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CHEM201 > LO1-13 + OOB-OOE > Flashcards

LO1-13 + OOB-OOE Flashcards

Midterm Concepts

1
Q

n

A

principle quantum number
- size & energy of atom (row number)

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2
Q

l

A

angular momentum quantum number

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3
Q

s has __ orbital(s); ___ electrons; n = __; l = ___.

A

1;2;1;0

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4
Q

p has ___ orbital(s); ___ electrons; n = __; l = ___.

A

3;6;2;1

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5
Q

d has ____ orbital(s); ___ electrons; n = __; l = ___.

A

5;10;3;2

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6
Q

f has ____ orbital(s); ___ electrons; n = __; l = ___.

A

7;14;4;3

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7
Q

Degenerate means

A

when orbitals within same subshell have the same energy; energetic equivalence

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8
Q

Core electrons are

A

all electrons except those with the highest n value

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9
Q

Paramagnetic

A

one of more unpaired electrons

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10
Q

Diamagnetic

A

no unpaired electrons

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11
Q

Isoelectronic

A

when atoms have the same electron configuration

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12
Q

Z eff

A

found in the units digit of column number

  • net positive charge
  • increases as you move right in the rows
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13
Q

Electronegativity

A

increases in uncle FONCL

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14
Q

Atomic radius

A

increases going left and down on PT

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15
Q

Ionization energy

A

minimum energy required to remove electrons
- exceptions with half-filled or completely filled subshells

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16
Q

Electron Affinity

A

energy change (released) when electrons are added
- positive
- increases going right up

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17
Q

number of columns away from the noble gas is the

A

number of bonds atoms want to make

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18
Q

Formal charge formula

A

valence electrons - # bonds - # lone electrons

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19
Q

CHIRAL

A

can’t be mirrored

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20
Q

ACHIRAL

A

can be mirrored

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21
Q

Relative size of ions is ____ for cations (_) because….

A

smaller; +
- because having less electrons means less electron repulsion, reducing the AR

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22
Q

Relative size of ions is ____ for anions (_) because….

A

larger; -
- because having more electrons increases electron repulsion, increasing the AR

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23
Q

H ea

A

enthalpy of electron attatchment
- energy change when electron is added
- negative

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24
Q

Lewis structures show:

A

bonds, atoms, electrons

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25
Q

Condensed structures show:

A

atoms - not bonds

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26
Q

Resonance structures

A

overall charge must remain the same
- can be equivalent and non-equivalent

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27
Q

Stability of Resonance Structures

A
  • we want more spread out/balanced formal charge; avoid concentration of FC
  • rather have negative FC on more electronegative atoms
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28
Q

Hybrid Structures

A

average of resonance structures

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29
Q

VSEPR

A

lone pairs repel
- 2x & 3x bonds take up more space

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30
Q

VSEPR - Linear electron geometry

A

180 degrees
2 electron regions

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31
Q

VSEPR - Trigonal Planar electron geometry

A

3 electron regions
120 degrees

32
Q

VSEPR - Trigonal Planar + 1 Lone Pair makes a ____________ electron geometry

A

3 electron regions
bent-angular
120 degrees

33
Q

VSEPR - Tetrahedral electron geometry

A

109.5 degrees
4 electron regions

34
Q

VSEPR - tetrahedral + 1 Lone pair makes a ________ electron geometry

A

trigonal pyramidal
< 109.5 degrees
4 electron regions

35
Q

VSEPR - terahedral + 2 lone pairs makes a _______ electron geometry

A

bent/angular
«109.5
4 electron regions

36
Q

VSEPR - trigonal bipyramidal electron geometry

A

5 electron regions
90 & 120 degrees

37
Q

VSEPR - trigonal bipyramidal + 1 lone pair makes a _____________ electron geometry

A

seesaw
<90 & <120
5 electron regions

38
Q

VSEPR - trigonal bipyramidal + 2 lone pairs makes a ____________ electron geometry

A

t-shape
<90 degrees
5 electron regions

39
Q

VSEPR - trigonal bipyramidal + 3 lone pairs makes a ____________ electron geometry

A

linear
180 degrees
5 electron regions

40
Q

VSEPR - octahedral electron geometry

A

90 degrees
6 electron regions

41
Q

VSEPR - octahedral + 1 lone pairs makes a ____________ electron geometry

A

square pyramid
<90 degrees
6 electron regions

42
Q

VSEPR - octahedral + 2 lone pairs makes a ____________ electron geometry

A

square planar
90 degrees
6 electron regions

43
Q

VSEPR - octahedral + 3 lone pairs makes a ____________ electron geometry

A

t-shape
<90 degrees
6 electron regions

44
Q

VSEPR - octahedral + 4 lone pairs makes a ____________ electron geometry

A

linear
180 degrees
6 electron regions

45
Q

Isomers

A

constitutional
stereo-isomers
cis & trans isomers
conformational isomers

46
Q

Constitutional isomers

A

different atomic connectivity

47
Q

stereo-isomers

A

reflections
- split into configurational and conformational

48
Q

conformational isomers

A

type of stereo-isomers
rotationally different

49
Q

configurational isomers

A

type of stereo-isomer
split into geometric & optical

50
Q

optical isomers

A
  • type of configurational isomers
  • split into diastereomers and enantiomers
51
Q

diastereomers

A

not all chiral molecules change
- achiral molecule : Meso compounds - have plane of symmetry and change chiral molecules
- cis& trans

52
Q

cis & trans

A

can always be diastereomers but not all diastereomers can be cis & trans

53
Q

Cis

A

same

54
Q

trans

A

different/opposite

55
Q

enantiomers

A

all chiral centers change
- mirrored

56
Q

Octet rule exceptions
(3)

A
  • incomplete ( B, Al, Ga)
  • expanded (>= Si)
  • odd electron species: have unpaired electrons (reactive!)
57
Q

Functional groups: ether bunny

A

know structure

58
Q

Functional groups: ketone

A

O=2R

59
Q

Functional groups: amide

A

O=R & NHR

60
Q

Functional groups: aldehyde

A

O=R&H

61
Q

Functional groups: amine

A

R-NH2

62
Q

Functional groups: carboxylic acid

A

O=R & OH

63
Q

Functional groups: ester

A

O=R&OR

64
Q

Functional groups: alcohol

A

R-OH

65
Q

multi-electron system leads to a _______________ due to electron-electron repulsion

A

separation in subshells

66
Q

energy level difference does not affect ____________ released when atoms relaxes

A

number of photons

67
Q

EA =

A

-H ea

68
Q

molecules with lots of O & an H will have an ___ bond

A

OH

ie. HCO3-

69
Q

The Hea value for noble gases is _____ because…

A

positive; resists addition of electron

70
Q

as electronegativity increases, Hea will ________ in magnitude and become more __________

A

increase; negative

71
Q

the longest wavelength of a photon corresponds to the ____________ energy

A

smallest

72
Q

as electronegativity increases, electron affinity ____________

A

increases

73
Q

as electronegativity increases, ionization energy ___________

A

increases

74
Q

as electronegativity increases, atomic radius ____________

A

decreases

75
Q

as electronegativity increases, n _________ & Zeff _________

A

decrease in the column; increases in the row

76
Q

as N increases, Z eff ________ and AR ________

A

decreases;increases

77
Q

as N increases, energy _______ and stability ____

A

increases; decreases

CHEM201 (2 decks)

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