pressure or temperature will change a given
substance
5.7.B.1
5.7.B.2
Chapters 12, 22,
and 23
Gases
Chapter 13
Liquids and Solids
Chapter 14
5.7.A
5.7.A
September 2, 2003
Page 3 of 4
Topic
Solutions
Skills
NJCCS
Describe properties and different types of solutions, Measure
concentration in terms of molarity, molality, mole fraction,
Chapter 15
and g/mL, Differentiate saturated, supersaturated, unsaturated
and be able to predict the state of a solution given a solubility
curve, Explain how solutions form and the motion of particles
in solution, Define solubility and factors that affect it, Identify
factors that affect rate of dissolution, Define colligative
property and describe osmotic pressure, boiling point
elevation, melting point depression and vapor pressure
reduction
Chemical
Explain the concept of reversibility in chemical reactions,
Equilibrium
Determine K (the equilibrium constant) for a given reaction
using the law of mass action, Use the reaction quotient (Q) to
Chapter 16
determine if a system is at equilibrium, and if not how a
system will shift to attain equilibrium, Define and explain Le
Chatelier’s principle, Describe how changes in concentration,
pressure, and temperature affect a reaction at equilibrium
Solubility and
Compare dissolution and precipitation, Apply a list of given
Precipitation
solubility rules to write complete and net ionic equations from
a given balanced molecular equation, Define solubility
Chapter 17
product (Ksp) and write the equation relating solubility product
to concentration, Evaluate whether or not a precipitate will
form using Ksp, Describe how a common ion can shift the
solubility equilibrium
Acids, Bases, and
State Arrhenius, Bronsted-Lowry, and Lewis definitions of
Salts
Acids and Bases, Identify properties of acids and bases,
Differentiate strong and weak acids and distinguish acid
Chapters18 and 19 strength from acid concentration, Identify conjugate acids and
conjugate bases, Calculate KA for a given acid and Kb for a
given base, Use Kw to relate Ka and Kb, Relate pH to [H+],
Describe how titration is used to determine the concentration
of an unknown acid or base
Oxidation and
Define oxidation and reduction, Identify oxidizing agents and
Reduction
reducing agents, Assign oxidation numbers to elements in
compounds or ions, Using a given activity series, classify
Chapter 20
metals in order of reactivity, Describe different types of redox
reactions such as corrosion, bleaching, combustion etc.,
Identify the oxidizing/reducing agents in a chemical equation
Organic Chemistry Explain carbon’s unique bonding properties, define organic
compounds and organic chemistry, explain how carbon and
Chapters 25 and 26 hydrogen atoms can form numerous hydrocarbon compounds,
define isomers, define polymers, differentiate different classes
of organic compounds, provide examples of selected classes of
organic compounds including their formulas.
5.7.A
5.7.B
5.7.B
5.7.A
5.7.B
5.7.B
5.7.A
5.7.B
September 2, 2003
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