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Pearson Chemistry Chapter 8 Test Review Flashcards | StudBud
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Pearson Chemistry Chapter 8 Test Review
Pearson Chemistry Chapter 8 Test Review
98 terms
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A combination of my questions and the Quiz! by HockeyNutZ
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Questions
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Answers
1
Which of the following molecules contains an odd number of valence electrons?
CO2
NH4
O2
NO
2
Which of the following electronegativity differences corresponds to a polar covalent bond?
0
2.5
0.4
1.2
3
A dipole is formed when a bond has:
Unequal electron sharing
No electronegativity difference
Equal electron sharing
A large difference in atomic size
4
What does the concept of resonance describe?
The vibration of molecules
The polarity of a bond
The movement of atoms within a molecule
The delocalization of electrons within a molecule
5
Which contains a coordinate covalent bond?
O2
[NH4]+
CH4
H2
6
What type of intermolecular force occurs between two nonpolar molecules?
Ion-Dipole interactions
Dipole-Dipole interactions
Hydrogen bonding
London Dispersion Forces (LDFs)
7
Which of the following exists as a diatomic molecule?
Na
Ar
He
Cl
8
How many single covalent bonds are there in a molecule of CH
4
?
1
3
4
2
9
Which of the following compounds contains both single and double covalent bonds?
CO2
H2O
C2H4
HCN
10
Two or more valid electron dot formulas that can be written for the same molecule or ion
cooridnate covalent bond
hybridization
resonance structures
structural formula
11
Which molecule contains a carbon-carbon double bond with both a sigma and a two pi bonds?
Ethene (C2H4)
Oxygen (O2)
Ethyne (C2H2)
Methane (CH4)
12
In a fluorine molecule (F
2
), what type of bond is formed by the overlap of 2p orbitals?
Sigma bond
Metallic bond
Ionic bond
Pi bond
13
The triple bond in nitrogen gas (N
2
) contributes to which of the following properties?
High reactivity
Low boiling point
High bond strength
Weak intermolecular forces
14
What type of bond is formed between magnesium (1.2) and oxygen (3.4)?
Metallic
Nonpolar covalent
Ionic
Polar covalent
15
How many hybrid orbitals are formed when one s orbital and three p orbitals mix?
2
3
5
4
16
Why are pi bonds generally weaker than sigma bonds?
Pi bonds are located on the bond axis.
Pi bonds do not involve p orbitals.
Pi bonds involve a smaller region of overlap.
Sigma bonds cannot occur in the same molecule.
17
How many sigma and pi bonds are present in a double bond?
One sigma, two pi
One sigma, one pi
Two sigma, two pi
Two sigma, one pi
18
The actual structure of a resonance-stabilized molecule is:
A hybrid of all possible resonance structures
The structure with the least number of bonds
The most electronegative structure
A single Lewis structure
19
What happens in a pi bond?
Atomic orbitals do not overlap.
Orbitals overlap end to end.
Orbitals overlap side by side.
Electrons move freely without bonding.
20
Which property is generally true as the number of bonds between two atoms increases?
Bond strength increases, and bond length decreases
Both bond strength and bond length increase
Both bond strength and bond length decrease
Bond strength decreases, and bond length increases
21
Bond dissociation energy is defined as:
The energy required to form a single bond
The energy required to break all bonds in a molecule
The energy released when a bond forms
The energy required to break one mole of bonds in a molecule
22
What is a key characteristic of a nonpolar covalent bond?
Unequal sharing of electrons
Transfer of electrons
Equal sharing of electrons
Formation of ions
23
What determines the polarity of a molecule?
The total number of valence electrons
Bond polarity and molecular shape
The number of atoms in the molecule
The difference in atomic mass between atoms
24
The weakest attractions that exist between molecules
structural formula
Von der Waals forces
cooridnate covalent bond
hybridization
25
What is a coordinate covalent bond?
A bond where electrons are transferred from one atom to another
A bond formed by overlapping of atomic orbitals
A bond where both electrons in the shared pair come from the same atom
A bond that involves a triple bond structure
26
Why does diamond have an extremely high melting point?
It has a high atomic mass
It has strong hydrogen bonds
It consists of covalently bonded atoms in a network solid
It contains metal atoms
27
Which diatomic molecule contains a triple covalent bond?
H2
O2
Cl2
N2
28
In a triple covalent bond, how many electrons are shared between two atoms?
6
8
4
2
29
Which factor affects molecular polarity?
The number of protons in each atom
The size of the atom
The number of neutrons in the nucleus
Bond polarity and molecular shape
30
What is the bond angle in an sp
3
hybridized molecule?
90
120
180
109.5
31
How many sigma and pi bonds are present in a triple bond?
One sigma, two pi
One sigma, one pi
Two sigma, one pi
Two sigma, two pi
32
A covalent bond formed between two different atoms in which the bonding electrons are shared
polar molecule
VSEPR theory
single covalent bond
polar covalent bond
33
In the N
2
molecule, what is the
total
number of unshared
pairs
of electrons?
3
4
1
2
34
What is the term for a group of atoms joined by covalent bonds that act as a single unit?
Ionic lattice
Polyatomic ion
Ion
Molecule
35
Which of the following correctly ranks the intermolecular forces from weakest to strongest?
London Dispersion Forces
Hydrogen Bonding
Dipole-Dipole
Ion-Dipole
36
Which type of hybridization occurs in ethene (C
2
H
4
)?
sp2
sp2d
sp
sp3
37
What type of bond is formed between hydrogen (2.2) and oxygen (3.4)?
Ionic
Polar covalent
Nonpolar covalent
Metallic
38
A covalent bond in which one pair of electrons is shared between two atoms
polar molecule
polar covalent bond
VSEPR theory
single covalent bond
39
Which of the following represents a single covalent bond?
CO2
O2
Cl2
N2
40
What is the hybridization of carbon in methane (CH
4
)?
sp³d
sp³
sp²
sp
41
Which of the following compounds contains polar covalent bonds?
NH3
O2
CH4
H2
42
How many double covalent bonds are there in a molecule of CO
2
?
1
2
3
4
43
Which of the following molecules can form hydrogen bonds?
CH4
CO2
HCl
NH3
44
Which type of orbital overlap leads to a sigma (σ) bond?
End-to-end overlap of atomic orbitals
Overlap of d orbitals
Side-by-side overlap of p orbitals
None of the above
45
What is a covalent bond?
A bond formed by the attraction between ions
A bond formed between a metal and a nonmetal
A bond formed by the transfer of electrons
A bond formed by the sharing of electrons
46
What is the name of the rule that states atoms tend to share electrons to acquire a full set of eight valence electrons?
Valence rule
Electron sharing rule
Ionic rule
Octet rule
47
A covalent bond in which one atom contributes both bonding electrons
molecular compound
polar covalent bond
single covalent bond
coordinate covalent bond
48
Which statement about molecular orbitals is correct?
Sigma bonds are stronger than pi bonds.
Pi bonds allow free rotation around the bond axis.
Sigma bonds result from side-by-side orbital overlap.
Molecular orbitals are localized to a single atom.
49
Which molecule is likely to be polar?
H2O
CH4
Cl2
CO2
50
Why are diatomic hydrogen molecules (H
2
) stable?
The attractions between nuclei and electrons overcome repulsions.
The nuclei repel each other strongly.
The attraction between nuclei and electrons is weaker than repulsions.
The electrons in each atom avoid bonding.
51
A molecule is automatically polar if it contains:
Equal electronegativity in all atoms
A symmetrical shape
Only nonpolar bonds
Lone pairs (of electrons) on the central atom
52
What is a sigma bond?
A bond formed by side-to-side overlap of atomic orbitals
A bond formed by end-to-end overlap of atomic orbitals
A bond weaker than a pi bond
A bond without electron sharing
53
Which is a covalent molecule?
KF
CaO
NH3
NaCl
54
Which molecule contains a triple covalent bond?
CO2
N2
O2
H2
55
Which molecular shape is predicted for water (H
2
O) based on VSEPR theory?
Trigonal planar
Tetrahedral
Bent
Linear
56
Which of the following molecules exhibits resonance?
HCl
CH4
O3
NH3
57
What is a characteristic of a pi bond?
Overlap occurs along the bond axis
Overlap occurs above and below the bond axis
Stronger than a sigma bond
No overlap occurs between orbitals
58
How many covalent bonds does carbon typically form?
3
1
2
4
59
Which molecule has the weakest intermolecular forces?
HF
CH4
H2O
NH3
60
Which of the following molecules is likely to be nonpolar?
NH3
CHCl2
CO2
H2O
61
The mixing of several atomic orbitals to form the same number of equivalent hybrid orbitals
resonance structures
hybridization
structural formula
cooridnate covalent bond
62
An electrically neutral group of atoms joined together by covalent bonds
single covalent bond
polar covalent bond
molecular compound
polar molecule
63
What is the molecular geometry of carbon dioxide (CO
2
)?
Tetrahedral
Bent
Trigonal planar
Linear
64
In Cl
2,
what is the
total
number of unshared
pairs
of electrons?
6
2
4
1
65
What does VSEPR theory state about molecular shapes?
Electrons are evenly distributed.
Electron pairs repel each other to maximize separation.
Atomic orbitals overlap to form molecular orbitals.
Only bonding pairs influence molecular geometry.
66
Which intermolecular force is the strongest?
Hydrogen bonding
London Dispersion Forces (LDFs)
Ion-Dipole interactions
Dipole-Dipole interactions
67
Which of the following molecules has sp
3
hybridization?
CH4
BF3
CO2
C2H4
68
What type of bond is formed between boron (2.0) and phosphorus (2.2)?
Nonpolar covalent
Ionic
Metallic
Polar covalent
69
How many shared electron pairs are there in a double covalent bond?
4
3
2
1
70
What determines whether a covalent bond is polar or nonpolar?
The size of the atoms
The atomic mass of the elements
The electronegativity difference between atoms
The number of valence electrons
71
What type of bond is formed when two atomic orbitals combine symmetrically around the axis connecting two nuclei?
Sigma bond
Covalent bond
Pi bond
Ionic bond
72
What type of molecular orbital is formed when atomic p orbitals overlap end to end?
Pi bond
Sigma bond
Bonding orbital
Hybrid orbital
73
What is the bond angle between the sp
2
hybrid orbitals in ethene (C
2
H
4
)?
109.5
90
180
120
74
What is the primary difference between single, double, and triple covalent bonds?
The number of electron pairs shared between atoms
The number of atoms involved in bonding
The size of the atoms
The types of atoms that form the bond
75
The molecule among the following that contains only one single covalent bond is
H2O
NH3
HI
N2
76
What is the bond angle in a methane (CH
4
) molecule?
105
109.5
90
107
77
Molecules adjust their shapes so that their electron clouds are as far apart as possible
single covalent bond
polar molecule
polar covalent bond
VSEPR theory
78
Which intermolecular force occurs between water molecules?
Ionic bonding
London Dispersion Forces (LDFs)
Hydrogen bonding
Metallic bonding
79
What is a molecular orbital?
An orbital belonging to a single atom
An orbital that applies to an entire molecule
An orbital with no electrons
An orbital shared by two atoms only
80
A molecule in which one end is slightly negative and the other end is slightly positive
polar molecule
single covalent bond
VSEPR theory
polar covalent bond
81
What type of bond is present in ethene (C
2
H
4
)?
A combination of single and double covalent bonds
A combination of double and triple covalent bonds
Only double covalent bonds
Only single covalent bonds
82
The diatomic molecule among the following that contains a single covalent bond is
O2
N2
F2
O2-
83
How many pi bonds are present in a triple bond?
Three
Two
None
One
84
Atoms share electrons in order to acquire the electron configuration of
alkaline earth metals
alkali metals
noble gases
halogens
85
What is the hybridization of the central carbon atom in ethyne (C
2
H
2
)?
sp3
sp2
sp
sp4
86
Name an element from the Periodic Table.
All of these
Oxygen
Hydrogen
Nitrogen
87
What type of bond results from the side-by-side overlap of p orbitals?
Pi bond
Sigma bond
Ionic bond
Metallic bond
88
Which bond would require the most energy to break?
H–H
N≡N
O=O
F–F
89
Why does water have a higher boiling point than expected?
It has hydrogen bonding
It has Dipole-Dipole interactions
It has weak intermolecular forces
It has strong London Dispersion Forces
90
A chemical formula that shows the arrangement of atoms in molecules and polyatomic ions
cooridnate covalent bond
resonance structures
hybridization
structural formula
91
Which of the following elements commonly form diatomic molecules through covalent bonding?
Calcium
Helium
Sodium
Nitrogen
92
Which molecule has a trigonal planar shape?
Boron trifluoride (BF3)
Ammonia (NH3)
Water (H2O)
Methane (CH4)
93
Which molecule contains a carbon-carbon double bond with both a sigma and a pi bond?
Hydrogen (H2)
Methane (CH4)
Ethyne (C2H2)
Ethene (C2H4)
94
What is a single covalent bond?
A bond formed by the transfer of electrons
A bond that occurs only between identical atoms
A bond where two electrons are shared between two atoms
A bond where four electrons are shared between two atoms
95
What type of hybridization is present in ethyne (C
2
H
2
)?
sp3
sp3d
sp
sp2
96
Which type of hybridization is involved in a molecule with a linear geometry?
sp2d
sp2
sp3
sp
97
What type of bond is formed between two oxygen atoms in O
2
?
Triple covalent bond
Ionic bond
Double covalent bond
Single covalent bond
98
A molecule of carbon dioxide (CO
2
) contains:
One triple covalent bond
Two double covalent bonds
One single and one double covalent bond
Two single covalent bonds
