Unit 1: Foundations of Chemistry
Chapter 1- Introduction to Chemistry
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What is the definition of chemistry?
Characterize scientific theory, scientific law, and hypothesis.
Chapter 2 - Matter and Change
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Name and define the two kinds of properties of matter.
Classify each of the following properties as physical or chemical. a. reacts with Zn to produce hydrogen gas b. has a density of .18 g/mL c. a white crystalline solid d. boiling point is 118 oC
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e. melting point is 22 oC f.
reacts with oxygen to produce metal oxide
Classify each of the following changes as physical or chemical. a.
explosion b.
corrosion c.
evaporation d.
food spoilage
Describe the particle arrangement and properties of gases, solids, liquids, and plasmas.
What is the difference between a mixture and a compound?
Chapter 3 - Scientific Measurement
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What is a quantitative and qualitative measurement?
Characterize accuracy and precision.
Determine the # of significant figures in each of the following measurements a. 213
11. b. 213.0 c. 0.0213 d. 0.02130 e. 500
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Perform addition/subtraction and multiplication/division with significant figures. Go to this website http://www.sciencegeek.net/APchemistry/APtaters/sigfigs.htm
and practice until you can make 100%.
What are the SI units for mass, length, amount of substance, and temperature?
Review metric conversions. Go to this site http://www.sciencegeek.net/Chemistry/taters/Unit0Metrics.htm
and practice.
14. Review density and how to calculate mass, volume, or density. Go to this site and complete the practice set. http://www.algebralab.org/practice/practice.aspx?file=word_density.xml
Unit 2: States of Matter and Energy Changes
Chapter 13 - States of Matter
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What does the kinetic molecular theory of gases say about particles?
Why does a liquid’s evaporation rate increase when the liquid is heated?
List the phase changes possible and know the definition of each.
What is dynamic equilibrium?
What causes a substance to boil?
What causes the vapor pressure of a contained liquid to increase?
During a phase change, the temperature of the substance __________. (increases, decreases, remains the same)
What is the direction of heat flow from object to object?
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What is the amount of heat required to raise the temperature of 200 g of aluminum by 10oC? ( specific heat for Al = 0.90 J/g o C)
Define specific heat. What are its units?
What substance has the highest specific heat?
What is the sign of ∆H when a reaction is exothermic? Is this amount of heat written as a product or reactant in the equation?

27. On what does the amount of heat transferred from an object depend?
Chapter 14 – Behavior of Gases
28. What factors affect gas pressure and how does pressure change with respect to each?
29. Name and define each of the 4 gas laws. Practice Go to this site and complete the practice set. http://www.sciencegeek.net/Chemistry/taters/Unit7GasLaws.htm
Unit 3: Atomic Structure
Chapter 4 - Atomic Structure
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What is an atom?
Describe an electron, proton, and neutron. Who discovered each particle and when?
Identify the major contribution of each of the following scientists to the development of the atomic theory. a. Democritus b. Dalton c. Rutherford d. J.J. Thomson e. Bohr
Describe the nucleus of an atom. f. Millikan
According to the Bohr model, electrons in the same energy level have the same
What is the mass number of the isotope Ne-12?
How many neutrons does the isotope Ne-12 contain?
Define isotope.
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38. What is the atomic weight of Mg based upon the following isotopic abundance?
Mg-24 78.70 % 23.98504 amu
Mg-25
Mg-26
10.13% 24.98584 amu
11.17% 25.98259 amu
39. Identify characteristics of metals and nonmetals.
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State the periodic law.
Identify periods and groups on the periodic table.
Chapter 5 - Electrons in Atoms
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Construct electron configurations for the following elements: a. Ca b. Si c. Ag d. Am e. Rn
Describe the Aufbau Principle, Pauli Exclusion Principle, and the Heisenberg Uncertainty Principle.
Calculate the energy of a photon having a frequency of 4 x 10 7 Hz. 44.
Unit 4: Periodicity
Chapter 6 - Periodicity
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Define atomic radii, ionization energy, and electronegativity.
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What are the trends (across a period and down a group) for each of the periodic properties?
Describe the reasons for the trends identified in the question above. The terms nuclear charge and shielding
48. should be used in your explanation.
What is the relationship between chemical behavior and electronic configurations? You should review electronic configurations.
What was Mendeleev's contribution to the development of the periodic table? 49.
Unit 5: Chemical Bonding
Chapters 7, 8, and 9
50. Practice writing formulas and naming compounds using http://staffweb.psdschools.org/rjensen/genchem/morepracticenms_forms.htm
51. How are ions formed? Which elements tend to form cations and which tend to form anions?
52. What are the 7 diatomic molecules?
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List types of electron configurations in terms of increasing stability.
A single covalent bond shares how many electrons?
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State the octet rule.
Draw the e-dot diagram for Sulfur.
Draw the e-dot diagram for SO2 and determine how many covalent bonds are present.
How do you determine if a bond is polar or not? A molecule?

Unit 6: Chemical Quantities
Chapter 10 - Chemical Quantities
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What is Avogadro's number and to what is it equal?
How many moles of Mg are in 60.8 grams?
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How many grams are there in 1.8 moles of Al?
How many atoms are there in 12.0 g of Fe?
If you experimentally determined the molecular weight of CO2 to be 40 grams, and the actual molecular weight is 44 grams, what would be the % error of your results?
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In the laboratory you determined that 2.2 grams of NaCl was contained in a mixture. The original sample weighed
3.1 grams. What is the % by mass of the NaCl?
What is the gram formula mass of Ba(NO3)2?
Practice calculating empirical formulas and molecular formulas using http://www.chemteam.info/Mole/Empirical-
MolecFormulas.html
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Chapter 11 - Chemical Reactions
67. Practice balancing equations using http://honorsph.startlogic.com/honorsphysicalscience/quizzes/Balancing_equations.htm
68. Practice classifying reactions here http://www.quia.com/quiz/2074347.html
and predicting equations here http://www.funtrivia.com/playquiz/quiz2460251c2b140.html
Chapter 12 - Stoichiometry
69. Practice stoichiometry problems using http://www.sciencegeek.net/Chemistry/taters/Unit4Stoichiometry.htm
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Chapter 16 – Solutions
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What are the factors which affect solubility?
Calculate the molarity of a solution with a volume of 250 mL which contains 36.0 g of NaBr.
72. How is a solution of .56 M prepared?