Chemical Bonds_Summative
Matching
Match each item with the correct statement below.
a. halide ion
e. valence electron
b. octet rule
f. coordination number
c. ionic bond
g. metallic bond
d. electron dot structure
____
____
____
____
____
1.
2.
3.
4.
5.
an electron in the highest occupied energy level of an atom
Atoms react so as to acquire the stable electron structure of a noble gas.
a depiction of valence electrons around the symbol of an element
an anion of chlorine or other halogen
the force of attraction binding oppositely charged ions together
Match each item with the correct statement below.
a. coordinate covalent bond
d. single covalent bond
b. double covalent bond
e. polar bond
c. structural formula
f. hydrogen bond
____
____
6. a covalent bond in which only one pair of electrons is shared
7. a covalent bond in which two pairs of electrons are shared
Multiple Choice
Identify the letter of the choice that best completes the statement or answers the question.
____
____
____
____
____
____
____
8. How many valence electrons are in an atom of phosphorus?
a. 2
c. 4
b. 3
d. 5
9. How many valence electrons are in an atom of magnesium?
a. 2
c. 4
b. 3
d. 5
10. How many valence electrons does a helium atom have?
a. 2
c. 4
b. 3
d. 5
11. How many valence electrons are in a silicon atom?
a. 2
c. 6
b. 4
d. 8
12. What is the name given to the electrons in the highest occupied energy level of an atom?
a. orbital electrons
c. anions
b. valence electrons
d. cations
13. How does calcium obey the octet rule when reacting to form compounds?
a. It gains electrons.
b. It gives up electrons.
c. It does not change its number of electrons.
d. Calcium does not obey the octet rule.
14. What is the charge on the strontium ion?
____ 15.
____ 16.
____ 17.
____ 18.
____ 19.
____ 20.
____ 21.
____ 22.
____ 23.
a. 2–
c. 1
b. 1–
d. 2
How many electrons does barium have to give up to achieve a noble-gas electron configuration?
a. 1
c. 3
b. 2
d. 4
What is the formula of the ion formed when potassium achieves noble-gas electron configuration?
a. K
c. K
b. K
d. K
Which of the following elements does NOT form an ion with a charge of 1 ?
a. fluorine
c. potassium
b. hydrogen
d. sodium
How does oxygen obey the octet rule when reacting to form compounds?
a. It gains electrons.
b. It gives up electrons.
c. It does not change its number of electrons.
d. Oxygen does not obey the octet rule.
What is the charge on the cation in the ionic compound sodium sulfide?
a. 0
c. 2
b. 1
d. 3
Which of the following occurs in an ionic bond?
a. Oppositely charged ions attract.
b. Two atoms share two electrons.
c. Two atoms share more than two electrons.
d. Like-charged ions attract.
What is the net charge of the ionic compound calcium fluoride?
a. 2–
c. 0
b. 1–
d. 1
Which of the following is true about an ionic compound?
a. It is a salt.
c. It is composed of anions and cations.
b. It is held together by ionic bonds.
d. all of the above
What is the formula unit of sodium nitride?
a. NaN
c. Na N
b. Na N
d. NaN
____ 24. What is the formula unit of aluminum oxide?
a. AlO
b. Al O
c. AlO
d. Al O
____ 25. Ionic compounds are normally in which physical state at room temperature?
a. solid
c. gas
b. liquid
d. plasma
____ 26. Which of the following is NOT a characteristic of most ionic compounds?
a. They are solids.
b. They have low melting points.
c. When melted, they conduct an electric current.
d. They are composed of metallic and nonmetallic elements.
____ 27. Which of the following particles are free to drift in metals?
a. protons
c. neutrons
b. electrons
d. cations
____ 28. What characteristic of metals makes them good electrical conductors?
a. They have mobile valence electrons.
b. They have mobile protons.
c. They have mobile cations.
d. Their crystal structures can be rearranged easily.
____ 29. Which is a typical characteristic of an ionic compound?
a. Electron pairs are shared among atoms.
b. The ionic compound has a low solubility in water.
c. The ionic compound is described as a molecule.
d. The ionic compound has a high melting point.
____ 30. Which of these elements does not exist as a diatomic molecule?
a. Ne
c. H
b. F
d. I
____ 31. Why do atoms share electrons in covalent bonds?
a. to become ions and attract each other
b. to attain a noble-gas electron configuration
c. to become more polar
d. to increase their atomic numbers
____ 32. Which of the following elements can form diatomic molecules held together by triple covalent bonds?
a. carbon
c. fluorine
b. oxygen
d. nitrogen
____ 33. Which elements can form diatomic molecules joined by a single covalent bond?
a. hydrogen only
b. halogens only
c. halogens and members of the oxygen group only
d. hydrogen and the halogens only
____ 34. Which of the following diatomic molecules is joined by a double covalent bond?
a.
c.
b.
d.
____ 35. A molecule with a single covalent bond is ____.
a. CO
c. CO
b. Cl
d. N
____ 36. Which type of solid has the highest melting point?
a. ionic solid
c. metal
b. network solid
d. nonmetallic solid
____ 37. Which symbol is used to help with grouping the atoms of a polyatomic ion
a. a parenthesis
c. a multiplication symbol
b. an asterisk
d. a dot
____ 38. Which of the following usually makes a substance dissolve faster in a solvent?
a. agitating the solution
b. increasing the particle size of the solute
c. lowering the temperature
d. decreasing the number of particles
____ 39. Which of the following occurs as temperature increases?
a. Solubility decreases.
c. Solubility remains the same.
b. Solubility increases.
d. Molarity doubles.
Short Answer
40. Write the formula for the compound barium oxide.
41. Write the formula for the compound rubidium phosphide.
42. Write the electron configuration diagram that shows the transfer of electrons that takes place to form the
compound sodium fluoride. Include the electron configurations of the ions formed.
Essay
43. Explain what a pseudo-noble-gas electron configuration is. Give 3 examples of ions that have this type of
configuration.
44. Why is ice less dense than liquid water?
45. Discuss the different factors that can affect the solubility of a substance. Include specific examples in your
discussion.
Chemical Bonds_Summative
Answer Section
MATCHING
1. ANS:
STO:
2. ANS:
STO:
3. ANS:
STO:
4. ANS:
5. ANS:
STO:
E
Ch.2.a
B
Ch.2.a
D
Ch.2.e
A
C
Ch.2.a
DIF: L1
REF: p. 187
OBJ: 7.1.1
DIF: L1
REF: p. 188
OBJ: 7.1.2
DIF: L1
REF: p. 188
OBJ: 7.1.4
DIF: L1
DIF: L1
REF: p. 192
REF: p. 194
OBJ: 7.1.4
OBJ: 7.2.1
6. ANS:
STO:
7. ANS:
STO:
D
Ch.2.a
B
Ch.2.a
DIF: L1
REF: p. 217
OBJ: 8.2.1
DIF: L1
REF: p. 221
OBJ: 8.2.1
D
DIF: L1
Ch.1.c, Ch.2.a, Ch.1.d
A
DIF: L1
Ch.1.c, Ch.2.a, Ch.1.d
A
DIF: L1
Ch.1.c, Ch.2.a, Ch.1.d
B
DIF: L1
Ch.1.c, Ch.2.a, Ch.1.d
B
DIF: L1
Ch.1.c, Ch.2.a
B
DIF: L1
Ch.1.c, Ch.2.a
D
DIF: L1
Ch.1.c, Ch.2.g
B
DIF: L1
Ch.1.c, Ch.2.a, Ch.1.d
B
DIF: L1
Ch.3.a
A
DIF: L1
Ch.1.g
A
DIF: L1
Ch.1.g, Ch.2.a
B
DIF: L1
Ch.2.a
A
DIF: L1
REF: p. 187
OBJ: 7.1.1
REF: p. 188
OBJ: 7.1.1
REF: p. 188
OBJ: 7.1.1
REF: p. 188
OBJ: 7.1.1
REF: p. 187
OBJ: 7.1.1
REF: p. 188
OBJ: 7.1.1
REF: p. 190
OBJ: 7.1.2
REF: p. 190
OBJ: 7.1.3
REF: p. 190
OBJ: 7.1.3
REF: p. 190
OBJ: 7.1.3
REF: p. 191
OBJ: 7.1.4
REF: p. 194
OBJ: 7.2.1
REF: p. 194
OBJ: 7.2.1
MULTIPLE CHOICE
8. ANS:
STO:
9. ANS:
STO:
10. ANS:
STO:
11. ANS:
STO:
12. ANS:
STO:
13. ANS:
STO:
14. ANS:
STO:
15. ANS:
STO:
16. ANS:
STO:
17. ANS:
STO:
18. ANS:
STO:
19. ANS:
STO:
20. ANS:
STO:
21. ANS:
STO:
22. ANS:
STO:
23. ANS:
STO:
24. ANS:
STO:
25. ANS:
STO:
26. ANS:
OBJ:
27. ANS:
STO:
28. ANS:
STO:
29. ANS:
STO:
30. ANS:
STO:
31. ANS:
STO:
32. ANS:
STO:
33. ANS:
OBJ:
34. ANS:
STO:
35. ANS:
STO:
36. ANS:
STO:
37. ANS:
STO:
38. ANS:
OBJ:
39. ANS:
STO:
Ch.2.a
C
Ch.3.a
D
Ch.2.a
C
Ch.3.a
D
Ch.3.a
A
Ch.2.a
B
7.2.2
B
Ch.2.a
A
Ch.2.a
D
Ch.2.a
A
Ch.2.a
B
Ch.2.a
D
Ch.2.a
D
8.2.1
A
Ch.2.a
B
Ch.2.a
B
Ch.2.a
A
Ch.5.a
A
16.1.1
B
Ch.6.c
DIF: L1
REF: p. 194
OBJ: 7.2.1
DIF: L1
REF: p. 194
OBJ: 7.2.1
DIF: L2
REF: p. 195
OBJ: 7.2.1
DIF: L2
REF: p. 195
OBJ: 7.2.1
DIF: L1
REF: p. 196
OBJ: 7.2.2
DIF: L1
STO: Ch.2.a
DIF: L1
REF: p. 196, p. 198
REF: p. 201
OBJ: 7.3.1
DIF: L1
REF: p. 201
OBJ: 7.3.1
DIF: L2
REF: p. 244
OBJ: 8.1.1
DIF: L1
REF: p. 217
OBJ: 8.2.1
DIF: L2
REF: p. 217
OBJ: 8.2.1
DIF: L2
REF: p. 221
OBJ: 8.2.1
DIF: L3
STO: Ch.2.a
DIF: L2
REF: p. 217, p. 218
REF: p. 221
OBJ: 8.2.3
DIF: L2
REF: p. 222
OBJ: 8.2.1, 8.2.4
DIF: L1
REF: p. 243
OBJ: 8.4.4
DIF: L1
REF: p. 454
OBJ: 15.2.4
DIF: L2
STO: Ch.6.b
DIF: L2
REF: p. 471, p. 472
REF: p. 474
OBJ: 16.1.3
REF: p. 195
OBJ: 7.2.1
STO: Ch.3.a
SHORT ANSWER
40. ANS:
BaO
DIF: L2
41. ANS:
Rb P
DIF: L2
42. ANS:
Na(1s 2s 2p 3s )
DIF: L3
REF: p. 195
F(1s 2s 2p )
OBJ: 7.2.1
Na (1s 2s 2p )
REF: p. 195
OBJ: 7.2.1
STO: Ch.3.a
F (1s 2s 2p )
STO: Ch.1.g, Ch.3.a
ESSAY
43. ANS:
A pseudo-noble-gas configuration has the form s p d . It has 18 electrons in the outer energy level and is a
relatively stable configuration. Examples of ions with this configuration are Ag , Cu , Cd , and Hg .
DIF: L3
REF: p. 190
OBJ: 7.1.3
44. ANS:
The structure of ice is a regular, open framework in which water molecules are farther apart from each other
than they are in liquid water. When ice melts, this open framework collapses and the water molecules move
closer together. As a result, liquid water is denser than ice.
DIF: L2
REF: p. 449
OBJ: 15.1.2
STO: Ch.2.h
45. ANS:
The factors are temperature, pressure, and the nature of the solute and solvent. Specific examples include the
following. Potassium nitrate is more soluble in water at high temperature than at low temperature. Gases are
less soluble at high temperatures than at low temperatures. The solubility of a particular gas increases as the
partial pressure of that gas above the solution increases. Sodium nitrate is much more soluble in water than is
barium sulfate, regardless of temperature, because the attractive forces between the ions in BaSO are
stronger than the attractive force of the solvent molecules.
DIF: L3
STO: Ch.6.c
REF: p. 474, p. 475
OBJ: 16.1.3