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Pearson Chemistry Chapter 8: Covalent Bonding Flashcards | StudBud
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Pearson Chemistry Chapter 8: Covalent Bonding
Pearson Chemistry Chapter 8: Covalent Bonding
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Chapter 8 Pearson Chemistry Textbook Review
Flashcards
55 cards
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Questions
55
Answers
1
In a ____ molecule, one end is slightly negative and the other end is slightly positive.
coordinate
ionic
nonpolar
polar
2
There is no such thing as a molecule of sodium chloride or magnesium chloride.
False
True
3
A structural formula represents the covalent bonds by ____.
dashes
stars
circles
dots
4
What is the molecular formula of ammonia, pictured here?
NH3(g)
H3C(g)
CH3(g)
NH2(g)
5
What is bond dissociation energy?
energy to move an electron to the next highest energy level
energy to form bonds between atoms
energy to break the bond between two ionically bonded atoms
energy to break the bond between two covalently bonded atoms
6
Which of these is a diatomic molecule?
F2
H2SO4
H2O2
CO2
7
Octet rule doesn't apply to any molecules whose total number of valence electrons is an even #.
True
False
8
Which hybrid orbital is pictured here?
sp4
sp
sp2
sp3
9
When polar molecules are placed between oppositely charged plates, they orient with...
respect to the more nonmetallic plate
respect to the bigger plate
respect to the smaller plate
respect to the charge of the plates
10
A polar covalent bond, known also as a polar bond, is a covalent bond between atoms in which...
electrons are transferred between atoms
electrons as shared unequally
electrons are not shared at all
electrons are shared equally
11
When atomic orbitals overlap, molecular orbitals are produced.
True
False
12
What does VSEPR theory stand for?
valence sigma electron pi repulsion theory
valence-shaped electron prediction-rotation theory
Vince Stollenmayer's Electron Protraction-Reflection theory
valence-shell electron-pair repulsion theory
13
A resonance structure is a structure that occurs when ___ with equal numbers of electron pairs.
there are two or more covalent bonds present
it is possible to draw two or more electron dot structures
it is impossible to draw an electron dot structure
there are two or more ionic bonds present
14
A molecular formula does not tell you about a molecule's structure.
True
False
15
Hydrogen bonds are the strongest of the intermolecular forces.
False
True
16
All covalent bonds contain a metal and a nonmetal.
False
True
17
Intermolecular attractions are stronger than either ionic or covalent bonds.
True
False
18
Molecular compounds tend to have higher melting and boiling points than ionic compounds.
False
True
19
What molecular shape is pictured here?
tetrahedral
pyramidal
bent triatomic
linear triatomic
20
The more electroneg. atom attracts electrons more strongly, gaining a slightly positive charge.
False
True
21
What is the chemical formula of a molecular compound called?
molecular chemical
compound molecule formula
chemical molecule compound
molecular formula
22
A molecular orbital that can be occupied by two electrons of a covalent bond is called a _____.
coordinate covalent bond
molecular compound
polyatomic orbital
bonding orbital
23
A tightly bound group of atoms that has positive or negative charge a behaves as a unit is a _.
molecular ion
monatomic molecule
polyatomic ion
diatomic molecule
24
What type of bond is pictured here?
delta
pi
beta
sigma
25
NH
3
(
g
) is the molecular formula of ammonia. What does the letter in parenthesis mean?
the volume of the molecule
the mass of the molecule in grams
the dimensions of the molecule
the state of matter that the molecule is in
26
Like an atomic orbital applies to an atom, a molecular orbital applies to an entire molecule.
True
False
27
Which hybrid orbital is pictured here?
sp4
sp
sp3
sp2
28
A large bond dissociation energy corresponds to a strong covalent bond.
False
True
29
Why is carbon dioxide nonpolar?
the pulls on the opposite sides cancel each other out
it is an ionic compound
it has two polar bonds
it's not; it's polar
30
In covalent bonds, sharing usually occurs so that atoms get the electron config of noble gases.
True
False
31
VSEPR theory: the repulsion between electron pairs causes molecular shapes to adjust so that...
valence-electron pairs attract one another
valence-electron pairs combine to form covalent bonds
valence-electron pairs transfer electrons between the atoms
valence-electron pairs stay as far apart as possible
32
When do dipole interactions occur?
when polar molecules are attracted to one another
when polar molecules repel one another
when ionic molecules repel one another
when nonpolar molecules are attracted from one another
33
What kind of covalent bond is pictured here?
triple
quadruple
double
single
34
When the atoms in the bond pull equally, the bonding electrons are shared equally. This is a...
polar ionic bond
nonpolar covalent bond
polar covalent bond
nonpolar ionic bond
35
Where does the shared pair of electrons come from in a coordinate covalent bond?
from other bonds outside of the molecule
from one of the unbound atoms
from both atoms in the bond
from one of the bonded atoms
36
What kind of diagram is pictured here?
ball-and-stick molecular model
space-filling molecular model
perspective drawing
structural formula
37
What molecular shape is pictured here?
tetrahedral
bent triatomic
pyramidal
linear triatomic
38
Which of these is NOT a name for a pair of valence electrons that is not shared between atoms?
nonbonding pair
lone pair
unshared pair
free pair
39
What type of bond is pictured here?
sigma
beta
pi
delta
40
How many bonds are pictured here?
one
four
three
two
41
Melting a network solid would require breaking covalent bonds thoughout the solid.
False
True
42
What are dispersion forces caused by?
the motion of protons
the motion of electrons
the motion of neutrons
the motion of molecules
43
Dipole interactions and dispersion forces are collectively known as what?
van der Waals forces
VSEPR forces
ver min Wells forces
Thomson forces
44
Orbital hybridization provides information about both molecular bonding and molecular shape.
True
False
45
The electron dot structure for an oxygen molecule can be represented as O::O.
False
True
46
What type of bond is pictured here?
beta
sigma
pi
delta
47
What does a molecular formula show?
how many molecules an element contains
how many molecules are in an atom of an element
how many atoms of each element a molecule contains
how many atoms are in each type of element
48
hybridization: several atomic orbitals mix to form the same number of equal hybrid orbitals.
False
True
49
What is a molecule?
a crystalline solid
a neutral group of atoms joined together by ionic bonds
a neutral group of atoms joined together by covalent bonds
a group of bonded protons
50
What is a covalent bond?
atoms held together by sharing protons
atoms held together by sharing electrons
atoms held together by transferring electrons
atoms held together by stealing electrons
51
Which hybrid orbital is pictured here?
sp2
sp
sp4
sp3
52
Which state of matter can covalent compounds exist in?
all of the above
solids
gases
liquids
53
The bonding of oxygen atoms in ozone is a ______ of extremes portrayed by resonance forms.
solution
hybrid
portrait
split
54
What is a dipole?
an electron that has two poles
a molecule that has two poles
a compound that has two poles
an atom that has two poles
55
What molecular shape is pictured here?
linear triatomic
tetrahedral
bent triatomic
pyramidal
