Review problems for final
FORMULAS [CHAPTER 7]
Name each:
1) CuS
2) SrSO4
3) NH4OH
4) NO2
5) AgCH3COO
6) Ni3(PO4)2
7) Zn(MnO4)2
8) Mg(NO3)2
9) AlN
10) K3P
11) HNO2 (aq)
12) SnO
13) P2O5
14) MnCO3
15) NaHCO3
1) potassium fluoride
2) barium nitrite
3) aluminum phosphide
4) sulfuric acid
5) strontium selenide
6) iron(II)bromate
7) lithium bromide
8) copper(I) oxide
9) chromium(III)sulfate
10) silver phosphate
11) sulfur tribromide
12) silicon tetrafluoride
13) magnesium cyanide
14) nickel (II) acetate
15) calcium hydroxide
Write formulas for each:
MOLES [CHAPTER 10]
1. What is the empirical formula of a compound that contains 53.73% iron and 46.27% sulfur?
2. A compound is 56.4% phosphorus and 43.7% oxygen with a molecular mass of 220u. What is its molecular
formula?
3. A hydrate is 50.66% anhydrous calcium chloride and 49.34% water. What is the formula and name for this
hydrate?
4. What is the percent of water in nickel(II)sulfate hexahydrate?
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5. What is the empirical formula for C6H12O6 ? (1pt)
for Al2(SO4)3 ? (1pt)
6. What is the molarity of a solution containing 10.0 grams of sodium hydroxide dissolved in 750 mL of solution?
[6pts]
7. In the lab, there is a bottle containing 125 cm3 of a 0.100 M solution of Cr(NO3)3. How many grams of
chromium(III)nitrate are in it? [6pts]
8. Do the following conversions.
a) Convert 8.68 grams of lithium bromide to formula units
b) Convert 0.365 grams of hydrochloric acid to moles
c) Convert 3.01 x 1019 atoms of carbon to grams.
d) Convert 1.50 moles of calcium hydroxide to grams.
EQUATIONS [CHAPTER 9]
DIRECTIONS: FINISH WORD EQUATION, STATE TYPE OF REACTION , WRITE A FULLY BALANCED FORMULA EQUATION
1.
potassium +
water
2.
silver nitrate +
3.
calcium chlorate 

calcium phosphate

2
magnesium hydroxide 
4.
phosphoric acid
+
5.
decane [C10H22]
+ oxygen 
6.
aluminum +
7.
potassium + oxygen 
magnesium chloride 
8. aluminum hydroxide 
9. rubidium bromide + chlorine 
10. barium chloride + sodium carbonate 
STOICHIOMETRY [CHAPTER 11]
1. How many grams of zinc chloride can be produced if 15.3 grams of hydrochloric acid reacts with excess zinc?
2. How much chlorine (mass) should be produced if 84.2 grams of aluminum chloride and some bromine are
reacted?
3. 64.9 grams of potassium chloride are reacted with excess oxygen to produce potassium chlorate. If 77.1 grams
are produced, what is the percent yield of this reaction?
4. You have 83.6 grams of hydrogen and some nitrogen which combine to form ammonia gas. How much
ammonia can be produced? If you do this in a lab and obtain 124 grams of ammonia, what is your percent
yield?
5. Aluminum metal is burned in oxygen gas.
a. Write the balanced equation for this reaction.
b. What mass of product can be made?
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BONDING [CHAPTER 8]
Write whether each is Ionic, Covalent, Both, or Neither
1.
2.
3.
4.
5.
6.
7.
8.
9.
10.
11.
12.
13.
14.
15.
16.
17.
18.
19.
20.
21.
22.
23.
24.
25.
conducts when melted
brittle solids
well defined crystals
can form very large compounds
molecules
soluble in water
low melting points
may be solids, liquids, or gases
sugar
table salt
shown as empirical formulas
made of ions
show charges for
molecular formulas
occurs between metals and nonmetals
occurs between two nonmetals
within diatomic molecules
share electrons
can show dot diagrams for
usually don’t conduct
aqueous solutions conduct
strong bonds
weak bonds
conducts in solid phase
may be partially charged
1.
Would iodine crystals dissolve in water? Would they dissolve in carbon tetrachloride? Why or why not?? Justify
your answer with bonding principles.
2.
Show Lewis structures for each:
a) rubidium chloride
b) barium oxide
c) francium oxide
e) carbon tetrafluoride
f) nitrate ion
g) hydroxide ion
d) ammonia gas
h) ethanol (C2H6O)
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i) phosphorus pentabromide
j) ozone (O3)
k) carbon dioxide
l) nitrous oxide (N2O)
GAS LAWS [CHAPTERS 12 & 13]
1.
A balloon measures 568 mL at 99.8 kPa. What is its volume at 125 kPa (assuming no temperature change)?
2.
What pressure would be needed to have a balloon go from 225 ml to 0.950 L, if it started at 12.7 pounds per square inch?
(no temperature change)
3.
A gas measures 500 cm3 at 25C. What is its volume at 50C? (no pressure change)
4.
What temperature, in Fahrenheit, is needed to change the volume of a gas from 75.5 dm 3 to 45.0 dm3, if it was first
measured at 72F? (no pressure change)
5.
A gas was measure to be 500 mL at STP. What is its volume at 25C and 0.988 atm?
6.
A gas sample is held at constant pressure. It occupies 5.67 L when the temperature is 21.6. Determine the volume it
would occupy at standard temperature.
7.
Some helium measure 456 cm3 at 15C and 750 torr. What temperature, in Celsius, is needed to change the volume to
523 cm3 at standard pressure?
8.
A gas sample is heated from -20C to 57C and the volume is increased from 2.00L to 4.50 L. If the initial pressure is
0.125 atm, what is the final pressure?
9.
What volume would 22.0 grams of carbon dioxide gas occupy at 0.913 atm and -10C?
10. What would be the mass of 2.67 Liters of oxygen gas measured at 745 torr and 20F?
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