Name_______________________
CHEMISTRY FINAL EXAM REVIEW GUIDE
CHAPTERS 8 AND 9
TERMS AND CONCEPTS:
Chemical reaction
Reactants
Products
Synthesis reactions
Decomposition reactions
Single replacement reactions
Double replacement reactions
Combustion of a hydrocarbon
catalyst
mole ratio
Avogadro’s number
molar mass
limiting reagent
excess reagent
actual yield
theoretical yield
percent yield
SKILLS/PROBLEM TYPES:
Balance equations
Tell the type of reaction
Translate word equations
Stoichiometry problems from balanced equations
Percent yield problems
PRACTICE PROBLEMS:
Translate, balance, and tell the type of reaction for each please.
1. Sodium phosphate + calcium chloride  sodium chloride and calcium phosphate
2. Tricarbon hexahydride + oxygen gas  carbon dioxide and water
3. Magnesium chlorate  magnesium chloride + oxygen gas
4.
Sodium oxide + water  sodium hydroxide
5. Calcium iodide + fluorine  calcium fluoride + iodine
Answer the following questions based on the chemical reaction given below please.
K3N +
CaCO3 
K2CO3 +
Ca3N2
6.
Balance the equation and tell its type.
7.
How many grams of potassium carbonate can be formed from 250 grams of potassium nitride
and excess calcium carbonate?
8.
How many moles of calcium carbonate are needed to produce 155 g of calcium nitride?
9. How many formula units of calcium carbonate are needed to react with 7.5 moles of potassium
nitride?
10. If calculations predict a yield of 215 grams of calcium nitride but only 211 grams are collected in
the lab, what is the percent yield?
Name_____________________
CHEMISTRY FINAL EXAM REVIEW GUIDE
CHAPTERS 10, 11, AND 16
TERMS AND CONCEPTS:
Heat
Temperature
Enthalpy
Entropy
Heat of reaction
Heat of fusion
Heat of vaporization
Solid
Liquid
Gas
Plasma
Condensation
Sublimation
boiling
evaporation
freezing
melting
temperature during a phase change
Kinetic molecular theory of gases (basic points)
Boyle’s Law
Charles’ Law
Gay-Lussac’s Law
Combined Gas Law
STP
Ideal Gas Law
Standard molar volume
SKILLS/PROBLEM TYPES:
Specific heat capacity
Enthalpy change for a chemical reaction
Gas Laws
Standard molar volume (at STP)
Density at STP
PRACTICE PROBLEMS:
1. You need 280.8 J to raise the temperature of 34.0 g of ammonia, NH3 (g), from 23.0 C to 25.0 C.
Calculate the specific heat capacity of ammonia.
2.
How much heat is needed to melt 5.6 kg of ice if the heat of fusion of water is 80 cal/g?
3.
How many grams of water can be vaporized by 15 000 J if the heat of vaporization of water is
2340 J/g?
4. The pressure on a 240.00 mL sample of helium gas is increased from 0.428 atm to 1.55 atm.
What is the new volume, assuming constant temperature?
5. A scientist warms 26 mL of gas at 0.0 C until its volume is 32 mL. What is the new temperature
in degrees Celsius?
6. A tank of oxygen for welding is at 31 C and 11 atm. What is the pressure, when it is taken to the
South Pole, where the temperature is -41 C?
7. How many moles of air are in 1.00 L at -23 C and 101 kPa?
8. A 4.44L container holds 15.4 g of oxygen at 22.55 C. What is the pressure?
9.
What is the density of chlorine gas at STP?
10. How many grams are present in a 55.5 L sample of carbon dioxide at STP?
Enthalpy change for a reaction: Let’s do #27-29 on pp. 371. You may need to use the chart of
heats of formation found within Chapter 10.
Name___________________________
CHEMISTRY FINAL EXAM REVIEW GUIDE
CHAPTERS 12, 14, and 15
TERMS AND CONCEPTS:
Mixture
Solution
Colloid
Suspension
Alloy
Molarity
Molality
Parts per million
Electrolytes
Miscible
“like dissolves like”
Arrhenius acid/base
Bronsted-Lowry acid/base
pH
pH scale
properties of acids
properties of bases
strong acids
strong bases
self-ionization of water
Kw
titration
equivalence point
buret
purpose of a titration
indicator
SKILLS/PROBLEM TYPES:
Molarity
Molality
Parts per million
Naming acids
pH/pOH problems
PRACTICE PROBLEMS:
1.
What is the molarity of a 750 mL solution that contains 59.9 grams of NaCl?
2.
How many grams of KNO3 should be added to water to make 650 mL of a 1.5 M KNO3 solution?
3.
How many moles of KOH must be added to 500 grams of water to make a 2.5 molal solution?
4.
A 500 gram sample of pond water contains 75 mg of lead. What is the concentration of lead in
ppm?
5.
A 350 gram sample of dirt contains 25 mg of radon. What is the concentration of radon in
ppm?
6. Name each acid please:
a. HNO4 ________________
b. HI____________________
c. H2SO2_________________
d. H3PO4_________________
e. HBr____________________
7.
Give the formula for each acid please:
a. Hypochlorous acid_________________
b. Hydrofluoric acid___________________
c. Persulfuric acid_____________________
d. Carbonous acid_______________________
e. nitric acid___________________________
8.
Give the pH, pOH, hydronium concentration , and hydroxide concentration for each of the
following please:
a. 0.25 M HNO3
b. 2.3 x 10 -3 M Ca(OH)2
c. 1.5 M H2SO4
d. 2.5 x 10 -5 M KOH
Name_______________________
CHEMISTRY FINAL EXAM REVIEW GUIDE
CHAPTERS 21 and 22
TERMS AND CONCEPTS:
Isotopes
Two ways to write isotopes
Mass defect
Fission
Fusion
Half-life
Beta decay
Alpha decay
Electron capture
Nuclide
Nucleons
Radioactivity
organic compound
alkanes
alkenes
alkynes
cyclic hydrocarbons
aromatic hydrocarbons
functional group
isomers
prefixes for organic compounds
4 types of organic reactions
polymers
SKILLS/PROBLEM TYPES:
Write and balance nuclear equations
--alpha decay, beta decay, and electron capture
Half-life problems
Name unsubstituted alkanes, alkenes, alkynes, and cyclic hydrocarbons
Name substituted alkanes, alkenes, and alkynes
Classify compounds by their functional group (alcohols, aldehydes, ketones, and carboxylic acids)
PRACTICE PROBLEMS:
1. Write the nuclear reaction for each please:
a. Beta decay of hydrogen-3
b. Electron capture by sodium-22
c. Alpha decay of polonium-210
d. Beta decay of sulfur-35
2. The half-life of an isotope is 2.0 years. How many years would it take for a 4.0 mg sample to
decay and have only 0.50 mg remain?
3. Selenium—83 has a half life of 25.0 minutes. How many minutes would it take for a 10.0 mg
sample to decay and have only 1.25 mg of it remain?
4. Actinium—226 has a half-life of 29 hours. IF 100 mg of actinium—226 disintegrates over a
period of 58 hours, how many mg of actinium—226 will remain?
5. Give the missing name or formula for each hydrocarbon please:
a. Butane________________
b. Ethyne________________
c. Cyclohexene________________
d. Nonane____________________
e. C3H8 ______________________
f. C5H10_______________________
g. C10H18______________________
6. Name each hydrocarbon please:
We will practice some of these on the board.
7.
Draw each hydrocarbon please:
a. Cyclopropene
b. 3-pentyne
c. 3-ethyl-2-hexene
d. 2,2-dimethyl propane
e. 4-ethyl-2,5-dimethyl heptanes
f. 2-methyl-2-butene