Chapters 8 & 9 Flashcards

1
Q

4 elements that can have an expanded octet

A

Sulfur, phosphorus, silicon, and chlorine

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2
Q

linear bond angle & #e⁻ groups

A

180 & 2

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3
Q

trigonal planar bond angle & #e⁻ groups

A

120 & 3

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4
Q

tetrahedral bond angle & #e⁻ groups

A

109.5 & 4

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5
Q

trigonal bipyramidal bond angle & #e⁻ groups

A

90 from top, 120 from center; 5

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6
Q

octahedral bond angle & #e⁻ groups

A

90 & 6

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7
Q

name for “middle” atoms & “top/bottom” atoms on tri-bipyr & octa shapes

A

equatorial & axial

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8
Q

Name & bond angle of - 1 e⁻ group from tri-planar

A

bent & <120

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9
Q

Name & bond angle of - 1 e⁻ group from tetrahedral

A

trigonal pyramidal & <109.5

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10
Q

Name & bond angle of - 2 e⁻ groups from tetrahedral

A

bent & <109.5

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11
Q

Name & bond angle of - 1 e⁻ group from trigonal-bipyramidal

A

see-saw & <90, <120, <180

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12
Q

Name & bond angle of - 2 e⁻ groups from trigonal-bipyramidal

A

T-shaped & <90, >180

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13
Q

Name & bond angle of - 3 e⁻ groups from trigonal-bipyramidal

A

Linear & 180

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14
Q

what types of atoms do e⁻ groups tend to replace

A

equatorial atoms

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15
Q

Name & bond angle of - 1 e⁻ groups from octahedral

A

square-pyramidal & <90, >180

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16
Q

Name & bond angle of - 2 e⁻ groups from octahedral

A

square planar & 90, 180

17
Q

Name & bond angle of - 3 e⁻ groups from octahedral

A

T-shaped & <90, >180

18
Q

Name & bond angle of - 4 e⁻ groups from octahedral

A

Linear & 180

19
Q

5 geometries that are always polar

A

bent, trig-pyramidal, see-saw, T-shape, square pyramid

20
Q

linear hybridization

A

sp

21
Q

trigonal planar hybridization

A

sp²

22
Q

tetrahedral hybridization

A

sp³

23
Q

trigonal bipyramidal hybridization

A

dsp³

24
Q

octahedral hybridization

A

d²sp³

25
Q

what does the superscripted number on hybridizations mean

A

the # of orbitals it superscripts; like p² would mean 2 p orbitals

26
Q

define sigma bond & symbol

A

σ; share e⁻ on internuclear axis (in between 2 atoms’ nuclei)

27
Q

define pi bond

A

shared e⁻ NOT on internuclear axis; instead above/below it

28
Q

sigma and pi bonds for each bond multiple

A
single = 1 σ
double = 1 σ & 1 π
triple = 1 σ & 2π
29
Q

what does delocalized resonance bonding mean?

A

the e⁻ are all around the mol instead of in the bond

30
Q

how to calculate formal charge of an atom

A

atom val e⁻ - # atom non-bond e⁻ - # bonds to atom

31
Q

2 ways to tell the best resonance structure

A

the best one has the most evenly-distributed formal atom charges & the neg charges are on the most elecneg atom

32
Q

def lattice E

A

amt E to separate 1 mol ion comp into gas ions; endothermic rxn

33
Q

2 ways to compare lattice E

A

bigger charge on atoms in the ion = bigger LE (like, MgO is better than NaF)
smaller ion itself = bigger LE

34
Q

how to determine polarity when the element in common between the two comps does NOT have the highest elecneg

A

1) cancel out that element in common

2) between the other 2 elements, the comp that has the HIGHER elecneg one is the more polar one

35
Q

how to determine polarity when the element in common between the two comps DOES have the highest elecneg

A

1) cancel out that element in common

2) between the other 2 elements, the comp that has the LOWER elecneg is the more polar one

36
Q

octet rule exceptions/facts x 3

A

Be & B can have less than octet
any atoms n = 3+ can have more than octet
basically only C, N, O, and F work with the rule lmao