Grades will be posted approximately every two weeks or after
major tests. If you want to know your
grade at any time all you need to do is ask.
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Chapter section
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Objective
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Standard
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Problems
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Laboratory
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1-1
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Explain why a knowledge of chemistry is central to many
human endeavors
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1-2
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List and described the steps of the scientific method
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1-3
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Explain the basic safety rules that must be followed
working in the chemistry laboratory
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1-4
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Identify the metric units of measurement used in chemistry
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P. 52 31, 33, 34.
P. 900 6,7.
Teacher generated problems.
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1-5
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Explain what causes uncertainty in measurements, compare
accuracy and precision
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3.1.10.E 3
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P. 900 8
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1
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1-6
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Explain how you use significant digits and scientific
notation, calculate percent error, define density and explain how it is
calculated
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3.1.10.E 3.
3.4.12.A 8.
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P. 52 37, 45, 49, 50, 53, 54 P. 900 10 to 14
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2
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1-7
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Explain how dimensional analysis and conversion factors
are used to solve problems in chemistry
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3.1.10.D 1
3.1.12.D 1
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P. 52 39 to 44, 55 to 57 P. 900 15 to 17
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2-1
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Named three basic forms of energy. State the law of conservation of energy.
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3.1.10.E 1.
3.4.12.a 6
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P. 901 1-4
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2-2
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Compare the Fahrenheit, sell see us, and tell the temperature
scales. Explain what is meant by absolute zero.
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3.1.10.D 2.
3.7.12.B 3.
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P. 83 21, 22 P. 901 5,6
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4
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2-3
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Name and describe the four states of matter. Compare physical and chemical properties of
matter. State the law of conservation
of matter.
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3.1.10.E 1.
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P. 901 7,8
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5
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2-4
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Explain the difference between an element compound.
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P. 901 9,10
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2-5
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Compare heterogeneous and homogeneous mixtures. Describes several techniques to separate
mixtures.
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3.4.10.A 8.
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P. 901 11,12
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3-1
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Define atom. Lists the
postulates of Dalton’s atomic theory.
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3.1.10.B 1.
3.1.10.E 1.
3.2.10.A 1.
3.2.12.A 2.
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3-2
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Discuss how atomic structure is related to
electricity. Explain what studies of
cathode rays and radioactivity revealed about atoms. Discuss Rutherford’s alpha scattering experiment
and how it showed the existence of the nucleus.
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3.1.10.E 1.
3.1.12.E 2.
3.2.10.A 1.
3.2.12.A 2.
3.4.12.C 6.
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3-3
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Name and describe the three subatomic particles in an
atom. Determined the number of
protons, neutrons, and electrons in an atom or ion. Define isotopes and atomic mass.
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3.4.10.A 1
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P. 902 9,10.
Teacher generated problems.
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3-4
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Describe the changes that accompany nuclear reactions. Define radioactivity
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3.4.12.A 2.
3.4.12.A 6.
3.4.12.A 7.
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P. 123 20,21 P. 902 12 to 15
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4-1
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Describe a wave in terms of its frequency, wavelength,
speed, and amplitude. Identify the
major regions of electromagnetic spectrum.
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3.4.12.C 1
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P. 129 4 P. 903 1 to 3
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4-2
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Explain what is meant by a quantum of energy. Relate the energy of radiation to his
frequency.
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3.2.10.A 1.
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P. 903 4,5
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4-3
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Distinguish between a continuous spectrum and a line
spectrum. State the main idea in Bohr’s model of the atom.
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3.1.10.B 1.
3.1.10.E 1.
3.1.12.E 2.
3.2.10.A 1.
3.2.12.A 2.
3.4.12.C 5
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P. 903 6,7
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10
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4-4
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Describe atomic orbitals in
terms of their shape, size, and energy.
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P. 157 20 P. 903 9 to 14
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4-5
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Determine electron configurations of several elements
using the principles of orbital energy, orbital capacity, and electron spin.
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3.1.10.B 3.
3.4.12.C 4.
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P. 157 23, 27 P. 903 15 to 17.
Teacher generated problems
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5-1
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State the periodic law and discuss the contributions that
Mendeleev and Moseley made to the periodic table.
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3.1.10.E 1.
3.1.12.E 2.
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13
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5-2
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Explain why elements in a group have similar properties. Identify the four blocks of the periodic
table.
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P. 904 4, 7
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16
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5-3
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Define the term periodic trend. Identified for important periodic trends
and explained how each reflects the electron configurations of the elements.
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3.1.10.C 1.
3.4.10.A 2.
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P. 904 10,11, 13 to 15
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7-1
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Describe the characteristics of an ionic bond. State the Octet rule.
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3.4.10.A 5.
3.4.12.C 6.
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P. 906 1 to 5
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19
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7-3
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Write names for ionic compounds, and binary covalent.
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3.4.10.A 6.
3.4.12.A 1.
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P. 253 28, 34 P. 906 9 to 15, 17.
Teacher generated problems.
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7-2
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Describe the characteristics of a covalent bond. Describe the difference between polar and nonpolar covalent bonds.
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3.4.10.A 5.
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P. 253 32 P. 906 6 to 12
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20
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8-1
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Describe the VSEPR theory.
Identify the common shapes of small molecules.
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P. 277 29,30 P. 907 1 to 11
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8-2
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Explain what determines the polarity of a molecule. Explain why water is a polar molecule.
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P. 277 25 P. 907 12 to 14
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22
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9-1
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Describe the characteristics of a chemical reaction.
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3.4.12.A 2.
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P. 908 1,2
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9-2
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Write balanced chemical equations.
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3.4.12.A 2.
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P. 302 31 to 34, 44 to 50 P. 908 3 to 11. Teacher generated problems. Worksheet 9-2
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25
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9-3
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Classify chemical reactions
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3.4.10.A 7.
3.4.12.A 2.
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P. 302 33 to 43
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27
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10-1
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Define a mole and describe its importance. Identifying use Avogadro’s Number. Define molar mass and explain how it relates
the mass of a substance to the number of particles in that substance.
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P. 344 30, 31 P.
909 1 to 10
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10-2
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Convert among the number of particles, moles, and mass of
a substance. Describe molar volume can
use it to solve problems.
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P. 344-5
32 to 42, 46-51 P. 909 11 to 16. Worksheet 10-2
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28, 29
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10-3
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Find a percentage composition of a given formula. Use percentage composition to determine the
formula of an unknown sample. Find empirical
and molecular formulas.
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P. 344-5 43 to 45, 54, 55 P. 909 17 to 23. Worksheet 10-3
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30
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11-1
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Define stoichiometry and
describe its importance. Relate stoichiometry to balanced chemical equations
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3.4.10.A 7
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P. 378 29 to 33, P. 910 2 to 5
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11-2
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Identify and solve different types of stoichiometry
problems.
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3.4.10.A 7
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P. 378 34 to 46, P. 910 6 to 15. Worksheet 11-2
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11-3
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Determine the limiting reactant of a chemical reaction. Calculate the amount of product formed in a
chemical reaction when reactants are present in non-stoichiometric
proportions.
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3.4.10.B 1.
3.4.12.B 2.
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P. 379 48, 49, P. 911 16 to 22. Worksheet 11-3
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12-1
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Distinguish between exothermic & endothermic reactions
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3.4.10.B 3.
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P 408 34, 35, P. 912 4
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12-2
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Explain what is meant by enthalpy and enthalpy
change. Define standard enthalpy
change and how it is used.
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3.4.12.B.1.
3.4.12.B 4.
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P. 391 3,4, P.408 38-42, 49,50 P. 912 5-8
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34
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12-3
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State Hass’s law. Apply Hess’s law to determine ΔH° for
a reaction.
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3.4.10.B 3.
3.4.12.B.1.
3.4.12.B 4.
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P.408 43,44, 51,52,55 P. 912 10,11
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CWC 18
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12-4
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Describe how a calorimeter determines heats of reactions.
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3.4.12.B.1.
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P. 397 5,6 P 408 45-48 P.912 12-18
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36
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12-5
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Compare heat and temperature.
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13-1
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Describe the kinetic molecular theory and explain how
accounts for observed gas behavior.
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13-2
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Explain what gas pressure means and describe how it is
measured.
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P. 427-9 1-4, P. 454 29-32,
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13-3
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State the gas laws.
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P. 434-40 5-10, P. 454 33-37
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CWC 6, 7
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13-4
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Discusses significance of the ideal gas equation. Compare ideal and real gases.
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3.1.10.E.1
3.4.10.A.3
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P.443 11,12, P. 454 38-41
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13-5
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Relate gas density to temperature and molar mass.
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P. 454 42
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14-1
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Explain how kinetic molecular theory accounts for the
physical properties of solids and liquids.
Describe the different types of intermolecular forces.
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3.1.10.B.1
3.4.10.A.4
3.4.12.A.4
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P.914 1-3
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14-2
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Defined viscosity and surface tension and explain their
relationship to intermolecular forces.
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14-4
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Described vaporization, condensation, and boiling. Describe freezing in melting. Identify the features of a phase diagram.
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CWC 4
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15-1
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Describe the properties of solutions. Identify the different types of solutions.
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P. 915 1,2
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15-2
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Measure the concentration of solutions in terms of molarity, molality, and mole
fraction. Differentiate among saturated, unsaturated, and super saturated
solutions
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P.915 3-15
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15-3
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Explain how solutions form. Define solubility and described factors
that affect solubility. Describe the factors
that affect the rate at which a solute dissolves in a solvent.
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3.4.12.A.8
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15-4
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Defined a colligative property
of a solution. Described four colligative
properties of solutions.
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P. 916 18-23
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44 CWC 15
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16-1
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Describe a reversible reaction. Define chemical equilibrium and explain how
is achieved.
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46
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16-2
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Determining equilibrium constant for a given reaction. Analyze the extent of the reaction from its
equilibrium constant. Use the reaction
quotient of a reaction to determine if a reaction is at equilibrium.
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3.1.10.E.2
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P. 559 24,27, P. 917 5-14
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16-3
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Explain Le Chatelier’s
principle. Describe out changes in concentration, pressure, and temperature
affect a reaction at equilibrium. Relate to Haber process to Le Chatelier’s principle.
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P. 559 28,29, P.918 15-18
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47
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17-1
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Compare dissolution and precipitation. Describe equilibria for aqueous solutions of ionic solids.
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P.586 30-40, P. 918 1-7
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49
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17-2
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Predict whether or not a precipitate will form using the
solubility product. Describing
precipitation reaction and relate it to solubility. Right net ionic equations to describe the
formation of an aqueous solution.
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3.1.10.E.2
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P586 41-44, 52-58, P. 919 8-13
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17-3
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Described a common ion, and explain how the common-ion
effect shifts solubility equilibria.
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P. 586 44, 45, 59
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18-1
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State the Brønsted- Lowry definition
of acids and bases. Identify the common
physical and chemical properties of acids and bases.
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3.2.10.A.1
3.4.12.A.5
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P. 919 2,4
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52
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18-2
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Explain what dissociation constants indicate about an acid
or a base. Use experimental data to
calculate a dissociation constant.
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P. 919 7-17
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18-3
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Explain what most acidic H atoms have in common. Explain what most bases have in
common. Describe how acids are named.
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3.4.12.A.1
3.4.10.A.6
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P. 919 18-20
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19-1
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Identify the ion concentrations in pure water. Describe the pH scale.
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P. 648 36-46, P. 921 1-8
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19-2
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Identify a buffer.
Explain how buffers work.
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3.1.10.E.2
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P. 648 47, P 921 9-11
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19-3
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Describe an acid-base titration. Explain how indicators are
used in titrations and how they are chosen.
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P. 648 49-52, P. 921 12, 14-16, 18, 19
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57,
CWC
23, 24, 25
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20-1
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Define oxidation and reduction. Explain what oxidation numbers are and how
they are assigned.
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3.4.12.A.2
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P. 681 20 P. 922 1-11
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20-2
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Explain what is meant by the activity series of metals.
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P. 922 12, 13
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60
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20-3
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Describes some applications of redox
reactions.
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20-4
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List the steps in balancing a redox
equation.
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3.4.12.B.3
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P. 681 27, 28
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22-1
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Define the rate of a chemical reaction. Identify the intermediate products of a
reaction mechanism. Describe a rate
law for a chemical reaction.
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3.1.10.E.4
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P. 925 6-8
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22-2
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Understand chemical reactions in terms of collision
theory. Explain out energy is involved
in chemical reactions. Define
Activation energy and describe and activated complex.
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3.4.10.B.3
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22-3
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List of factors that affect reaction rates and explain
them according to collision theory.
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23-1
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Explain was meant by a spontaneous process.
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P. 926 1, 2
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23-2
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Relate enthalpy changes to spontaneity.
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P. 926 5, 6
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67
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23-3
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Define entropy.
State the Entropy criterion for a spontaneous process.
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P. 926 7, 8
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23-4
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State the criterion for reaction spontaneity in terms of
its free energy change.
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P. 926 10-17
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Chemistry
Tutoring Available on Saturdays. Let Mr. Cahill know if you plan to come.