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AP Chemistry > Chapter 10: Molecular Structure and Bonding Theories > Flashcards

Chapter 10: Molecular Structure and Bonding Theories Flashcards

1
Q

the arrangement of the atoms in a molecule has a strong influence on its

A

physical properties and chemical reactivity

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2
Q

the valence-shell electron-pair repulsion (VSEPR) model predicts the shapes of most molecules from their

A

Lewis structures

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3
Q

the main premise of VSEPR model is that the electron pairs about an atom

A

repel each other

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4
Q

VSEPR Rule 1: a molecule hs a shape that …..

A

minimizes eletrostatic repulsions between valence-shell electron pairs

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5
Q

minimum repulsion results when the electron pairs are as

A

far apart as possible

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6
Q

the VSEPR model predicts the shape around

A

each central atom

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7
Q

steric number =

A

(number of lone pairs on central atom) + (number of atoms bonded to central atom)

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8
Q

the steric number is used to determine the

A

bonded-atom lone-pair arrangement

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9
Q

the BALPA is the shame that maximizes the distances between

A

regions of electron density about a central atom

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10
Q

bond angles for linear

A

180

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11
Q

bond angles for trigonal planar

A

120

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12
Q

bond angles for tetrahedral

A

109.5

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13
Q

bond angles for trigonal bipyramidal

A

90 and 120

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14
Q

bond angles for octahedral

A

90 and 90

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15
Q

SN: 2, balpa:

A

linear

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16
Q

SN: 3, BALPA:

A

trigonal planar

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17
Q

SN: 4, BALPA:

A

tetrahedral

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18
Q

SN: 5, BALPA:

A

trigonal bipyramidal

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19
Q

SN: 6, BALPA:

A

octahedral

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20
Q

two positions for molecular shapes:

A

axial and equatorial

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21
Q

axial atoms have different … from equatorial ones

A

environments

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22
Q

when central atoms have lone pairs, the molecular shape is not the same as the

A

bonded-atom lone-pair arrangement

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23
Q

the molecular shape is the geometric

A

arrangement of the atoms in a species

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24
Q

the lone pairs influence the molecular shape but are …, because there are no atoms at the …

A

not part of it; locations of the lone pairs

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25
each type of electron pair exerts a different
repulsion on other electron pairs
26
VSEPR Rule 2: forces between electron pairs vary as
lone-pair-lone-pair repulsion>lone-pair-bonding-pair repulsion>bonding-pair-bonding-pair repulsion
27
in a trigonal bipyramidal BALPA, the structure that minimizes the number of 90 degree lone pair interactions is favored-
lone pairs always go to the equatorial position
28
for molecules with more than one central atom, the geometry about each atom is assigned by applying the VSEPR model to each
central atom individually
29
the VSEPR model does not predict how the geometry around one central atom will be oriented with respect to
others in the moleule
30
polar molecules will orient to maximie
electrostatic attractions
31
the degree of polarity is measured by a
dipole moment
32
the dipole moment is the magnitude of the separated charges times the
distance between them
33
the ... between bonded atoms is used to predict the polarity of each bond, known as the ...
difference in electronegativity; bond dipole
34
the dipole moment of the molecule is the
vector sum of the individual bond dipoles
35
molecules with lone pairs of electrons on a central atom generally are
polar
36
a molecule with polar bonds is nonpolar if its geometry causes the
bond polarities to sum to zero
37
molecules are nonpolar when there are no ... on the central atom and all of the atoms bonded to the central atom are ...
lone pairs; identical
38
valence bond theory describes covalent bonds as being fromed by atoms sharing valence electrons in
overlapping valence orbitals
39
(valence bond theory) the bonding is based on the ... available to make bonds and the .... that the atoms provide for bonding
orbitals; number of valence electrons
40
hybrid orbitals are orbitals obtained by
mixing two or more atomic orbitals of the same central atom
41
the new hybrid orbitals have different ... and ... properties from the orbitals used in constructing them
shapes; directional
42
the energy and directional characteristics of the new hybrid orbitals are decided by the ... and ... of atomic orbitals used in the mixing
type; number
43
1 s orbital + 1 p orbital forms
two sp hybrid orbitals
44
the sp hybrid orbitals describe the bonding on central atoms that have
180 degree bond angles
45
the steric number of 2 indicates ... hybrid orbitals
sp
46
1 s orbital + 2 p orbitals forms
3 sp^2 hybrid orbitals
47
for sp2 hybrid orbitals, ... remains unchanged
one p orbital
48
the sp2 hybrid orbitals describe the bonding on atoms that have ... and a steric number of ..
120 degree bond angles; 3
49
1 s orbital + 3 porbitals forms
4 sp^3 hybrid orbitals
50
the sp3 hybrid orbitals describe the bonding on central atoms that have approximately .... and a steric number of ..
109-degree bond angles; 4
51
for molecules that have central atoms with steric numbers of 5 or 6, more than ... are needed to make the hybrid orbitals
four atomic orbitals
52
the additional orbitals are taken from the
d subshell
53
1 d orbital + 1 s orbital + 3 p orbitals forms
5 sp^3d hybrid orbitals
54
2 d orbitals + 1s orbital + 3 p orbitals
six sp^3d^2 hybrid orbitals
55
the steric number and number of hybrid orbitals are
equivalent
56
sigma bonds exist int he region
directly between two bonded atoms
57
in a sigma bond, the shared pair of electrons is symmetric about th eline
joining the two nuclei of the bonded atoms
58
all single bonds are
sigma bonds
59
sigma bonds form from the overlap of ... orbitals or hybrid orbitals oriented ...
s or p; along the bond
60
all hybrid orbitals make only
sigma bonds
61
pi bonds exist in the region ... between two bonded atoms
above and below a line drawn
62
double bonds have .. sigma bond and ... pi bond
1; 1
63
triple bonds have .. sigma bond and ... pi bond
1; 2
64
isomers are compounds with the same ... but different ...
molecular formula; structures
65
when double bonds are formed between two carbon atoms, the potential for ... isomerism arises due to lack of ... around double bonds
cis-trans; rotation
66
cis-trans isomerism is observed only if each carbon atom has
2 different substitutents attached
67
pi bonds contribute to the ... model of electrons in bonding, and help explain ..
delocalized; resonance
68
electron density from pi bonds can be distributed ... all around the ring, above and below the plane
symmetrically
69
molecular orbital theory is a model that combines atomic orbitals to form new orbitals that are shared over the
entire molecule rather than between two atoms
70
a molecular orbital is a ... of an electron in a molecule
wave function
71
the number of molecular orbitals formed must equal the number of
atomic orbitals used to make them
72
these wave functions can be added to generate ... or they can be subtracted to generate ...
bonding orbitals; anti-bonding orbitals
73
bonding orbitals concentrate electron density
between atoms
74
anti-bonding orbitals reduce the
electron density between atoms
75
bonding molecular orbitals are ... and antibonding molecular orbitals are ... than the atomic orbitals that are combined
more stable; less stable
76
moleuclar orbital theory allows us to calculate bond order (...) and the number of unpaired electrons (...)
measure of stability; paramagnetism
77
according to molecular orbital theory, bond order is :
1/2(# e- in bonding orbitals - #e- in anti-bonding orbitals)
78
a homonuclear diatomic molecule contains
two atoms of the same element
79
heteronuclear diatomic molecules contain one atom of each of
two different elements t
80
the molecular orbital diagrams are close to those for homonuclear diatomic molecules when the valence energies for each atom are
fairly close in energy
81
delocalized molecular orbitals are: orbitals in which an electron in a molecule is
spread over more than two atoms
82
cis: same substituents
parallel
83
trans: substitutents are
opposite to each other

AP Chemistry (24 decks)

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