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STUDENTS SHOULD
KNOW
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EXAMPLES OF WHAT
STUDENTS SHOULD BE ABLE TO DO
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Properties Of Matter
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1. There are differences and
similarities among pure substances, solutions, and
heterogeneous mixtures. (AKSci - A.1)
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• Identify pure substances,
solutions, and heterogeneous mixtures from given physical
properties.
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2. Changes in substances can be
classified as chemical and/or physical. (AKSci -
A.2)
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• Conclude whether a reaction
is chemical or physical on the basis of evidence such as
formation of a precipitate, production of gas, change of
color, and/or change in energy.
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3. The concentrations of solutions
can be expressed in a variety of units. This concentration
affects physical properties of the solution. (AKSci -
A.1)
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• Carry out concentration
calculations in molarity, mole fraction, and percent
composition.
• Using concentrations
determine if/and how the boiling point, melting point, vapor
pressure, and osmotic pressure change.
• Describe solutions as
saturated, unsaturated, and supersaturated.
• Explain saturation as an
equilibrium effect.
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4. There are standard methods of
naming and formula writing for elements and compounds
(emphasize IUPAC system). (AKSci - A.1)
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• Name binary compounds that
are composed of metals and nonmetals, transitions metals and
nonmetals, two nonmetals, and acids.
• Name compounds that contain
polyatomic ions.
• Write formulas from a given
name.
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5. Elements can be classified as
metal, metalloids or nonmetal. (AKSci - A.1)
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• Classify an element as a
metal, nonmetal, or metalloid on the basis of its
properties.
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6. Substances can be classified as
ionic, metallic, covalent network, or molecular and/or acid,
base, or neutral. (AKSci - A.1, A.2)
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• Classify a crystalline
substance as either ionic, metallic, molecular, or network
covalent on the basis of its properties.
• Predict the properties of a
classified crystal.
• Explain the properties of
ionic, metallic, molecular, or network covalent crystals
from their structure and forces holding them
together.
• Determine whether a
substance is acidic, basic or neutral on the basis of
structure, name, changes in indicators, pH, and
physical/chemical properties.
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Chemical Change
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1. Chemical changes are described
with balanced chemical equations. (AKSci - A.2,
A.8a)
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• Balance chemical equations
given the reactants and products. Recognize reaction types
and predict products for simple reactions.
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2. The number of particles is
measured in a unit called mole. (AKSci - A.1)
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• Convert between units of
moles, mass, and number of particles.
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3. Balanced chemical equations are
used to make calculations related to chemical reactions.
(AKSci - A.2, A.8a)
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• Determine the amount (mass,
gas volume, number of particles, or moles) of product formed
or reactant used knowing an initial amount of one other
chemical present.
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4. Reaction rate will be affected
by changes of temperature, concentration, surface area, and
use of catalysts. (AKSci - A.2, A.8a)
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• Predict and explain the
effect on reaction rate and time caused by temperature
changes.
• Predict and explain the
effect on reaction rate and time caused by concentration
changes or for solids changes in surface area.
• Explain the effect of adding
a catalyst to a given reaction. The explanation should
include both a potential energy graph and activation energy.
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5. Electron transfer can take place
in a chemical reaction. (AKSci - A.1, A.2, A.8a)
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• Assign oxidation numbers and
determine if a particular reaction involves electron
transfer.
• In a reaction that involves
electron transfer identify the chemical oxidized and the
chemical reduced.
• Balance simple equations
involving electron transfer.
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6. H+ transfer can take place in a
chemical reaction. (AKSci - A.2, A.8a)
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• Identify the acid and base
in a reaction involving transfer of H+.
• Perform an acid/base
titration to determine the concentration of an
unknown.
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7. The strength of an acid and/or
base is related to its composition and degree to which it
breaks down. (AKSci - A.2, A.8a)
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• Identify strong or weak
acids/bases based on their formulas and names.
• Explain the difference
between strong, weak, concentrated, and dilute
solutions.
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8. The pH scale gives a level of
acidity/basicity for a solution based on the concentration
of H+ (or hydronium ion) present. (AKSci - A.2,
A.8a)
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• Experimentally determine pH
using indicators, pH meters, and/or test papers.
• Interpret pH data to
determine level of acidity/basicity.
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9. Many reactions consist of both a
forward and reverse reaction occurring simultaneously.
Through this process equilibrium can be achieved. (AKSci -
A.2, A.8a)
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• Explain how to recognize an
equilibrium on the basis of properties and explain the
dynamic process involved in equilibrium such as vapor
pressure, phase change, solubility, and chemical
equilibria.
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Structure of Matter
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1. Physical changes and properties
of matter can be explained through sketches, models, and
descriptions of the particles. (AKSci - A.1, A.2)
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• Construct sketches or models
of solids, liquids, and gases. Use these to determine how
phase changes proceed.
• Construct molecular models
to determine shape and molecular polarity in simple
compounds.
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2. Some physical changes consist of
both a forward and reverse process occurring simultaneously.
Through this process physical equilibrium can be achieved.
(AKSci - A.2)
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• Identify the opposing
changes and discuss their rates, in phase change
equilibrium.
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3. Chemical changes and reactions
can be explained using sketches, models, and descriptions of
the reacting particles and particles produced. (AKSci -
A.2)
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• Use sketches and models to
describe chemical reactions.
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4. Kinetic molecular theory
explains changes in gas volumes, moles, pressure, and
temperature. This allows for calculations to be performed
relating these quantities. (AKSci - A.1)
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• Use the particle model of
gases to explain the relationship of pressure, volume,
moles, and temperature in gases.
• Perform calculations to
determine one of the four major variables given the other
three (pressure, volume, moles, and temperature) using the
ideal gas law.
• Determine experimentally the
relationships of pressure versus volume, pressure versus
temperature, and volume versus temperature. Express these
relationships in graphs and interpret these
graphs.
• Calculate the effect of
changes in gaseous systems, using the combined gas
law.
• Suggest and recognize
practical applications using these relationships.
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5. Atoms are made of a positive
nucleus surrounded by negative electrons. (AKSci -
A.1)
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• Determine the number of
protons and neutrons in the nucleus and the electrons
surrounding it for a particular isotope.
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6. An atom's electron
configuration, particularly the outermost electrons,
determines how the atom can interact with other atoms. Atoms
form bonds to other atoms by transferring or sharing
electrons. (AKSci - A.1, A.8a)
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• Write an electron
configuration for any atom including the use of short hand
method.
• Determine if a bond between
atoms is ionic, polar covalent, or nonpolar covalent on the
basis of electronegativity or position on the periodic
table.
• Explain the difference
between ionic, polar covalent or nonpolar covalent
bonds.
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7. The nucleus, a tiny fraction of
the volume of an atom, is composed of protons and neutrons,
each almost two thousand times heavier than an electron. The
number of positive protons in the nucleus identifies the
element. In a neutral atom, the number of electrons equals
the number of protons. An atom may acquire a charge by
gaining or losing electrons. (AKSci - A.1)
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• Construct a mental model
showing the positions and sizes of the subatomic particles.
• Discuss the formation of
ions by gaining or losing electrons only.
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8. Neutrons have a mass that is
nearly identical to that of protons and have no electrical
charge. Neutrons affect the mass and stability of the
nucleus. Isotopes of an element have the same number of
protons but differ in the number of neutrons. (AKSci -
A.1)
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• Determine the identity,
mass, and reactivity of an element from the number of
protons, neutrons, and electrons.
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9. An element's location on the
periodic table can be used to determine similarities and
trends among the elements. (AKSci - A.1)
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• Discuss the evolution of the
periodic table as a scientific tool.
•Recognize and explain trends
on the periodic chart in quantities/properties such as
ionization energy, electron affinity, reactivity, metallic
character, electronegativity, and atomic size.
• Determine the number of
valence electrons and charge of an element's most common ion
from the periodic chart.
• Compare and contrast
families and periods.
• Identify elements from
particular families such as alkali metals, alkaline earth
metals, halogens, and noble gases.
• Construct Lewis electron dot
structures for simple compounds.
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10. The arrangement of atoms in a
molecule determines the molecule's properties. Shapes are
particularly important in how molecules interact with
others. (AKSci - A.1)
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• Determine a molecule's shape
using Valence Shell Electron Pair Repulsion
Theory.
• Determine molecular polarity
from the shape and bond polarity of a molecule.
• Determine the type and
strength of intermolecular forces based on molecular
polarity. Relate the strength of intermolecular forces to
physical properties such as boiling point, melting point,
surface tension, solubility, vapor pressure, adhesion,
cohesion, and viscosity.
• Suggest and recognize
practical applications using intermolecular
forces.
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11. Nuclear changes are different
than chemical changes. The nucleus can change, resulting in
a different element and/or radioactivity. (AKSci -
A.2)
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• Distinguish between nuclear
and chemical reactions.
• Write balanced reactions
involving alpha, beta, and gamma emission.
• Discuss relevant
applications of nuclear chemistry.
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Energy Change
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1. Temperature is a measurement of
average kinetic energy. Heat is a measurement of
transferable energy. (AKSci - A.2, A.9)
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• Measure temperature and heat
in appropriate units.
• Interpret a graph of kinetic
energy versus number of particles.
• Perform an experiment to
measure heat flow.
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2. Chemical and physical changes
can be classified as exothermic or endothermic. Balanced
equations with an energy term can be used to calculate
energy changes. (AKSci - A.2)
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• Identify reactions as either
exothermic or endothermic from experimental data or an
equation including an energy term.
• Determine the energy change
for a given mass or moles from an equation with an energy
term.
• Discuss the transitions
between potential and kinetic energy in a chemical
reaction.
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3. When energy changes in an
isolated atom or molecule, the energy changes in discrete
jumps from one value to another. This change in energy
occurs when radiation is absorbed or emitted, so the
radiation also has discrete energy values. (AKSci - A.2,
A.9)
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• Explain the lines in a
spectra on the basis of electrons changing between discrete
energy levels.
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