Chemistry II Summative #1 Study Guide
Multiple Choice
Identify the choice that best completes the statement or answers the question.
Figure 5-3
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1. Which numbered region in Figure 5-3 represents the p-block of elements?
a. 1
c. 3
b. 2
d. 4
2. Which numbered region in Figure 5-3 represents the f-block of elements?
a. 1
c. 3
b. 2
d. 4
3. Which numbered region in Figure 5-3 represents the s-block of elements?
a. 1
c. 3
b. 2
d. 4
4. Which numbered region in Figure 5-3 represents the d-block of elements?
a. 1
c. 3
b. 2
d. 4
5. Which numbered regions in Figure 5-3 contain the representative elements?
a. 1 and 2
c. 1 and 3
b. 2 and 3
d. 1, 2, and 3
6. Which numbered region in Figure 5-3 represents the transition metals?
a. 1
c. 3
b. 2
d. 4
7. Which numbered region in Figure 5-3 represents the inner transition metals?
a. 1
c. 3
b. 2
d. 4
8. Which lettered region in Figure 5-3 represents the nonmetals?
a. a
c. c
b. b
d. none of the regions
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9. Which lettered region in Figure 5-3 represents the semimetals?
a. a
c. c
b. b
d. none of the regions
Figure 5-4
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10. Based on Figure 5-4, what general trend exists for first ionization energy across a period, from left to right?
a. Ionization energy increases.
b. Ionization energy decreases.
c. Ionization energy remains fairly constant.
d. Ionization energy first increases, then decreases.
11. Based on Figure 5-4, what general trend exists for first ionization energy down a group?
a. Ionization energy increases.
b. Ionization energy decreases.
c. Ionization energy remains fairly constant.
d. Ionization energy first increases, then decreases.
12. In Figure 5-4, which group tends to have the highest ionization energy? The lowest?
a. halogens; alkaline earth metals
c. alkali metals; noble gases
b. alkaline earth metals; halogens
d. noble gases; alkali metals
13. In Figure 5-4, which period tends to have the highest ionization energy? The lowest?
a. 1; 4
c. 2; 3
b. 4; 1
d. 3; 2
14. As atoms bond with each other, they
a. increase their potential energy, thus creating less-stable arrangements of matter.
b. decrease their potential energy, thus creating less-stable arrangements of matter.
c. increase their potential energy, thus creating more-stable arrangements of matter.
d. decrease their potential energy, thus creating more-stable arrangements of matter.
15. If two covalently bonded atoms are identical, the bond is
a. nonpolar covalent.
c. dipole covalent.
b. polar covalent.
d. coordinate covalent.
16. When atoms share electrons, the electrical attraction of an atom for the shared electrons is called the atom's
a. electron affinity.
c. resonance.
b. electronegativity.
d. hybridization.
CONCEPT MASTERY
Use the diagrams to answer the questions or complete the statements.
1A
Li
Na
K
Rb
Cs
2A
Be
Mg
Ca
3A
B
Al
4A
C
Si
5A
N
P
6A
O
S
7A
F
Cl
Br
8A
Ne
Ar
Kr
Xe
Figure 7-1
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17. Use Figure 7-1 to determine the symbol of the ion that has the electron configuration [Ar]3d104s24p6.
a. K+
c. Br2–
+
b. Rb
d. Cl–
18. Use Figure 7-1 to determine four other elements whose ions have the same electron configuration as that of an ion of
sodium.
a. Mg, Al, F, O
c. Mg, Al, S, Cl
b. Li, K, Rb, Cs
d. Ne, Mg, Al, Si
19. In Figure 7-1, the ions of which three elements have the same electron configuration as Ar?
a. Ne, Kr, Xe
c. Cl, F, Br
b. S, Cl, Ca
d. Na, Mg, Cl
20. Determine the formula of the compound formed between calcium and hydroxide ions.
a. CaOH
c. CaOH2
b. Ca(OH)2
d. Ca2OH
21. Determine the formula of the compound formed between calcium and sulfate ions.
a. CaS
c. Ca2S2
b. Ca2(SO4)2
d. CaSO4
22. Determine the formula of the compound aluminum phosphide.
a. AlP
c. Al(PO)4
b. AlPO4
d. Al3(PO4)3
23. Determine the formula of copper(II) chloride.
a. Cu2Cl
c. CuCl
b. (CuCl)2
d. CuCl2
24. Determine the formula of iron(III) nitrate.
a. Fe(NO3)3
c. Fe3NO3
b. FeN
d. None of these is correct.
25. What is the formula of sulfuric acid?
a. HS
c. H2SO4
b. H2S
d. HSO4
26. What is the formula of hydrochloric acid?
a. HOCl
c. H2Cl2
b. HCl
d. H2(ClO)2
Element
Electronegativity
F
4.0
O
3.5
Cl
3.0
Br
2.8
C
2.5
H
2.1
P
2.1
B
2.0
Mg
1.2
Ca
1.0
Na
0.9
K
0.8
Figure 7-3
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27. Using Figure 7-3, predict the kind of bond that will form between boron and hydrogen.
a. nonpolar covalent
c. ionic
b. polar covalent
d. intermolecular covalent
28. Using the information in Figure 7-3, predict the physical state of the compound formed between magnesium and oxygen
at the temperature of boiling water.
a. probably a gas
b. probably a liquid
c. probably a solid
d. impossible to determine from the given data
29. Using the information in Figure 7-3, predict the physical state of the compound formed between phosphorous and
hydrogen, PH3, at the temperature of boiling water.
a. probably a gas
b. probably a liquid
c. probably a solid
d. impossible to determine from the given data
30. Use Figure 7-3 to determine the charge distribution in a molecule of sodium and bromine.
a. Sodium gains a slight negative charge.
b. Bromine gains a slight positive charge.
c. Bromine gains a slight negative charge.
d. The charge is distributed evenly.
31. Using Figure 7-3, what kind of compound would be formed between potassium and bromine?
a. nonpolar covalent
c. ionic
b. polar covalent
d. macromolecular covalent
32. Using Figure 7-3, which two elements would form the most ionic bond possible?
a. F–F
c. Ca–O
b. F–O
d. K–F
33. Using Figure 7-3, which two elements would form the most nonpolar covalent bond possible?
a. F–K
c. H–P
b. Ca–Na
d. Na–K
Figure 7-4
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34. In Figure 7-4, what type of bonding should replace letter a?
a. covalent
c. nonpolar covalent
b. polar covalent
d. ionic
35. In Figure 7-4, what type of bonding should replace letter b?
a. covalent
c. nonpolar covalent
b. polar covalent
d. ionic
36. In Figure 7-4, what type of bonding should replace letter c?
a. covalent
c. nonpolar covalent
b. polar covalent
d. ionic
37. The equation A + BX  AX + B is the general equation for a
a. double-displacement reaction.
c. single-displacement reaction.
b. decomposition reaction.
d. combustion reaction.
38. In what kind of reaction do the ions of two compounds exchange places in aqueous solution to form two new
compounds?
a. synthesis reaction
c. decomposition reaction
b. double-displacement reaction
d. combustion reaction
39. The reaction represented by the equation 2Mg(s) + O2(g)  2MgO(s) is a
a. synthesis reaction.
c. single-displacement reaction.
b. decomposition reaction.
d. double-displacement reaction.
40. The reaction represented by the equation Mg(s) + 2HCl(aq)  H2(g) + MgCl2(aq) is a
a. composition reaction.
c. single-displacement reaction.
b. decomposition reaction.
d. double-displacement reaction.
41. The reaction represented by the equation 2HgO(s)  2Hg(l) + O2(g) is a(n)
a. single-displacement reaction.
c. combustion reaction.
b. synthesis reaction.
d. decomposition reaction.
42. The reaction represented by the equation Pb(NO3)2(aq) + 2KI(aq)  PbI2(s) + 2KNO3(aq) is a
a. double-displacement reaction.
c. decomposition reaction.
b. synthesis reaction.
d. combustion reaction.
43. The reaction represented by the equation 2KClO3(s)  2KCl(s) + 3O2(g) is a(n)
a. synthesis reaction.
c. combustion reaction.
b. decomposition reaction.
d. ionic reaction.
44. The reaction represented by the equation Cl2(g) + 2KBr(aq)  2KCl(aq) + Br2(l) is a(n)
a. synthesis reaction.
c. single-displacement reaction.
b. decomposition reaction.
d. combustion reaction.
45. In one type of synthesis reaction, an element combines with oxygen to yield a(n)
a. acid.
c. oxide.
b. hydroxide.
d. metal.
46. Oxides of active metals, such as CaO, react with water to produce
a. metal carbonates.
c. acids.
b. metal hydrides.
d. metal hydroxides.
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47. An active metal and a halogen react to form a(n)
a. salt.
c. acid.
b. hydroxide.
d. oxide.
48. When a binary compound decomposes, what is produced?
a. an oxide
c. a tertiary compound
b. an acid
d. two elements
49. Many metal hydroxides decompose when heated to yield metal oxides and
a. metal hydrides.
c. carbon dioxide.
b. water.
d. an acid.
50. In the equation 2Al(s) + 3Fe(NO3)2(aq)  3Fe(s) + 2Al(NO3)3(aq), iron has been replaced by
a. nitrate.
c. aluminum.
b. water.
d. nitrogen.
Problem
51. Complete and balance the following equation.
Al Cl
52. Complete and balance the following equation.
CH
O
CO
53. Complete and balance the following equation.
Fe (SO )
Ba(OH)
54. Balance the following equation. Indicate whether combustion is complete or incomplete.
C H
O
CO H O
55. Complete and balance the following equation:
K PO
BaCl
56. Consider the description: copper(II) oxide reacts with sulfuric acid to produce copper(II) sulfate and water. List the steps
required to write its balanced chemical equation. State how to determine which of the five general types of reaction this
represents.
57. Predict the precipitate that forms when aqueous solutions of silver nitrate and potassium chloride react to form products
in a double-replacement reaction. Include a discussion of how to write the complete chemical equation describing this
reaction.
58. How does the figure below illustrate Hund's rule?
59. How does the figure above illustrate the Pauli exclusion principle?
60. The electron configuration for nitrogen is 1s2 2s2 2p3. What does the 3 in 2p3 mean?
61. Differentiate between an ionic compound and a molecular compound.
62. Draw the orbital diagram for phosphorus.
63. Draw a Lewis structure for carbon disulfide, CS2.
64. Tell what type of chemical reaction is represented by the following formula equation. Then balance the equation.
C3H8(g) + O2(g)
CO2(g) + H2O(l)
65. Use the activity series to determine if the following reaction is possible. If it is possible, write the products and balance
the equation. If not, explain.
2K(s) + ZnCl2(aq)
66. Using a periodic table, write the formula for an ion that contains 34 protons and 36 electrons.
67. Using a periodic table, write the formula for an ion that contains 19 protons and 18 electrons.
68. Using a periodic table, determine the number of protons, neutrons, and electrons in the ion
Cr3+.
69. Identify the element that has the following electron configuration: 1s22s22p63s23p64s23d104p65s24d105p2. How many
unpaired electrons are present?
70. Write the electron configuration for francium (Fr, atomic number 87). How many unpaired electrons are present?
71. How many different kinds of covalent bonds can a nitrogen atom form? Explain.
72. The two chemical equations below appear to describe the same chemical reaction. Explain how the two reactions are
different from each other. Hypothesize any differences you might be able to observe in these two reactions represented
by the following equations.
Mg(s) + 2H2O(l)  Mg(OH)2(aq) + H2(g)
Mg(l) + 2H2O(g)  Mg(OH)2(aq) + H2(g)
Chemistry II Summative #1 Study Guide
Answer Section
MULTIPLE CHOICE
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ANS:
C
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A
B
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D
C
B
A
B
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A
3
B
3
B
A
B
B
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A
D
A
C
B
A
C
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D
C
D
D
A
C
1
B
1
A
2
C
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1
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1
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1
1
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1
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1
1
1
1
OBJ:
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DIF:
DIF:
5E 5.d
5E 5.d
5E 5.d
5E 5.d
5E 5.d
5E 5.d
5E 5.d
5E 5.d
5E 5.d
5E 5.f
5E 5.f
5E 5.f
5E 5.f
I
I
OBJ:
REF:
2
1
PTS:
1
DIF:
I
REF:
1
PTS:
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1
1
1
1
1
1
1
1
1
1
1
1
1
1
1
1
1
1
1
1
1
OBJ:
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OBJ:
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DIF:
7G 7.b
7G 7.b
7G 7.b
7G 7.b
7G 7.b
7G 7.b
7G 7.b
7G 7.b
7G 7.b
7G 7.b
7G 7.d
7G 7.d
7G 7.d
7G 7.d
7G 7.d
7G 7.d
7G 7.d
7G 7.d
7G 7.d
7G 7.d
II
REF:
2
PTS:
1
DIF:
I
REF:
2
PTS:
1
DIF:
II
REF:
2
PTS:
1
DIF:
II
REF:
2
OBJ:
41. ANS:
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42. ANS:
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43. ANS:
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44. ANS:
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45. ANS:
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46. ANS:
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47. ANS:
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48. ANS:
OBJ:
49. ANS:
OBJ:
50. ANS:
OBJ:
2
D
2
A
2
B
2
C
2
C
3
D
3
A
3
D
3
B
3
C
4
PTS:
1
DIF:
II
REF:
2
PTS:
1
DIF:
II
REF:
2
PTS:
1
DIF:
II
REF:
2
PTS:
1
DIF:
II
REF:
2
PTS:
1
DIF:
II
REF:
2
PTS:
1
DIF:
II
REF:
2
PTS:
1
DIF:
II
REF:
2
PTS:
1
DIF:
II
REF:
2
PTS:
1
DIF:
II
REF:
2
PTS:
1
DIF:
II
REF:
2
DIF:
L3
REF:
p. 327
OBJ:
11.1.3 | 11.2.2
REF:
p. 327
OBJ:
11.1.3 | 11.2.2
OBJ:
11.1.3 | 11.2.2
PROBLEM
51. ANS:
2Al 3Cl
2AlCl
PTS: 1
STA: SC.HS.1.1.8
52. ANS:
CH
2O
CO
2H O
PTS: 1
DIF: L3
STA: SC.HS.1.1.8
53. ANS:
Fe (SO )
3Ba(OH)
2Fe(OH)
3BaSO
PTS: 1
DIF: L3
STA: SC.HS.1.1.8
54. ANS:
2C H
7O
6CO 8H O (incomplete)
REF:
p. 327
PTS: 1
DIF: L3
OBJ: 11.1.3 | 11.2.2
55. ANS:
2K PO
3BaCl
Ba (PO ) s
REF:
STA:
p. 327 | p. 336
SC.HS.1.1.8
6KCl
PTS: 1
DIF: L2
REF: p. 327
OBJ:
STA: SC.HS.1.1.8
56. ANS:
A first approach is to indicate the reactants and products in a word equation:
11.3.2
copper(II) oxide + sulfuric acid
copper(II) sulfate + water
Next, convert the word equation to a skeleton equation using chemical formulas:
CuO(s) + H SO (aq)
CuSO (aq) + H O(l)
Because the Cu
is exchanged in this reaction involving an aqueous solution, and the molecular compound H O is
formed, the reaction type is double-replacement. In this case, the skeleton equation already is balanced. Inspection of
substances on the left and right of the equation shows that the same relative amounts (number of atoms) of each element
are present in the reactants and the products.
PTS: 1
DIF: L3
REF: p. 334 | p. 335
OBJ: 11.1.3 | 11.2.1
STA: SC.HS.1.1.8
57. ANS:
Because the reaction is a double-replacement type, cations are exchanged among compounds during the reaction. The
first step is to write the equation in skeleton form:
AgNO + KCl
AgCl + KNO
Inspection of this equation shows that the insoluble precipitate silver chloride forms in an aqueous solution of potassium
nitrate. The relative amounts of elements are the same on either side of the equation, so the complete equation is:
AgNO (aq) + KCl(aq)
AgCl(s) + KNO (aq) (balanced)
PTS: 1
DIF: L3
REF: p. 334 | p. 335
OBJ: 11.3.2
STA: SC.HS.1.1.8
58. ANS:
According to Hund's rule, the arrangement of electrons with the maximum number of unpaired electrons is the most
stable arrangement.
PTS: 1
DIF: III
REF: 3
OBJ: 2
59. ANS:
According to the Pauli exclusion principle, no two electrons can have the same set of four quantum numbers. Therefore,
no more than two electrons can occupy an orbital, and these two must have opposite spins.
PTS: 1
DIF: III
REF: 3
OBJ: 2
60. ANS:
The 3 in 2p3 indicates that three electrons are in the p orbitals of the second energy level.
PTS: 1
DIF: II
REF: 3
OBJ: 3
61. ANS:
Atoms in a molecular compound share electrons to achieve stability. Atoms in an ionic compound gain or lose electrons
to form ions, which combine so that the number of positive and negative charges is equal.
PTS: 1
62. ANS:
DIF:
II
REF:
3
OBJ:
1
PTS: 1
63. ANS:
DIF:
III
REF:
3
OBJ:
3
PTS: 1
64. ANS:
DIF:
III
REF:
3
OBJ:
5
3
OBJ:
1
combustion, C3H8(g) + 5O2(g)
3CO2(g) + 4H2O(l)
PTS: 1
DIF: III
65. ANS:
reaction will occur, 2K(s) + ZnCl2(aq)
REF:
2KCl(aq) + Zn(s)
PTS: 1
DIF: III
REF: 3
OBJ: 2
66. ANS:
An atom with 34 protons has atomic number 34 and must therefore be an atom of selenium (Se). The uncharged atom
also has 34 electrons. The two extra electrons give the ion a 2– charge, so the symbol is Se2–.
PTS: 1
OBJ: 3C 3.g
67. ANS:
An atom with 19 protons has atomic number 19 and must therefore be an atom of potassium (K). The uncharged atom
also has 19 electrons. The deficit of one electron gives the ion a net charge of 1+, so the symbol is K +.
PTS: 1
OBJ: 3C 3.g
68. ANS:
52 = mass number = total number of protons and neutrons
24 = atomic number = number of protons
52 - 24 = 28 = number of neutrons
3+ = charge = number of protons - number of electrons
24 - x = 3+; x = number of electrons = 21
PTS: 1
OBJ: 3C 3.g
69. ANS:
The element must be tin (Sn, atomic number 50), given the number of electrons present and their distribution. There are
two unpaired electrons, in the 5p sublevel.
PTS: 1
OBJ: 4D 4.h
70. ANS:
1s22s22p63s23p64s23d104p65s24d105p66s24f145d106p67s1. There is one unpaired electron, at the 7s level.
PTS: 1
OBJ: 4D 4.h
71. ANS:
A nitrogen atom has five valence electrons. To have a complete octet of electrons, the nitrogen atom forms three
covalent bonds. It could form three single bonds, one single, and one double bond, or one triple bond.
PTS: 1
DIF: II
REF: 2
OBJ: 5
72. ANS:
The conditions under which the two reactions take place are different. In one case, solid magnesium is added to liquid
water, while in the other case, liquid magnesium reacts with gaseous water (perhaps steam). Although the products are
the same in each case, one might expect the second reaction to proceed more rapidly than the first because of the higher
temperature of the water (steam) and the breaking of the crystal lattice in magnesium.
PTS:
1
DIF:
II
REF:
1
OBJ:
3