Term 2 Final Exam Review Question Answers
Pg. 87 #17-24
17. 12,000 g
18. 50. mm
19. 0.128 L
20. 0.081 ms
21. 1011 pg
22. 400
23. 1031
24. 0.9814 g/cm3
Pg. 188, #3, 4, 6, 8, 9, 21-23, 25
3. A
4. D
6. B
8. B
9. C
21. Hydrogen does not truly belong to any family of elements
22. They have one valence electron beyond their inner core that is relatively
easy to lose, resulting in an ion with a 1+ charge.
23. The are one electron short of 8 electrons in their outer energy level. As a
result, they commonly obtain an extra electron, forming an ion with a 1charge.
25. The increasing number of protons pulls the electrons closer to the
nucleus.
Pg. 216 #1-9, 28
1. C
6. B
2. D
7. A
3. C
8. C
4. C
9. C
5. D
28. Their outermost electron shells have the stable s2p6 configuration (s2 for
helium).
Pg. 220 #7-10, 22, 27, 31, 35-39, 43
7. Alpha radiation is a stream of helium nuclei. Beta rays are electrons;
gamma rays are high-energy rays, similar to x-rays.
8. Positively charged protons and neutral neutrons are found in the nucleus
with a cloud of negativity charged electrons surrounding them. Protons
and neutrons have a mass of 1 amu; electrons have a mass of 1/1800 amu.
9. Atomic number = number of protons; mass number = number of protons +
number of neutrons. Electric charge indicates gain or loss of electrons.
10. They have the same number of protons and electrons, but different
numbers of neutrons
22. In general, larger atoms have lower ionization energies because their
electrons are in higher energy levels farther from the nucleus.
27. (a) 80 p+, 121 n0, 78 e(b) 53 p+, 74 n0, 54 e31. 6630Zn
35. (a) Sr = [Kr]5s2
(b) Lu = [Xe]6s24f145d1
36. (a) Ca
(b) I
37. (a) S = [Ne]3s23p4
(b) Hg = [Xe]6s24f145d10
38. P, As, Ge
39. I+, I, I43. In3+ = [Kr]4d10
Pg. 252 #1-9, 19. 21-25, 28, 34
1. B
6. C
2. D
7. C
3. B
8. D
4. A
9. C
5. D
19. Atoms tend to gain, lose, or share electrons in order to acquire a full set
of valence electrons. It helps us predict the way atoms bond.
21. Cations have a positive charge. Anions have a negative charge.
Monatomic ions are one-atom ions. Polyatomic ions are multiple-atom ions.
22. A single bond has one shared pair of electrons, a double bond has two,
and a triple bond has three.
23. The charge of the copper ion is different. The Roman numerals show the
first to be Cu1+ and the second to be Cu2+.
24. A substance that dissolves in water to produce H+ ions. Like ionic
compounds, acids separate into a cation and an anion on water.
25. When the electronegativity of one atom in a bond is significantly
different from that of the other atom, a polar bond results. When the
atoms have electronegativities that are close of the same, a nonpolar
bond results.
28. (a) AgNO3
(d) H2SO4
(b) Mg(OH)2
(e) Pb(C2H3O2)2
(c) CCl4
(f) Fe(NO3)3
34. (a) antimony sulfide
(d) carbonic acid
(b) iron (II) sulfide
(e) silicon dioxide octahydrate
(c) sodium oxide
(f) calcium sulfate dihydrate
Pg. 276 #1-6, 8, 9, 21, 25, 30
1. D
5. A
2. B
6. C
3. B
8. A
4. D
9. A
21. The polarity of a molecule is determined by the shape of the molecule
and the type of bond within it. Polar bonds must be present to create the
slight positive and negative charges. The shape of the molecule
determines whether or not the charges are balanced in the molecule.
25. (a) Nonpolar. Br2 has no polar bonds
(b) Polar. Oxygen is more electronegative than carbon.
(c) Polar. Polar bonds exist and two pairs of unshared valence electrons
result in a bent shape.
(d) Nonpolar. The 6 flourine atoms are grouped evenly around the sulfur
atom.
(e) Nonpolar. The chlorine atoms are arranged on opposite side of the
atom and form a 180 bond angle.
(f) Polar. This molecule has a linear shape, but differences in
electronegativity between the two atoms cause the molecule to be
polar.
30. (a) Bent, sp3
(c) Pyramidal, sp3
(b) Tetrahedral, sp3
(d) Linear, sp3
Pg. 300 #1, 3-8, 24, 25, 39
1. C
6. B
3. C
7. A
4. D
8. B
5. D
24. (a) 4 P + 5 O2  2 P2O5
(b) 2 NaNO3  2 NaNO3 + O2
(c) 2 C8H18 + 25 O2  16 CO2 +18 H2O
(d) H2SO4 + 2 NaOH  Na2SO4 + 2 H2O
25. (a) Decomposition. A complex substance has decomposed into two
simpler substances
(b) Double-replacement reaction. Ions form from different compounds
have replaced each other.
(c) Single-replacement reaction. An uncombined element has replaced an
atom in an ionic compound.
(d) Direct combination action. Two substances have combined to form a
new compound.
39. (a) 2 NH3  N2 + 3 H2, decomposition.
(b) 3 Ba(C2H3O2)2 + 2 Na3PO4  Ba3(PO4)2 + 6 NaC2H3O2, doublereplacement.
(c) Zn + 2HCl  ZnCl2 + H2, single-replacement.
(d) 2 Hg + O2  2 HgO, direct combination.
Pg. 306 #15-29, 32-41
15. Nitric acid – acid
16. Calcium iodide – ionic compound
17. Iron (III) oxide – ionic compound
18. Dinitrogen tetroxide – molecule
19. Hydroflouric acid – acid
20. Copper (II) phosphate – ionic compound
21. Ammonium chloride – ionic compound
22. Carbon monoxide – molecule
23. Tetrahedral – nonpolar
24. Bent – polar
25. Linear – nonpolar
26. Linear – polar
27. Trigonal planar – polar
28. Trigonal planar – nonpolar
29. Trigonal planar – polar
32. Decomposition: 2 Al(OH)3  Al2O3 + 3H2O
33. Direct combination: 4 Fe + 3 O2  2 Fe2O3
34. Single-replacement
35. Direct combination: 2H2 +O2  2H2O
36. Direct combination: 2Na + Cl2  2NaCl
37. Decomposition
38. Double-replacement
39. Single replacement: 2AgNO3 + Zn  Zn(NO3)2 + 2Ag
40. Double-replacement: Al2(SO4)3 + 3BaCl  2AlCl3 + 3BaSO4
41. 2C2H6 +7O2  4CO2 + 6H2O
Pg. 342 #1-9
1. A
2. A
3. B
4. D
5. B
6. B
7. A
8. C
9. B
Pg. 376 #1-7, 56, 58
1. A
5. D
2. D
6. A
3. B
7. A
4. B
56. 373 L O2
58. (a) 2.64 g Cu
(b) Percent yield = Actual yield/expected yield x 100%
= 2.51 g Cu/2.64 g Cu x 100% = 95.1%
Pg. 412 #11-14
11. (a) 82.3 g
(b) 108. L
12. 2.498 mol C
13. 12.6 g Li
14. 3.33 L H2; 1.67 L O2
Pg. 590 #1, 2, 9
1. A solution is a homogeneous mixture of two or more substances in a
single state. A solution can be separated into its individual components by
distillation or crystallization.
2. Substance dissolved is the solute. (such as salt in seawater) Dissolving
agent is the solvent. (water in seawater)
9. Raise the temperature, or stir.
Pg. 652 #1, 3, 4, 9
1. Acids—taste sour, conduct electricity, react with metals, turn blue litmus
paper red, neutralize bases.
Bases—taste bitter, feel slippery, conduct electricity, turn red litmus paper
blue, neutralize acids.
3. HCl (acid) + NaOH (base)  NaCl (salt) + H2O
4. A strong acid completely dissociates to form H+ ions; a weak acid only
partially does so.
9. See Figure 18-25 in your book.
Pg. 898 #1, 2, 17, 21
1. Fission—the splitting of the atomic nucleus of a heavy element into two
lighter elements.
Fusion—light nuclei are combined under thermonuclear conditions to
create larger nuclei
2. Gamma radiation is much more energetic than alpha or beta.
17. (a) inorganic – carbon dioxide
(d) inorganic – calcium carbonate
(b) organic – ethane
(e) organic – ethanamine
(c) organic – acetic acid
21. C6H12O6 + 6O2  6H2O + 6CO2
Photosynthesis is the opposite reaction