Name___________________________
Period___________________________
Date__________________________
Chemistry II
Final Exam Review
1. Define the following terms – capillarity, dissociation, hydrogen bonding, polar covalent bond,
polar molecule, saturated solution, supersaturated solution, surface tension, Tyndall effect,
unsaturated solution, pressure, Dalton’s law, Charles’s law, Gay-Lussac’s law, Boyle’s law, the
combined gas law, the ideal gas law, absolute zero, boiling point, diffusion, freezing point, heat
of fusion, heat of vaporization, ideal gas, Joule, kinetic energy, kinetic theory, melting point,
pressure, temperature, vapor pressure, volatile, Arrhenius acid, Arrhenius base, binary acid,
diprotic acid, monoprotic acid, oxyacids, strong acid, strong base, triprotic acid, weak acid, weak
base, sublimation, deposition
2. What are the four properties of gases that are most easily observed?
3. Compare and contrast hydrogen bonding and polar covalent bonding.
4. Compare and contrast concentrated and dilute solutions.
5. Calculate the molarity of a 4837 mL solution that contains 37 grams of MgCO3.
6. How many grams of water are necessary for a 2.3 m solution that contains 84 grams of NH4OH?
7. How would you prepare a 6.2 m solution of strontium chloride using 2.34 kg of water?
8. How many L of water are needed to make a 6.0 M solution that contains 345 grams of lithium
nitrate?
9. If I want to make 1375 mL of 3.0 HCl, how many mL of 8.0 M HCl do I need to use?
10. Describe what is happening AT THE MOLECULAR LEVEL when surface tension occurs. In other
words, why does a liquid form a “bubble” above the top of a container?
11. Use dimensional analysis, and equivalent pressures, to convert the following pressures.
a. 44 psi to atm
b. 125 kPa to mm Hg
c. 1.34 atm to kPa
d. 743 torr to psi
12. A certain sample of gas occupies 48 L at a temperature of 39°C. What temperature, in °C, would
be required to get 350 L?
13. How many moles of oxygen would be contained in a 6 L container at 288 K and a pressure of 3.1
atm?
14. If a 4123 mL sample of nitrogen gas is kept at a pressure of 656 mm Hg, what pressure would be
required for a 12 L sample?
15. How many atoms are in 50 grams of SiO2?
16. Calculate the mass, in grams of 3.4 x 1024 atoms of CaBr2.
17. How many grams of boron would be produced if 25.0 grams of boron trichloride reacted with
excess hydrogen gas?
BCl3
+
H2
------->
B
+
HCl
18. How many grams of calclum carbonate are needed to produce 48.0 grams of carbon dioxide?
CaCO3
+
SiO2
------->
CaSiO3
+
CO2
19. How many liters of oxygen gas are required to produce 83 grams of diphosphorus pentoxide?
P4
+
O2
------->
P2O5
20. If 48 grams of CS2 react with excess oxygen gas, how many liters of carbon dioxide are formed?
CS2
+
O2
------->
CO2
+
SO2
21. A 19 gallon sample of carbon dioxide is held at 40°C and a pressure of 12 psi. If the pressure is
changed to 19 psi and the temperature is lowered to 12°C, what will the new volume be, in
gallons?
22. What is the pressure of a 0.45 mol sample of neon at 212°F and 111 kPa?
23. Explain how Toricelli’s barometer works.
24. Are there higher pressures at lower altitudes or higher altitudes? What is the reason for this?
25. A bottle of vanilla extract was left uncovered in a cabinet overnight. When the cabinet door was
opened, a strong odor of vanilla was detected. Explain.
26. How does a real gas differ from an ideal gas?
27. A sample of Cl2(g) and N2(g) are both at 298 K. Compare the kinetic energy of these two
substances.
28. Describe the physical state of absolute zero. (What are the particles doing). Use mathematical
expressions when necessary. Be thorough!
29. Titanium (IV) oxide can be used as a pigment in paint and as a whitening tool. If 40 L of oxygen
are used in the process at STP, what mass of TiO2 will be produced?
TiCl4 +
O2
→
TiO2
+
Cl2
30. When phosphorus burns it produces P4O10 which reacts with water to produce phosphoric
acid. When 100 g of P4O10 is produced, how many grams of water were used?
P4O10
+
H2O
→
H3PO4
31. The combustion of methane produces carbon dioxide and water. If 28 g of CH4 are used, how
many L of CO2 will be produced at 200 kPa and 123ºC?
CH4
+
O2
→
CO2
+
H2O
32. For each of the following statements, mark A for Acid or B for Base
a. produces OH- ions
b. sodium hydroxide
c. H3PO4in antacids
d. in plaster
e. tastes bitter and feels slippery
f. alkaline
g. in aspirin
h. produces H+ ions
i. in citrus fruits
33.
34.
35.
36.
37.
38.
j. more H+ than OHk. pH of 3.75
l. breaks down fats and oils
m. in apples
n. sour tasting and reacts chemically with metals
Complete the following definitions of statements.
a. Neutralization reactions result in the production of water and
______________________
b. A form of pollution caused by the burning of sulfur-containing fossil fuels is
_____________________________
c. A liquid that is colorless in acids and turns bright pink in bases is
_______________________________________
d. The pH of pure distilled water is ___________________________________
e. Blue litmus paper will be __________________________ in basic solutions.
f. Compounds containing only hydrogen and carbon are called
_____________________________
g. Blue litmus paper will be ________________________ in acidic solutions.
h. A substance that is not an acid or a base, but when added to water produces an acid or
base is called a/an ____________________________________
i. The chemical formula for hydrochloric acid is __________________________
j. A compound formed from the positive ion of a base and the negative ion of an acid is
a/an _____________________________________
For each of the following statements mark + for True or 0 for False.
a. Acids and bases are not electrolytes.
b. pH papers are more accurate than litmus paper.
c. MgO is an acidic anhydride.
d. A solution with a pH of 4 has 10 times the amount of H+ ions as a neutral solution.
e. A solution of pH 11 is more basic than a solution of pH 13.
Thoroughly describe the pH scale. Be sure to use the following terms: acid, base, neutral, H+
and OH-.
Write a balanced chemical reaction to show the following neutralization reactions
a. hydrofluoric acid and sodium hydroxide
b. sulfuric acid and calcium hydroxide
c. acetic acid and magnesium hydroxide
Calculate the pH of the following solutions containing the given concentration of H3O+ ions.
Also, say if each solution is an acid or a base.
a. 6.2 x 10-8 M H3O+
b. .0021 M H3O+
What is the H3O+ concentration of a solution given the following pH’s. Also, say if each solution
is an acid or a base.
a. 5.3
b. 12.8
39. Calculate the pH of solutions with the following pOH’s.
a. 8.8
b. 2.6
40. Use the kinetic-molecular theory to describe solids, liquids, and gases.
41. Explain the meaning of the phrase “like dissolves like.”
42. Compare and contrast molarity and molality.
43. Compare and contrast solutions, suspensions, and colloids.
44. Why do we use salt on the roads in the winter?
45. Thoroughly describe the difference between a strong acid and a strong base.
46. Compare and contrast structural formulas and molecular formulas.
47. Draw the following organic compounds.
a. 3,3-dimethyl-1-butyne
b. 3-pentene
c. 4-ethyl-2-methyl-3-heptene
d. Ethene
e. Ethyne
f. 5,6-diethyl-7-methyl-3-octene
g. 1,3-butadiene
48. Name the following organic compounds.
a.
b.
c.
d.
e.