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Chem 1610 > Chapter 9 > Flashcards

Chapter 9 Flashcards

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

A

trigonal bipyramidal e- domain geometry

t-shaped molecular geometry

22
Q

5 e- domains
2 bonding
3 nonbonding

A

trigonal bipyramidal e- domain geometry

linear molecular geometry

23
Q

6 e- domains
6 bonding
0 nonbonding

A

octahedral e- domain geometry

octahedral molecular geometry

24
Q

6 e- domains
5 bonding
1 nonbonding

A

octahedral e- domain geometry

square pyramidal molecular geometry

25
Q

6 e- domains
4 bonding
2 nonbonding

A

octahedral e- domain geometry

square planar molecular geometry

26
Q

bonding vs. lone pair attraction

A

bonding e- pair is attracted by two atoms

nonbonding electron pair centers on one atom

27
Q

lone pairs and bond angels

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

28
Q

polar

A

bond dipoles are not symmetrical

29
Q

nonpolar

A

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

30
Q

molecules you should know

A 
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
Q

VSEPR

A

predicts shape around central atoms

32
Q

how do hybrid orbitals form?

A

AO combine to form hybrid orbitals

33
Q

hybrid orbitals

A

it holds the shared pair of electrons
they possess directional properties
sp, sp2, sp3, (sp3d, sp3d2)

34
Q

sp hybrid orbital

A

sp: BeCl2 - linear
sp2: BF3, SO2 - trigonal planar
sp3: CH4, NH3, H2O - tetrahedral

35
Q

single bond

A

aka sigma bond

electron density concentrated on the axis connecting the nuclei (internuclear axis)
H2, Cl2, BeF2

36
Q

double bond

A

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
Q

which is stronger, pi or sigma bonds?

A

less overlap so the pi bond is weaker than sigma bond

38
Q

triple bond

A

acetylene C2H2

one pi bond above/below, other pi bond is front/behind

39
Q

acetylene

40
Q

ethylene

41
Q

delocalized pi bonding

A

possessed by molecules with two or more resonance structures

e.g. SO2, NO3-, benzene

42
Q

MO for s orbitals

A

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
Q

which MO is more stable?

A

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
Q

BO

A

1/2 (electron in bonding MO - electrons in antibonding MO)

45
Q

MO for p orbitals

A

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
Q

MO orbital for sideways p orbital overlap

A

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
Q

degenerate

A

p(pi) MO are degenerate = have the same exact energy

48
Q

which is the most effective form of overlap?

A

head on is more effective than isdeways

49
Q

MO exceptions for diatomics

A

sigma, pi, pi, sigma for B2, C2, N2

sigma, pi, sigma, pi for O2, F2, and Ne2

due to orbital interactions

50
Q

BO and bond length

A

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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