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Chem 1610 > Chapter 9 > Flashcards

Chapter 9 Flashcards

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1
Q

covalent bond

A

forms between two atoms when a pair of electrons is shared

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2
Q

electron domain

A

the region where electrons will be found

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3
Q

bonding electron pair

A

forming a covalent bond

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4
Q

nonbonding electron pair

A

lone pair: electrons are located on one atom (NH3)

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5
Q

ideal e- domain geometry for 2 e- pairs

A

linear - 180

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6
Q

ideal e- domain geometry for 3 e- pairs

A

trigonal planar -120

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7
Q

ideal e- domain geometry for 4 e- pairs

A

tetrahedral - 109.5

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8
Q

ideal e- domain geometry for 5 e- pairs

A

trigonal bipyramidal (90, 120, 180)

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9
Q

ideal e- domain geometry for 6 e- pairs

A

octahedral (90)

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10
Q

lone pairs and bond angles

A

nonbonding e- pair exerts a repulsive force on adjacent e- pairs = compresses bond angles

bond angles decrease as nonbonding pairs increase: e.g. CH4 —> NH3 —> H2O

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11
Q

polar molecule

A

bond dipoles are not symmetrical

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12
Q

nonpolar molecule

A

bond dipoles cancel (e.g. equal and/or arranged symmetrically around the center)

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13
Q

2 e- domains
2 bonding
0 nonbonding

A

linear e- domain geometry and molecular geometry

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14
Q

3 e- domains
3 bonding
0 nonbonding

A

trigonal planar e- domain geometry

trigonal planar molecular geometry

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15
Q

3 e- domains
2 bonding
1 nonbonding

A

trigonal planar e- domain geometry

bent molecular geometry

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16
Q

4 e- domains
4 bonding
0 nonbonding

A

tetrahedral e- domain geometry

tetrahedral molecular geometry

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17
Q

4 e- domains
3 bonding
1 nonbonding

A

tetrahedral e- domain geometry

trigonal pyramidal molecular geometry

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18
Q

4 e- domains
2 bonding
2 nonbonding

A

tetrahedral e- domain geometry

bent molecular geometry

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19
Q

5 e- domains
5 bonding
0 nonbonding

A

trigonal bipyramidal e- domain geometry

trigonal bipyramidal molecular geometry

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20
Q

5 e- domains
4 bonding
1 nonbonding

A

trigonal bipyramidal e- domain geometry

see saw molecular geometry

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21
Q

5 e- domains
3 bonding
2 nonbonding

Study These Flashcards
A

trigonal bipyramidal e- domain geometry

t-shaped molecular geometry

22
Q

5 e- domains
2 bonding
3 nonbonding

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A

trigonal bipyramidal e- domain geometry

linear molecular geometry

23
Q

6 e- domains
6 bonding
0 nonbonding

Study These Flashcards
A

octahedral e- domain geometry

octahedral molecular geometry

24
Q

6 e- domains
5 bonding
1 nonbonding

Study These Flashcards
A

octahedral e- domain geometry

square pyramidal molecular geometry

25
6 e- domains 4 bonding 2 nonbonding
octahedral e- domain geometry | square planar molecular geometry
26
bonding vs. lone pair attraction
bonding e- pair is attracted by two atoms | nonbonding electron pair centers on one atom
27
lone pairs and bond angels
nonbonding e- pair exerts a repulsive force on adjacent e- pairs = compresses bond angles bond angles decrease as nonbonding pairs increase: e.g. CH4 —> NH3 —> H2O
28
polar
bond dipoles are not symmetrical
29
nonpolar
bond dipoles cancel (e.g. equal and/or arranged symmetrically around the center)
30
molecules you should know
``` 2 e- domains: BeCl2, HCN 3 e- domains: BCl3, CH2O, SO2 4 e- domains: CH4, AsO3^-3, H2O 5 e- domains: PF5, ClF4+, ICl3, XeF2 6 e- domains: SF6, ClF5, XeF4 ```
31
VSEPR
predicts shape around central atoms
32
how do hybrid orbitals form?
AO combine to form hybrid orbitals
33
hybrid orbitals
it holds the shared pair of electrons they possess directional properties sp, sp2, sp3, (sp3d, sp3d2)
34
sp hybrid orbital
sp: BeCl2 - linear sp2: BF3, SO2 - trigonal planar sp3: CH4, NH3, H2O - tetrahedral
35
single bond
aka sigma bond electron density concentrated on the axis connecting the nuclei (internuclear axis) H2, Cl2, BeF2
36
double bond
pi bond side to side overlap of p orbitals: above and below p orbitals are not hybridized they are perpendicular to internuclear axis e- density is above and below nuclei plane (is there a probability of finding p e- density on internuclear axis? NO) less overlap than sigma bond ethylene C2H4 —> CH2 = CH2: 5 sigma bonds and 1 pi bond
37
which is stronger, pi or sigma bonds?
less overlap so the pi bond is weaker than sigma bond
38
triple bond
acetylene C2H2 | one pi bond above/below, other pi bond is front/behind
39
acetylene
C2H2
40
ethylene
CH2 = CH2
41
delocalized pi bonding
possessed by molecules with two or more resonance structures e.g. SO2, NO3-, benzene
42
MO for s orbitals
addition: sigma bonding orbital - constructive interaction with high electron density along internuclear axis subtractions: sigma antibonding orbital - destructive interaction NO electron density between nuclei
43
which MO is more stable?
the more stable MO bonding orbital (sigma) is lower in energy that the atomic orbital (AO) the less stable MO anti bonding orbital is higher in energy that the atomic orbital
44
BO
1/2 (electron in bonding MO - electrons in antibonding MO)
45
MO for p orbitals
when you add then you can make a sigma bonding orbital constructive interaction with electron density along internuclear axis (like s MO) subtraction: antibonding orbital destructive interaction: NO electron density between nuclei (like s MO)
46
MO orbital for sideways p orbital overlap
addition: pi bonding orbital - constructive interaction w/ e- density above/below, front/behind internuclear axis between nuclei subtraction: pi antibonding orbital - destructive interaction w/ NO e- density between nuclei
47
degenerate
p(pi) MO are degenerate = have the same exact energy
48
which is the most effective form of overlap?
head on is more effective than isdeways
49
MO exceptions for diatomics
sigma, pi, pi, sigma for B2, C2, N2 sigma, pi, sigma, pi for O2, F2, and Ne2 due to orbital interactions
50
BO and bond length
a BO of 1.5 has a shorter and stronger bond than a BO of 1.2

Chem 1610 (7 decks)

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