Chemistry review
Chapter 1:
1. 4.0
2. a. 2.2%
b. 2.2%
3. a. 2
b. 4
c. 4
d. 4
e. 1
10.28
15
f. 3
g. 4
h. 7
i. 3
4. a. 3.1 x 10 -4
b. 3.1 x 107
c. 3.6 x 104
d. 4.0 x 10-6
5. a. 5 x102
b. 4.8 x 102
c. 4.80 x 102
6. a. 102.623
b. 236.2
c. 1.9
d. 33.03
7. a. 0.6 pennyweight
b. 72 g
c. 19.3 cm3
8. Same amount because they are the same volume
9. A. 351.1 K
b. 248 K
c. 0 K
d. 1074 K
10. 0.26 cm3
11. 9.8 g; 49 carats
12. 3.8 g/mL
13. The one that floats because it is less dense
14. Solid: particles are close together and vibrate in place
Liquid: particles flow past each other but are close together
Gas: particles are far apart and move quickly
15. Homogeneous= looks the same throughout
Heterogeneous= looks different
16. a. pure, compound
b. mixture
c. mixture
d. pure, element
e. mixture
f. pure, element
g. mixture
h. mixture
i. pure, compound
17. In a physical change, the substance does not change identify but in a chemical change it does change its identify.
18. Precipitate, color change, heat or light, gas (bubbles)
19. A. mixture- physical
b. compound-chemical
c. mixture, physical
Chapter 2:
1. Thomson- discovered electron with cathode ray tube
Becquerel
Rutherford-discovered nucleus with gold foil experiment
Dalton thought that the atom was the smallest unit of matter but these discoveries showed that there were
smaller particles that made up the atom
2. Atomic number tells the number of protons and the mass number tells the protons + neutrons
3. The atomic mass is the mass of a specific isotope of an atom, the average atomic mass is the weighted average
of all the isotopes of an element.
4. An atom with the same number of protons but different number of neutrons or mass
5. A. 22,20
d. 36,50
b. 30, 34
e. 33,42
c. 32, 44
f. 19, 22
6. A. O-17
b. Cl-37
c. Co-60
d. Fe-57
e. I-131
f. Li-7
7.
8.
9.
10.
63.546 Copper
207.2169 lead
Family/group is a vertical column and periods are horizontal rows
A. alkaline earth metals
b. noble gas
11. Sn-118, +2
12. B and d
13. A. Te
b. Rb
c. Ar
d. At
14. A. lose, +1
b. lose, +2
c. gain, -3
d. lose, +2
e. gain, -1
f. gain, -2
15. A. 26, 24; FeO
b. 26, 23; Fe 2 O 3
c. 56, 54; BaO
d. 55, 54; Cs 2 O
e. 16, 18; Al 2 S 3
f. 15,18; AlP
16. Ra; 142
g. lose, +3
h. gain, -2
g. 35,36; AlBr 3
h. 7, 10; AlN
Nomenclature practice:
1. Write formulas for the following substances:
a. Barium sulfate ______BaSO 4 _________________
b. Ammonium chloride ___NH 4 Cl_______________
c. Chlorine monoxide ______ClO__________
d. Silicone tetrachloride ____SiCl 4 _____________
e. Magnesium fluoride _______MgF 2 _________
f. Sodium oxide ___________Na 2 O________
g. Sodium peroxide_________Na 2 O 2 _________
h. Copper (I) iodide ______CuI_______________
dichromate_____________
i. Zinc sulfide __________ZnS_____________
j. Potassium carbonate _____K 2 CO 3 _____________
k. Hydrobromic acid ________HBr_______
l. Perchloric acid ___________HClO 4 __________
m. Lead (II) acetate __________Pb(C 2 H 3 O 2 ) 2 ________
n. Sodium permanganate ____NaMnO 4 ___________
o. Lithium oxalate ____________Li 2 C 2 O 4 _____
p. Potassium cyanide __________KCN__________
q. Iron (III) hydroxide __Fe(OH) 3 ________________
r. Silicone dioxide ___SiO 2 ____________________
s. Nitrogen trifluoride ___NF 3 ________________
t. Chromium (III) oxide ___Cr 2 O 3 _______________
u. Calcium chlorate ________Ca(ClO 3 ) 2 __________
v. Sodium acetate __NaC 2 H 3 O 2 _________________
w. Cobalt (III) nitrate ______Co(NO 3 ) 3 _____________
x. Nitrous acid ____HNO 2 ______________________
y. Ammonium phosphate ___(NH 4 ) 3 PO 4 _____________
z. Potassium chromate _____K 2 CrO 4 _____________
2. Name each of the following compounds
a. Cu 2 O__copper (I) oxide_________________
b. PCl 3 _________phosphorus trichloride____
c. Li 3 N__litium nitride___________________
d. BaSO 3 ___barium sulfite________________
e. N 2 F 4 ___dinitrogen tetrafluoride_________________
f. KClO 4 _____potassium perchlorate_______________
g. NaH___sodium hydride_________________
h. (NH 4 ) 2 Cr 2 O 7 _ammonium
i. HNO 2 ___nitrous acid________________
j. Sr 3 P 2 ____strontium phosphide___________
k. Mg(OH) 2 ___magnesium hydroxide_____________
l. Al 2 S 3 __aluminum sulfide____________
m. AgBr__silver bromide___________
n. P 4 O 10 __tetraphosphorus decoxide_________
o. HC 2 H 3 O 2 __acetic acid__________
p. CaI 2 __calcium idode___________
q. MnO 2 __manganese (IV) oxide___________
r. Li 2 O__lithium oxide___________
s. FeI 3 ___iron (III) iodide_________
t. Cu 3 PO 4 ___copper (I) phophate___________
u. HCl___hydrochloric acid___________
v. NaCN_sodium cyanide____________
w. Cs 3 N__cesium nitride____________
x. Zn(NO 3 ) 2 __zinc nitrate___________
y. N 2 O___dinitrogen monoxide__________
z. H 3 PO 3 __phosphorous acid___________
3. For each equation below, identify the type (synthesis, decomposition, single replacement, double replacement, or
combustion), and then write the balanced reaction.
a. Ammonium sulfate reacts with barium nitrate to form ammonium nitrate and barium sulfate
(NH 4 ) 2 SO 4 + Ba(NO 3 ) 2  2NH 4 NO 3 + BaSO 4
b. Zinc metal is added to a solution of copper (II) chloride to form zinc chloride and copper metal
Zn + CuCl 2  ZnCl 2 + Cu
c. Propane gas (C 3 H 8 ) is burned in excess oxygen to form carbon dioxide and water.
C 3 H 8 + 5O 2  3CO 2 + 4H 2 O
d. Solid calcium chlorate is heated strongly decomposing into calcium chloride and oxygen gas.
Ca(ClO 3 ) 2  CaCl 2 + 3O 2
e. Magnesium and nitrogen gas are heated together to form magnesium nitride
4Mg + 3N 2  2Mg 2 N 3
f. Chlorine gas is bubbled through a solution of sodium bromide to form sodium chloride and bromine.
Cl 2 + 2NaBr  2NaCl + Br 2
g. Solutions of lead (II) nitrate and calcium iodide are combined to form lead iodide and calcium nitrate.
Pb(NO 3 ) 2 + CaI 2  PbI 2 + Ca(NO 3 ) 2
h. Sulfuric acid is combined with sodium hydroxide to form sodium sulfate and water.
H 2 SO 4 + 2NaOH  Na 2 SO 4 + 2H 2 O
i.Isopropyl alcohol (C 3 H 7 OH) is burned in oxygen to form carbon dioxide and water
2C 3 H 7 OH + 9O 2  6CO 2 + 8H 2 O
j. Iron metal shavings are added to hydrochloric acid to from iron(II) chloride and hydrogen gas.
Fe + 2HCl  FeCl 2 + H 2
k. Solid sodium carbonate is heated in a crucible and forms sodium oxide and carbon dioxide
Na 2 CO 3  Na 2 O + CO 2
l. Na + 2H 2 O NaOH + H 2
Chapter 3
1. A. 2,1,2
b. 1,1,2
c. 1,4,1,5
d. 1,4,1,4
e. 2,13,10,10
f. 1,3,1,3
g. 2,2,1
h. 1,3,2
i. 1,3,1,3
j. 1,1,32
k. 2,1,1,2
l. 2,3,1,6
m.4,9,4,10
n. 1,1,1,4
2. A. 2KClO 3  2KCl + 3O 2
b. Zn + H 2 SO 4  H2ZnSO 4
c. PCl 3 + 3H 2 O  H 3 PO 3 + 3HCl
d. 3H 2 S + 2Fe(OH) 3  Fe 2 S 3 + 6H 2 O
3. A. 294 g/mol
b. 12.8211 mol
c. 73.077 x 1023 molecules
d. 2.42 x 1023 atoms
4.
5.
6.
7.
0.0116 mol
6.61 g
80.4 g
284.73 g/mol