1. Ch13,14 – Gas Laws
1. According to the kinetic theory, gases consist of particles that:
a. occupy considerable volume b. are close together
c. exert attractive and repulsive forces among themselves
d. move rapidly in constant random motion e. None of these
2. At sea level, atmospheric pressure is equal to __________
3. STP refers to ________________________
4. Absolute zero is:
a. the temperature at which the motion of particles theoretically ceases
b. 0 K
c. a temperature that has never been produced in the laboratory
d. All of these e. None of these

2. 5. At 80 K, the particles of gas have:
a. twice the average kinetic energy of the same particles at 40K
b. half the average kinetic energy of the same particles at 40K
c. one-forth the average kinetic energy of the same particles at 20K
d. None of these
 6. Compare H2O as a gas, liquid, and solid.
a. Which state has the most kinetic energy?
b. Which state has a definite shape?
c. Which state has its volume most affected by pressure?
7. Water could be made to boil at 92ºC by:

3. 8. As the temperature of a fixed volume of a gas increases,
the pressure will __________
9. The volume of a gas is doubled while the temperature is held constant.
The pressure of the gas __________   
10. If a sample of oxygen occupies a volume of 2.15 L at a pressure
of 58.0 kPa and a temperature of 25C, what volume would this sample
occupy at kPa and 0C? (Combined Gas Law)

4. 11. The volume (in L) that would be occupied by 5.00 mol of O2
at STP is: (PV = nRT)

5. Chapter 7,8 – Ionic and Covalent Bonds
1. How many valence electrons does an atom of any element
in Group 15 have?
2. Draw the electron dot structure for an atom of fluorine
and phosphorous.
3. The general electron dot structure . X : could represent
which column on the periodic table?
4. When a magnesium atom loses its valence electrons,
what is the charge on the resulting ion? How about aluminum?

6. 5. What is the electron configuration of oxygen
and also the oxide ion, O-2?
How about fluorine and also the fluoride ion, F-1?
6. An ionic compound is:
a. generally a salt b. held together by ionic bonds
c. composed of anions and cations d. all of the above   
7. Which of these is not a characteristic of most ionic compounds?
a. solid at room temperature b. conducts an electric current when melted
c. has a low melting point
d. produced by reaction between metallic and nonmetallic elements

7. 8. A covalent bond forms?
a. when as element becomes a noble gas b. when atoms share electrons
c. between metals and nonmetals
d. when electrons are transferred from one atom to another   
9. Name one element with eight valence electrons.
  Name one element with six valence electrons.
10. In general metals react by:
a. losing valence electrons b. gaining valence electrons
c. sharing valence electrons
d. sometimes gaining and sometimes losing valence electrons.

8. 11. An ion of K has the same electron configuration as what noble gas?
12. Will the following atoms combine to form ionic bonds, polar
covalent bonds, or nonpolar covalent bonds?
a. sodium and bromine b. nitrogen and oxygen c. hydrogen and carbon

9. 13. Draw the structural diagrams for CO2, SO42–,
Draw the hybridization of ethane, C2H6, and for ethene, C2H4 .
List the type of hybridization, include the number of sigma and pi bonds.

10. Chapter 15,16 – Properties of Water and Solutions
1. The high surface tension of water is due to ___________________
2. Is a solution is a heterogeneous or homogeneous mixture?
Can the solute be filtered out of the solvent?
What does it mean to say a solution is saturated?
Mixtures from which some of the particles will settle slowly upon standing
are referred to as:
a. homogeneous. b. solutions. c. suspensions. d. colloids  
3. What is an electrolyte?
Which is the following is not an electrolyte?
a. Cane sugar (aq) b. HCI (aq) c. KCI (aq) d. (NH4)2SO4(aq)

11. 4. How many water molecules are attached in the substance
copper sulfate pentahydrate?
barium hydroxide octahydrate?
5. Which of these would you expect to be soluble in the nonpolar solvent
carbon disulfide, CS2?
a. SnS2 b. CaCO3 c. CCl4 d. H2O
6. Which of the following would be expected to dissolve very readily
in water? a. CH4 b. H2 c. NaOH d. CCl4   

12. 7. If salt is dissolved in water, water serves as the solute or solvent?
8. What 3 things can you do to usually make a substance
dissolve faster in a solvent?
9. To increase the solubility of a gas at constant temperature,
would it be better to increase or decrease the pressure above the liquid?
10. What is the molarity of a 200 mL solution in which 0.2 mole
of sodium bromide is dissolved?

13. Chapter 17 – Thermochemistry
1. Water has a specific heat capacity of 4.18 J/(g.ºC).
Iron has a specific heat capacity of 0.44 J/(g.ºC).
Which can absorb more heat energy without changing its temp as much?   
2. The boiling point of an unknown solution is 125ºC.
What is this temperature in Kelvin?

14. 3. An unknown, non-reactive metal masses at 55.52 g. It is heated to
a temperature of 95.7°C then place in a calorimeter filled with
distilled water intially at 20.1°C. They reach equilibrium at 22.4°C.
What is the specific heat of the metal?   
4. Label the numbered areas of the phase diagram. 
120
For H2O:
5) ________
4) ________
100
Temp
(°C)
3) _________
2) _______
1) _______
-10
Time

15. 5. A beaker contains 250 mL of water and is placed on a hot plate.
The water is heated. Heat energy comes from the hot plate, enters the
water, and the water’s temperature rises until it starts to boil.
When the water starts to boil, the temperature stops rising, yet the hot
plate continues to pump heat energy into the water. How can this be?
6. Given the reaction: N2(g) + 3H2(g)  2 NH3(g) ΔH = – 92 kJ
Is the reaction endothermic or exothermic?
Re-write the reaction to include the heat.
If 5 L of Hydrogen react with excess nitrogen, how much heat is produced?

16. Chapter 18 – Reaction Rates and Equilibrium
1. N2(g) + 3H2(g)  2 NH3(g), if someone keeps adding more and
more hydrogen gas to an excess of nitrogen, what will happen to
the amount of ammonia produced?   
2. If that reaction took place in a large balloon and was allowed to reach
equilibrium, what would happen if someone squeezed the balloon
into a smaller volume?
3. Which has more entropy, solid iodine or iodine that has sublimed
into a gas?

17. 4. At 25ºC, the following reaction occurs:
4NH3(g) + 7O2(g)  4NO2(g) + 6H2O(g) kJ
a. The change in entropy, ΔS = – J/K.
Does this reaction have a favorable change in entropy?   
b. Is this reaction spontaneous, based on
the Gibb’s Free Energy Equation?

18. d. Ca(OH)2 e. NH3 f. HClO3 g. HClO
Chapter 19 – Acids and Bases
1. Which of the following substances are acids and which are bases?
While you’re at it, why don’t you name them as well!
a. HCl b. H2SO4 c. NaOH
d. Ca(OH) e. NH f. HClO g. HClO   
2. The pH of pure water is 7. If you squirt some lemon juice in it,
its pH drops to 6. Is it considered acidic or basic?

19. C5H5N(aq) + HOH(l) C5H5NH+(aq) + OH-(aq)
3. The pH of a concentrated HCl solution is 1.
The pH of the lemon juice is 6. What is the concentration of H+ ions
in each?   
4. Identify the acid-base pairs:
C5H5N(aq) + HOH(l) C5H5NH+(aq) + OH-(aq)

20. Chapter 20 – Neutralizations
1. Sodium hydroxide neutralizes hydrochloric acid.
a. What are the products?
b. If your stomach contains 500 mLs of a 0.1 M HCl solution,
how many grams of NaOH could you swallow to neutralize this acid?
(Please don’t attempt this!)

21. Chapter 21 – Redox
1.   Fe + HCl  FeCl3 + H2
Ox____
Red____

22. Cr+3(aq) + 3e-  Cr(s) E0= –0.50 V
Ch22 – Electrochem
1. A voltaic cell is constructed using electrodes
with the following half-reactions.
Fe e-  Fe(s) E0 = –0.44 V
Cr+3(aq) + 3e-  Cr(s) E0= –0.50 V
Determine the cell reaction and the standard cell potential.

23. Carbon Chains and Functional Groups
1. Octane, commonly found in gasoline, is an alkane,
a chain of carbon atoms, one of many hydrocarbons
we have mentioned this year.
a. Please draw a model of the molecule.
b. Explain why the molecule is saturated.
2. Ethene, C2H4, is a non-saturated hydrocarbon.
Show how it can become saturated if it forms
the alkane named ethane, C2H6.

24. 3. Butane, C4H10, is an alkane with 2 isomers. Draw them.
4. Ethanol, C2H5OH, is an alcohol group.
Show how it is different from ethane.