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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
Condensed structures show:
atoms - not bonds
26
Resonance structures
overall charge must remain the same - can be equivalent and non-equivalent
27
Stability of Resonance Structures
- we want more spread out/balanced formal charge; avoid concentration of FC - rather have negative FC on more electronegative atoms
28
Hybrid Structures
average of resonance structures
29
VSEPR
lone pairs repel - 2x & 3x bonds take up more space
30
VSEPR - Linear electron geometry
180 degrees 2 electron regions
31
VSEPR - Trigonal Planar electron geometry
3 electron regions 120 degrees
32
VSEPR - Trigonal Planar + 1 Lone Pair makes a ____________ electron geometry
3 electron regions bent-angular 120 degrees
33
VSEPR - Tetrahedral electron geometry
109.5 degrees 4 electron regions
34
VSEPR - tetrahedral + 1 Lone pair makes a ________ electron geometry
trigonal pyramidal < 109.5 degrees 4 electron regions
35
VSEPR - terahedral + 2 lone pairs makes a _______ electron geometry
bent/angular <<109.5 4 electron regions
36
VSEPR - trigonal bipyramidal electron geometry
5 electron regions 90 & 120 degrees
37
VSEPR - trigonal bipyramidal + 1 lone pair makes a _____________ electron geometry
seesaw <90 & <120 5 electron regions
38
VSEPR - trigonal bipyramidal + 2 lone pairs makes a ____________ electron geometry
t-shape <90 degrees 5 electron regions
39
VSEPR - trigonal bipyramidal + 3 lone pairs makes a ____________ electron geometry
linear 180 degrees 5 electron regions
40
VSEPR - octahedral electron geometry
90 degrees 6 electron regions
41
VSEPR - octahedral + 1 lone pairs makes a ____________ electron geometry
square pyramid <90 degrees 6 electron regions
42
VSEPR - octahedral + 2 lone pairs makes a ____________ electron geometry
square planar 90 degrees 6 electron regions
43
VSEPR - octahedral + 3 lone pairs makes a ____________ electron geometry
t-shape <90 degrees 6 electron regions
44
VSEPR - octahedral + 4 lone pairs makes a ____________ electron geometry
linear 180 degrees 6 electron regions
45
Isomers
constitutional stereo-isomers cis & trans isomers conformational isomers
46
Constitutional isomers
different atomic connectivity
47
stereo-isomers
reflections - split into configurational and conformational
48
conformational isomers
type of stereo-isomers rotationally different
49
configurational isomers
type of stereo-isomer split into geometric & optical
50
optical isomers
- type of configurational isomers - split into diastereomers and enantiomers
51
diastereomers
not all chiral molecules change - achiral molecule : Meso compounds - have plane of symmetry and change chiral molecules - cis& trans
52
cis & trans
can always be diastereomers but not all diastereomers can be cis & trans
53
Cis
same
54
trans
different/opposite
55
enantiomers
all chiral centers change - mirrored
56
Octet rule exceptions (3)
- incomplete ( B, Al, Ga) - expanded (>= Si) - odd electron species: have unpaired electrons (reactive!)
57
Functional groups: ether bunny
know structure
58
Functional groups: ketone
O=2R
59
Functional groups: amide
O=R & NHR
60
Functional groups: aldehyde
O=R&H
61
Functional groups: amine
R-NH2
62
Functional groups: carboxylic acid
O=R & OH
63
Functional groups: ester
O=R&OR
64
Functional groups: alcohol
R-OH
65
multi-electron system leads to a _______________ due to electron-electron repulsion
separation in subshells
66
energy level difference does not affect ____________ released when atoms relaxes
number of photons
67
EA =
-H ea
68
molecules with lots of O & an H will have an ___ bond
OH ie. HCO3-
69
The Hea value for noble gases is _____ because...
positive; resists addition of electron
70
as electronegativity increases, Hea will ________ in magnitude and become more __________
increase; negative
71
the longest wavelength of a photon corresponds to the ____________ energy
smallest
72
as electronegativity increases, electron affinity ____________
increases
73
as electronegativity increases, ionization energy ___________
increases
74
as electronegativity increases, atomic radius ____________
decreases
75
as electronegativity increases, n _________ & Zeff _________
decrease in the column; increases in the row
76
as N increases, Z eff ________ and AR ________
decreases;increases
77
as N increases, energy _______ and stability ____
increases; decreases

CHEM201 (2 decks)

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