Chemical Bonding Chapter 8 Exam Prep

Introduction to Chemistry, 5e (Bauer)

Chapter 8 Chemical Bonding

1) Which of the following compounds is likely to have covalent bonds?

A) NaCl

B) LiF

C) CO

D) CaBr2

E) MgO

2) Which of the following compounds is likely to have covalent bonds?

A) MgS

B) KF

C) SO2

D) SrCl2

E) RbF

3) Which of the following compounds is likely to have covalent bonds?

A) LiBr

B) CsF

C) BaCl2

D) Cr2O3

E) NO2

4) Which of the following compounds is likely to have covalent bonds?

A) CaBr2

B) OF2

C) NaF

D) BaBr2

E) LiCl

5) Which of the following substances has bonding best described as ionic bonding?

A) SiO2

B) TiO2

C) SO2

D) CO2

E) O2

6) Which of the following substances has both ionic and covalent bonding?

A) NaCl

B) Cl2

C) MgO

D) MgCO2

E) None of these

7) Which image(s) in the figure represents an ionic compound?

A) I only

B) II only

C) III only

D) IV only

E) I and IV

8) Which image(s) in the figure represents a compound that contains covalent bonds?

A) I only

B) II only

C) II and III

D) II, III, and V

E) V only

9) Which image(s) in the figure represents an ionic compound?

A) I only

B) II only

C) III only

D) IV only

E) I and IV

10) Which image(s) in the figure represents a compound with covalent bonds?

A) II only

B) III only

C) IV only

D) II and III

E) II, III, and V

11) Which of the following compounds is likely to occur as a gas at room temperature?

A) CaF2

B) CH4

C) MgO

D) FeCl3

E) LiF

12) Which of the following compounds is likely to occur as a gas at room temperature?

A) CaF2

B) MgS

C) NO2

D) NaF

E) CoCl2

13) Which of the following compounds is likely to occur as a solid at room temperature?

A) CH4

B) SO2

C) CaCl2

D) CO2

E) H2O

14) Which of the following compounds is likely to occur as a solid at room temperature?

A) PH3

B) NO3

C) MgCl2

D) SO2

E) ClO2

15) Which of the following compounds is likely to have a relatively high boiling point?

A) CoCl3

B) NH3

C) CO

D) NO2

E) CH4

16) Which of the following compounds is likely to have a relatively high boiling point?

A) PH3

B) FeCl3

C) NO

D) SO2

E) C2H6

17) Which of the following elements is the most electronegative?

A) carbon

B) silicon

C) nitrogen

D) oxygen

E) lithium

18) Which of the following elements is the most electronegative?

A) H

B) S

C) F

D) Cl

E) P

19) In which of the following bonds does nitrogen have a partial negative charge (δ–)?

A) N–C

B) N–O

C) N–F

D) N–N

E) None of these

20) In which of the following bonds does hydrogen have a partial negative charge (δ–)?

A) H–F

B) H–B

C) H–C

D) H–H

E) None of these

21) In which of the following molecules does oxygen have a partial positive charge (δ+)?

A) O2

B) OF2

C) H2O

D) MgO

E) None of these

22) Using periodic trends, arrange the following atoms in order of increasing electronegativity: Cl, Si, Ga, Sr

A) Cl < Si < Ga < Sr

B) Si < Ga < Sr < Cl

C) Si < Cl < Ga < Sr

D) Sr < Ga < Si < Cl

E) Sr > Ga < Cl < Si

23) Using periodic trends, arrange the following atoms in order of increasing electronegativity: F, O, S, As

A) F < O < S < As

B) As < O < S < F

C) As < S < O < F

D) S < As < O < F

E) S < As < F < O

24) Using periodic trends, arrange the following atoms in order of increasing electronegativity: Se, Cl, Mg, Na

A) Se < Cl < Mg < Na

B) Na < Mg < Cl < Se

C) Mg < Na < Se < Cl

D) Se < Mg < Na < Cl

E) Na < Mg < Se < Cl

25) Using periodic trends, arrange the following atoms in order of increasing electronegativity: S, Sr, P, Cs

A) S < Sr < P < Cs

B) S < P < Sr < Cs

C) P < Cs < Sr < S

D) Cs < Sr < S < P

E) Cs < Sr < P < S

26) Which of the following molecules contains the most polar bonds?

A) F2

B) OF2

C) NF3

D) BF3

E) CF4

27) Arrange the following bonds in order of increasing polarity: C-O, C-C, C-N, C-F

A) C-O < C-C < C-N < C-F

B) C-N < C-O < C-F < C-C

C) C-F < C-O < C-N < C-C

D) C-C < C-N < C-O < C-F

E) C-C < C-O < C-N < C-F

28) Arrange the following bonds in order of increasing polarity: F-F, F-C, F-O, F-N

A) F-F < F-C < F-O < F-N

B) F-F < F-O < F-N < F-C

C) F-O < F-N < F-F < F-C

D) F-N < F-O < F-F < F-C

E) F-N < F-C < F-O < F-F

29) Arrange the following bonds in order of increasing polarity: Cl-S, Cl-P, Cl-Si, Cl-Cl

A) Cl-S < Cl-P < Cl-Si < Cl-Cl

B) Cl-S < Cl-Si < Cl-P < Cl-Cl

C) Cl-Si < Cl-S < Cl-Cl < Cl-P

D) Cl-Cl < Cl-S < Cl-P < Cl-Si

E) Cl-Cl < Cl-P < Cl-Si < Cl-S

30) Arrange the following bonds in order of increasing polarity: O-H, C-H, F-H, H-H

A) O-H < C-H < F-H < H-H

B) C-H < O-H < F-H < H-H

C) H-H < C-H < O-H < F-H

D) C-H < H-H < O-H < F-H

E) H-H < C-H < F-H < O-H

31) Arrange the following bonds in order of increasing polarity: H-Cl, H-I, H-Br, H-F

A) H-Cl < H-I < H-Br < H-F

B) H-Cl < H-Br < H-I < H-F

C) H-F < H-Cl < H-Br < H-I

D) H-I < H-Br < H-Cl < H-F

E) H-I < H-Cl < H-Br < H-F

32) The Lewis symbol for F is:

A) A

B) B

C) C

D) D

E) E

33) The Lewis symbol for Mg is:

A) A

B) B

C) C

D) D

E) E

34) The Lewis symbol for S is:

A) A

B) B

C) C

D) D

E) E

35) The Lewis symbol for C is:

A) A

B) B

C) C

D) D

E) E

36) The Lewis symbol for N is:

A) A

B) B

C) C

D) D

E) E

37) The Lewis symbol for O2– is:

A) A

B) B

C) C

D) D

E) E

38) The Lewis symbol for P3– is:

A) A

B) B

C) C

D) D

E) E

39) The Lewis symbol for Ba2+ is:

A) A

B) B

C) C

D) D

E) E

40) The Lewis symbol for Al3+ is:

A) A

B) B

C) C

D) D

E) E

41) The formula for calcium sulfide is:

A) Ca2S

B) CaS2

C) CaS

D) Ca2S2

E) Ca2S3

42) The formula for aluminum chloride is:

A) AlCl

B) AlCl2

C) Al2Cl3

D) AlCl3

E) AlCl4

43) The formula for aluminum oxide is:

A) AlO

B) Al2O

C) AlO2

D) Al3O2

E) Al2O3

44) The formula for calcium nitride is:

A) CaN

B) Ca2N

C) CaN2

D) Ca3N2

E) Ca2N3

45) Which of the following statements regarding ionic compounds is incorrect?

A) Ions are held together in an ionic lattice by electrostatic attractions.

B) The crystal structure of a given compound will depend on the sizes and number of ions in a formula unit of the compound.

C) Ionic compounds tend to have low melting points.

D) Ionic compounds are formed when a metal and a nonmetal react.

E) In forming an ionic compound from its elements, one element transfers one or more electrons to another element.

46) Which of the following statements regarding ionic compounds is incorrect?

A) In many ionic compounds, a metal accepts electron(s) from a nonmetal.

B) Ionic compounds tend to have high melting points.

C) Electrostatic attractions hold the ions together in an ionic lattice.

D) Ionic compounds must be electrically neutral.

E) The formula of an ionic compound will have the simplest possible whole-number ratio of the ions to each other.

47) Which of the following statements regarding covalent bonding is incorrect?

A) In covalent bonding, electrons are shared between two atoms.

B) Most elements try to acquire an octet of electrons in their valence shell when bonding.

C) Hydrogen only requires two electrons in its valence shell when bonding.

D) Covalent bonds occur between a metal and a nonmetal.

E) It is possible for two atoms to share more than one pair of electrons.

48) Which of the following statements regarding covalent bonding is incorrect?

A) Hydrogen atoms in a Lewis structure will have eight electrons around the H symbol.

B) Covalent bonds occur between nonmetals.

C) Two atoms may share up to three pairs of electrons.

D) Carbon typically forms four bonds.

E) The elements which exist as diatomic molecules do so in order to achieve a stable electron configuration.

49) Which of the following best represents the bonding for NaBr?

A)

B) Na-Br

C) Na-Br:

D) :Na-Br:

E)

50) Which of the following best represents the bonding for MgCl2?

A) Cl-Mg-Cl

B)

C) Mg-Cl-Cl

D) :Cl-Mg-Cl:

E)

51) Which of the following best represents the bonding for CaO?

A) A

B) B

C) C

D) D

E) E

52) Which of the following best represents the bonding for K2O?

A) A

B) B

C) C

D) D

E) E

53) How many single bonds are typically formed by the element C?

A) 1

B) 2

C) 3

D) 4

E) The number of bonds varies.

54) How many single bonds are typically formed by the element N?

A) 1

B) 2

C) 3

D) 4

E) The number of bonds varies.

55) How many single bonds are typically formed by the element O?

A) 1

B) 2

C) 3

D) 4

E) The number of bonds varies.

56) Identify the main-group element X that could form the compound with the following Lewis structure:

A) C

B) O

C) N

D) F

E) P

57) Identify the main-group element X that could form the compound with the following Lewis structure:

A) C

B) O

C) N

D) F

E) P

58) Identify the main-group element X that could form the compound with the following Lewis structure:

A) P

B) B

C) C

D) F

E) S

59) An unknown molecular compound has the following Lewis structure. Which of the following elements could be the identity of X?

A) S

B) H

C) C

D) Cl

E) N

60) An unknown molecular compound has the following Lewis structure. Which of the following elements could be the identity of X?

A) Si

B) S

C) P

D) Cl

E) Ne

61) An unknown molecular compound has the following Lewis structure. Which of the following elements could be the identity of X?

A) C

B) N

C) O

D) Cl

E) Ne

62) The correctly drawn Lewis structure for CBr4 will have ________.

A) 4 single bonds

B) 5 single bonds

C) 4 single bonds and 1 pair of nonbonding electrons on the carbon atom

D) 4 single bonds and 2 pairs of nonbonding electrons on the carbon atom

E) 4 single bonds and 3 pairs of nonbonding electrons on the carbon atom

63) The correctly drawn Lewis structure for C2H2 will have ________.

A) 4 single bonds

B) 5 single bonds

C) 4 single bonds and 1 double bond

D) 4 single bonds and 1 triple bond

E) 5 double bonds

64) The correctly drawn Lewis structure for SiH4 will have ________.

A) 4 single bonds and 1 pair of nonbonding electrons on the Si atom

B) 4 double bonds to the Si atom

C) 2 single and 2 double bonds on the Si atom

D) 2 single bonds to Si and 2 single bonds to terminal H atoms

E) 4 single bonds to Si

65) The correctly drawn Lewis structure for NH2OH will have ________.

A) 3 single bonds and 3 pairs of nonbonding electrons

B) 4 single bonds and 3 pairs of nonbonding electrons

C) 3 single bonds, 1 double bond, and 2 pairs of nonbonding electrons

D) 2 single bonds, 2 double bonds, and 2 pairs of nonbonding electrons

E) 4 single bonds and 2 pairs of nonbonding electrons

66) The correctly drawn Lewis structure for HCN will have ________.

A) 2 single bonds and 5 pairs of nonbonding electrons

B) 1 single bond, 1 double bond, and 3 pairs of nonbonding electrons

C) 2 double bonds and 2 pairs of nonbonding electrons

D) 1 single bond, 1 triple bond, and 1 pair of nonbonding electrons

E) 2 double bonds and 1 pair of nonbonding electrons

67) Which of the following contains a triple bond?

A) H2

B) N2

C) O2

D) F2

E) Cl2

68) Which of the following contains a double bond?

A) CH4

B) C2H6

C) C2H4

D) C2H2

E) H2

69) Which of the following contains a triple bond?

A) C2H6

B) HCN

C) NO3−

D) NH3

E) O3

70) Draw the Lewis structure for the NO2– ion. What is the total number of electrons shared between nitrogen and the two oxygen atoms?

A) 2

B) 3

C) 5

D) 6

E) 8

71) Which of the following molecules should exhibit resonance?

A) H2O

B) N2

C) O3

D) CO2

E) CCl4

72) Which of the following molecules should exhibit resonance?

A) H2S

B) Cl2 

C) SO2

D) O2

E) CH4

73) Which of the following molecules or ions should exhibit resonance?

A) C2H2

B) Br2

C) CO32−

D) CO

E) SiH4

74) How many equivalent resonance structures best represent(s) the NO2– ion?

A) 1

B) 2

C) 3

D) 4

E) It does not exhibit resonance.

75) Which of the following is best represented by two equivalent resonance structures?

A) O3

B) CO2

C) NO3–

D) N2

E) none of these

76) Which of these molecules or ions has a violation of the octet rule (other than H)?

A) CO2

B) H2S

C) SF4

D) CH4

E) PCl3

77) Which of these molecules or ions has a violation of the octet rule (other than H)?

A) CO

B) H2O

C) PCl5

D) Br2

E) NH3

78) Which of these molecules or ions has a violation of the octet rule (other than H)?

A) BH3

B) F2

C) PH3

D) NO3−

E) SF2

79) Which of these molecules or ions has a violation of the octet rule (other than H)?

A) C2H2

B) NH4+

C) SO2

D) BeF2

E) I2

80) In which of the following does the central atom NOT obey the octet rule?

A) BH3

B) NH3

C) PH3

D) H2S

E) All of these obey the octet rule.

81) Identify the class of organic substance for the molecule CH3CH2OH.

A) alkane

B) alkene

C) alcohol

D) amine

E) ester

82) Identify the class of organic substance for the molecule CH3CH-NH2.

A) alkane

B) alkene 

C) alcohol

D) amine

E) ester

83) Identify the class of organic substance for the molecule CH3CH=CH2.

A) alkane

B) alkene

C) alcohol

D) amine

E) ester

84) Identify the class of organic substance for the molecule H3C-CH3.

A) alkane

B) alkene

C) alcohol

D) amine

E) ester

85) Which of the following statements regarding VSEPR theory is correct?

A) The name of the molecular shape which has three atoms and one unshared pair of electrons on the central atom is trigonal planar.

B) Nonbonding electron pairs have no influence on molecular shape.

C) It is not necessary to draw the Lewis structure of a molecule before predicting its shape.

D) VSEPR theory can be used to predict the shape of a molecule.

E) The molecular shape called "bent" always has only one pair of unshared electrons on the central atom.

86) Which of the following statements regarding VSEPR theory is correct?

A) When counting the number of electron groups on the central atom, a double bond counts as two groups.

B) The trigonal pyramidal shape has three atoms and one unshared pair of electrons on the central atom.

C) The unshared pairs of electrons are unimportant in both the Lewis structure and in VSEPR theory.

D) A trigonal planar molecular shape has four atoms attached to the central atom.

E) It is not necessary to draw a correct Lewis structure for a given molecule before using VSEPR to predict the shape of that molecule.

87) Which of the following has a parent structure that is tetrahedral?

A) H2S

B) SiCl4

C) NF3

D) SO42–

E) all of these

88) Which of the following has a parent structure that is trigonal planar?

A) NH3

B) H2O

C) SO2

D) CO2

E) all of these

89) Predict the molecular shape and give the approximate bond angles in the PCl3 molecule.

A) linear, 180º

B) trigonal planar, 120º

C) tetrahedral, 109.5º

D) trigonal pyramidal, 109.5º

E) bent, 120º

90) Predict the molecular shape and give the approximate bond angle in the SO2 molecule.

A) linear, 180°

B) trigonal planar, 120°

C) tetrahedral, 109.5°

D) trigonal pyramidal, 109.5°

E) bent, 120°

91) Predict the molecular shape and give the approximate bond angle in the CO2 molecule.

A) linear, 180°

B) trigonal planar, 120°

C) tetrahedral, 109.5°

D) trigonal pyramidal, 109.5°

E) bent, 120°

92) Predict the molecular shape and give the approximate bond angles in the SiH4 molecule.

A) linear, 180°

B) trigonal planar, 120°

C) tetrahedral, 109.5°

D) trigonal pyramidal, 109.5°

E) bent, 120°

93) Predict the molecular shape and give the approximate bond angles in the SO3 molecule.

A) linear, 180°

B) trigonal planar, 120°

C) tetrahedral, 109.5°

D) trigonal pyramidal, 109.5°

E) bent, 120°

94) Predict the molecular shape and give the approximate bond angles in the SO32– polyatomic ion.

A) linear, 180°

B) trigonal planar, 120°

C) tetrahedral, 109.5°

D) trigonal pyramidal, 109.5°

E) bent, 120°

95) Predict the molecular shape and give the approximate bond angles in the CO32– polyatomic ion.

A) linear, 180°

B) trigonal planar, 120°

C) tetrahedral, 109.5°

D) trigonal pyramidal, 109.5°

E) bent, 120°

96) Predict the molecular shape and give the approximate bond angle in the OF2 molecule.

A) linear, 180°

B) trigonal planar, 120°

C) tetrahedral, 109.5°

D) trigonal pyramidal, 109.5°

E) bent, 109.5°

97) Which of the following has bond angles closest to 120°?

A) CO2

B) H2O

C) O3

D) CH4

E) NH3

98) Which of the molecules in the figure are polar? (Assume that the bonds are all polar.)

A) I, II, and III

B) I, II, III, and IV

C) II, III, and IV

D) I, II, and IV

E) I, III, and IV

99) Which of the molecules in the figure are polar? (Assume that the bonds are all polar.)

A) I, II, and III

B) I and II

C) I, III, and IV

D) II only

E) II and IV

100) Which of the molecules in the figure has unshared electron pairs on the central atom?

A) I, II, and III

B) I and II

C) I, III, and IV

D) II only

E) not enough information

101) Which of the molecules in the figure has unshared electron pairs on the central atom?

A) II and III

B) I and III

C) I, II, and III

D) I, II, III, and IV

E) not enough information

102) Which of the following molecules is polar?

A) CCl4

B) H2S

C) SO3

D) CO2

E) BeF2

103) Which of the following molecules is polar?

A) BCl3

B) NH3

C) SiCl4

D) CBr4

E) BeBr2

104) Which of the following molecules is polar?

A) BF3

B) CH4

C) CS2

D) PCl3

E) BeCl2

105) Which of the following molecules is a nonpolar molecule with polar bonds?

A) NF3

B) CH2Cl2

C) CF4

D) O3

E) CO

106) The K2+ ion forms commonly because it is isoelectronic with chlorine.

107) When there are extra electrons available in a Lewis structure, they are used to make double or triple bonds in the molecule.

108) Resonance is a representation of how electrons shift rapidly from one atom to another in a molecule or ion.

109) If a molecule has polar bonds, the overall molecule must be polar.

110) Electronegativity is a measure of the amount of energy needed to remove an electron from an atom.

111) Electron pairs on molecules maximize the distance between themselves in order to minimize repulsions.

112) Molecular compounds are more likely to be gases at room temperature than ionic compounds.

113) Metallic elements are more electronegative than nonmetallic elements.

114) Diatomic elements such as F2 and Cl2 are polar because these elements are very electronegative.

115) A trigonal planar molecule will have an unshared pair of electrons on the central atom.

116) Draw a Lewis structure for CCl4. How many unshared pairs of electrons are on the carbon atom? On each chlorine atom?

117) Draw a Lewis structure for H2S. How many unshared pairs of electrons are on the sulfur atom?

118) Draw a Lewis structure for PH3. How many unshared pairs of electrons are on the phosphorus atom? Does this molecule have any resonance forms?

119) Draw a Lewis structure for SO2. How many unshared pairs of electrons are on the sulfur atom? How many resonance forms does this molecule have?

120) Consider the following Lewis structure for CO32–. How many resonance forms does this ion have?

121) Consider the following Lewis structure for NO3–. How many resonance forms does this ion have?

122) One of these molecules is SF2, and one is BeF2. Is A correctly labeled BeF2? Is SF2 polar? Is BeF2 polar?

123) Is CO2 an example of a nonpolar molecule that has polar bonds?

124) What is the shape of PCl3? Is this molecule polar or nonpolar?