Introductory Chemistry: Atoms First, 5e (Russo/Silver)
Chapter 5 Chemical Bonding and Nomenclature
5.1 Multiple-Choice Questions
1) Which of the following statements best describes an ionic bond?
A) a strong lattice of positively and negatively charged atoms held together by electrical forces
B) the bonding type present in bound, non-metal atoms
C) the equal sharing of two electrons between adjacent atoms
D) the bonding type present between two metal atoms
2) Which of the following is considered an elemental substance?
A) I2 (iodine)
B) H2O (water)
C) Fe (an iron nail)
D) A and C are elemental substances.
E) All of the preceding are elemental substances.
3) Which of the following substances is molecular (composed of individual molecules) in
composition?
A) carbon in coal
B) drinking water
C) a copper ingot
D) helium in a balloon
4) Which phrase best describes a covalent bond between two atoms?
A) a stable arrangement of charged atoms held together by electrostatic forces
B) a stable arrangement of atoms made by sharing two electrons between adjacent atoms
C) uncommon, as electrons are free to jump from one atom to another
D) an exchange of nuclei between two atoms
5) Which of the following exists as a diatomic molecule?
A) neon
B) oxygen
C) phosphorus
D) silicon
6) Which of the following may not exist as a diatomic molecule?
A) oxygen
B) nitrogen
C) argon
D) hydrogen
7) The number of valence electrons in silicon is ________.
A) 2
B) 4
C) 6
D) 8
8) The number of valence electrons in sulfur is ________.
A) 2
B) 4
C) 6
D) 8
9) The number of valence electrons in magnesium is ________.
A) 2
B) 4
C) 6
D) 8
10) The number of valence electrons in aluminum is ________.
A) 2
B) 3
C) 5
D) 7
11) The number of valence electrons in neon is ________.
A) 2
B) 4
C) 6
D) 8
12) The number of valence electrons in nitrogen is ________.
A) 2
B) 3
C) 5
D) 6
13) Which of the following elements has the highest number of valence electrons?
A) magnesium
B) lithium
C) argon
D) phosphorus
14) How many covalent bonds can an element of Group VA form with other elements?
A) 4
B) 3
C) 2
D) 1
15) How many valence electrons does a single, neutral iodine atom have?
A) 3
B) 4
C) 5
D) 7
16) How many covalent bonds can a single oxygen atom form with other elements?
A) 3
B) 4
C) 2
D) 1
17) Every single COVALENT bond represents ________ electrons.
A) one
B) two
C) four
D) One cannot say unless the atoms that make up the bond are known.
18) Which of the following represents the correct Lewis dot structure for selenium (Se)?
A)
B)
C)
D)
19) Which of the following elements has the lowest number of valence electrons?
A) magnesium
B) lithium
C) argon
D) phosphorus
20) To follow the octet rule, how many electrons must a neutral sulfur atom gain when forming a
negative ion?
A) 1
B) 2
C) 6
D) 8
21) How many unpaired electrons does the oxide anion (O2-) have?
A) 3
B) 2
C) 1
D) 0
22) How many valence electrons are needed to construct the Lewis dot structure of the BCl3
molecule?
A) 11
B) 21
C) 24
D) 32
23) What is the most likely formula of the neutral, ionic compound formed by magnesium and
oxygen?
A) Mg2O
B) MgO2
C) Mg3O2
D) MgO
24) What is the most likely formula of the neutral, ionic compound formed by lithium and
nitrogen?
A) Li2N
B) Li3N
C) LiN
D) LiN2
25) Which of the following does not have the same number of valence electrons as the other
three elements?
A) nitrogen
B) phosphorus
C) beryllium
D) arsenic
26) Which of the following has the same number of valence electrons as sulfur?
A) nitrogen
B) oxygen
C) arsenic
D) boron
27) Which of the following elements has the least number of valence electrons?
A) krypton
B) potassium
C) calcium
D) aluminum
28) Which of the following pairs has the same number valence electrons?
A) magnesium and potassium
B) lithium and calcium
C) argon and xenon
D) phosphorus and tellurium
29) The expected binary compound between magnesium and bromine is ________.
A) MgBr
B) MgBr2
C) Mg2Br
D) Mg2Br2
30) The expected formula between aluminum and oxygen is ________.
A) AlO
B) AlO2
C) Al2O
D) Al2O3
31) The expected formula between silicon and fluorine is ________.
A) SiF
B) SiF2
C) SiF4
D) SiF6
32) The expected formula between sodium and oxygen is ________.
A) NaO
B) Na2O2
C) Na2O
D) Na2O3
33) The expected formula between calcium and oxygen is ________.
A) CaO
B) CaO2
C) Ca2O
D) Ca2O5
34) The expected formula between calcium and iodine is ________.
A) CaI
B) Cal2
C) Ca2I
D) Ca2I3
35) The expected formula between magnesium and sulfur is ________.
A) MgS
B) MgS2
C) Mg2S
D) Mg2S3
36) The expected formula between potassium and sulfur is ________.
A) KS
B) K2S3
C) K2S
D) KS2
37) The expected formula between hydrogen and nitrogen is ________.
A) HN
B) NH2
C) NH3
D) NH4
38) What is the number of single bonds in C2H6O?
A) 5
B) 6
C) 7
D) 8
39) Water has ________ covalent bonds and ________ lone pairs.
A) 2; 2
B) 2; 4
C) 2; 0
D) 2; 6
40) Methane has ________ covalent bonds and ________ lone pairs.
A) 4; 2
B) 4; 1
C) 4; 0
D) 2; 4
41) Phosphine, PH3, has ________ covalent pairs and ________ lone pairs.
A) 3; 0
B) 3; 1
C) 3; 2
D) 2; 0
42) Hydrazine, N2H4, has ________ covalent bonds and ________ lone pairs.
A) 2; 2
B) 4; 2
C) 3; 4
D) 5; 2
43) Hydrazine has ________ valence electrons.
A) 14
B) 12
C) 10
D) 8
44) Nitrogen trifluoride has ________ valence electrons.
A) 20
B) 22
C) 24
D) 26
45) Nitrogen trifluoride has ________ valence electrons that are contributed by the nitrogen
atom.
A) 5
B) 8
C) 10
D) 12
46) Nitrogen trifluoride has ________ bonds, ________ of which are single bonds.
A) 3; 3
B) 5; 1
C) 7; 2
D) 8; 3
47) Nitrogen trifluoride has ________ lone pairs of electrons.
A) 2
B) 5
C) 8
D) 10
48) Carbon tetrafluoride has ________ total valence electrons.
A) 24
B) 28
C) 32
D) 36
49) Which of the following has at least one double bond?
A) hydrogen
B) carbon dioxide
C) chlorine
D) nitrogen
50) How many resonance structure could be drawn for the nitrate ion?
A) 0
B) 1
C) 2
D) 3
51) Acetylene, C2H2, has ________.
A) two single bonds
B) two double bonds
C) one triple bond
D) both A and C
52) The number of valence electrons in the carbonate anion is ________.
A) 20
B) 22
C) 24
D) 26
53) The number of valence electrons that belong to the oxygens in the carbonate anion is
________.
A) 15
B) 18
C) 20
D) 24
54) The number of valence electrons in the nitrate anion is ________.
A) 23
B) 24
C) 28
D) 30
55) The phosphate anion has ________ valence electrons.
A) 29
B) 30
C) 32
D) 36
56) Each atom in the oxygen molecule contributes ________ valence electrons for a total of
________ electrons
A) 6; 12
B) 6; 8
C) 8; 6
D) 12; 6
57) Which of the following has a triple bond?
A) water
B) carbon dioxide
C) oxygen
D) nitrogen
58) Which of the following has more than one double bond?
A) carbon monoxide
B) carbon dioxide
C) oxygen
D) nitrogen
59) Which of the following gases does not have a triple bond?
A) hydrogen cyanide
B) acetylene, C2H2
C) carbon dioxide
D) nitrogen
60) Which of the following does not have at least one multiple covalent bond?
A) carbon dioxide
B) ethene, C2H4
C) hydrogen cyanide
D) ethane, C2H6
61) Which of the following is the molecular formula for ozone?
A) O3
B) O3–
C) O3-2
D) O2-2
62) The numerical rating of an atom’s ability to attract the shared electrons is called ________.
A) electronegativity
B) ionization
C) covalency
D) redistribution
63) Which of the following bonds will have the smallest difference in electronegativity?
A) HBr
B) NaF
C) H2
D) HS–
64) Which of the following bonds will have the largest difference in electronegativity?
A) HBr
B) NaF
C) H2
D) HS–
65) If the electrons are shared equally between the two atoms, the bond is called ________.
A) ionic
B) non-polar covalent
C) hydrogen bonding
D) polar covalent
66) In a(n) ________ bond, the electrons are transferred.
A) ionic
B) covalent
C) hydrogen bonding
D) polar covalent
67) In a(n) ________ bond, the electrons are shared unequally.
A) ionic
B) non-polar covalent
C) hydrogen bonding
D) polar covalent
68) Identify the most polar covalent bond.
A) C-C
B) C-H
C) C-F
D) C-Cl
69) Identify the least polar covalent bond.
A) C-C
B) C-H
C) C-F
D) C-Cl
70) Identify the ionic bond.
A) C-S
B) Na-F
C) N-O
D) F-F
71) Which of the following phrases best describes the H-O bonds present in water (H2O)?
A) nonpolar and ionic
B) nonpolar and covalent
C) polar and ionic
D) polar and covalent
72) Which of the following compounds has a covalent bond?
A) NaCl
B) KBr
C) LiH
D) H2
73) Identify the most electronegative element.
A) fluorine
B) oxygen
C) carbon
D) sodium
74) Identify the least electronegative element.
A) fluorine
B) oxygen
C) carbon
D) sodium
75) The central atom in sulfuric acid is ________.
A) oxygen
B) sulfur
C) hydrogen
D) none of the above
76) Consider a bond A-B. If the difference in electronegativity is 1.0, the bond is considered
________.
A) ionic
B) covalent
C) polar covalent
D) hydrogen
77) Consider a bond A-B. If the difference in electronegativity is 3.5, the bond is considered
________.
A) ionic
B) covalent
C) polar covalent
D) hydrogen
78) Consider a bond A-B. If the difference in electronegativity is 0.0, the bond is considered
________.
A) ionic
B) covalent
C) polar covalent
D) hydrogen
79) What is the chemical name of the compound whose formula is K2O?
A) dipotassium oxygen
B) potassium oxide
C) potasside oxygen
D) potassium oxygen
80) What is the chemical formula of calcium phosphate?
A) CaPO4
B) Ca2PO4
C) Ca3PO4
D) Ca3(PO4)2