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CHE118A > Lecture Quiz 2- Lectures 5-10 > Flashcards

Lecture Quiz 2- Lectures 5-10 Flashcards

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1
Q

Def: Arrhenius Acid

A

donates H+ in H2O
-sour, turns litmus pink, reacts w/ metals

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2
Q

Def: Arrhenius Base

A

donates OH- in H2O
-bitter, turns litmus blue, feels soapy

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3
Q

Is CH3OH an Arrhenius Acid or Arrhenius Base? What about CH3COOH?

A

both are not arrehenius acids or bases. They can’t lose the OH- because they are a covalent bond - equal sharing

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4
Q

Def: BL acid

A

donates H+
-almost anything with H

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5
Q

BL acid exceptions

A

sp3 C-H, 6 e- species like CH3+, BH3

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6
Q

Def: BL base

A

accepts H+
-should have a lone pair or (-) charge

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7
Q

BL base exceptions

A

strong acids

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8
Q

Def: Lewis Acid

A

Accepts e- pair into empty orbital

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9
Q

Fe3+. Zn2+, and Cu2+ are:

A

Lewis Acids – metal ions

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10
Q

Def: Lewis Base

A

donate e- pair to an empty orbital (H+)

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11
Q

All BL bases are

A

Lewis bases

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12
Q

Is CH3+ a BL acid?

A

No

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13
Q

Def: electrophile

A

e- loving
-E+
-accepts an e- pair

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14
Q

All BL acids are

A

Lewis Acids

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15
Q

All electrophiles are

A

BL acids = Lewis Acids

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16
Q

An atom has a (-) dipole. Is it electrophilic or nucleophilic?

A

Nu-

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17
Q

An atom has a (+) dipole. Is it electrophilic or nucleophilic?

A

E+

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18
Q

T/F E+ are an expanded def of acids

A

T

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19
Q

Def: basicity

A

abt thermodynamics / delta H

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20
Q

Def: nucleophilicity

A

abt kinetics/rate/Ea

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21
Q

If a halogen is bonded to H, is it a base?

A

Not a base but can lose H+ as it donates e- and act as a Nu-

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22
Q

If a halogen is bonded to a C, is it a base?

A

No and they can’t lose C, so they can’t act as a Nu0

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23
Q

The larger the Ka, the (weaker/stronger) the acid, the (greater/smaller) dissociation

A

The larger the Ka, the stronger the acid, and the greater the dissociation

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24
Q

The larger the pKa, the (weaker/stronger) the acid

A

weaker

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25
What is the pKa range for acids?
-10 - +50
26
The stronger the acid, the (weaker/stronger) the conjugate base.
stronger acid = weaker conjugate base
27
What 5 things make a stronger acid?
Large Electronegative Resonance More S character Induction
28
Acids get stronger as you move (up/down) and (left/right) on the periodic table due to size.
down right
29
Order from weakest to strongest acid HF, HI, HBr, HCl
HF, HCl, HBr, HI
30
A larger atom with a H+ will have a strong/poor orbital overlap for bonds
poor orbital overlap
31
HCl pKa =
-6
32
HBr pKa =
-8
33
HI pka =
-10
34
Order from weakest to strongest acid: H2O, HF, CH4, NH3
CH4, NH3, H2O, HF
35
Why does acidity increase as EN increases
The electronegative atom is already try to hold its e-
36
What has more acidity? A localized or delocalized charge?
delocalized
37
-OH pKa
15-18
38
What's stronger, ethanol or alcohol?
Alcohol
39
Why does acidity increase with more reasonance?
The conjugate base is stabilized when the acid loses a proton, by delocalizing the negative charge across multiple atoms, making it less likely to regain the proton and thus enhancing the acid's ability to donate a hydrogen ion (H+) in solution; essentially, a more stable conjugate base leads to a stronger acid.
40
Acidity increases as more s-orbital character in _____ orbital
hybrid orbital
41
Why does acidity increase with more s character?
e- can approach the nucleus -s orbital e-'s at the nucleus have no node through the nucleus -p orbital e-'s can't be at the nucleus because of it -More s character = the more (+) and (-) chargers can attract
42
Order from weakest to strongest acid: alkyne, alkane, alkene
1st Alkyne - 3 bond -- has 50% S 2nd Alkene - 2 bonds -- has 33% S 3rd Alkyne - 1 bond -- has 25% S
43
The more (protonated/deprotonated) C is, the stronger the acid
deprotonated
44
Def Induction:
subtle, more about where in general range of specific groups is rather than a new pKa range -a long range EN model of effects of neighbors through as pi bonds
45
What are 3 examples of induction
-A neighbor with a larger EN = larger effect, pulls away from H making it easier to dissociate -A lot of neighbors having large effect. -A neighbor that is closer
46
Carboxylic acid pKa:
3-5
47
Alkane pKa:
~50
48
Alkene pKa:
~44
49
Alkyne pKa:
~25
50
List the 4 types of hydrocarbons
alkane, alkene, alkyne, and aromatic/arene
51
What hybridization are all of the C atoms in an Alkane? Alkanes only have what type of bonds?
sp3 -- sigma bonds
52
What hybridization are all of the C atoms in an Alkene
sp2 (double bonds)
53
What hybridization are all of the C atoms in an Alkyne
sp (triple bond)
54
What functional group has a circle of pi electrons?
aromatic/arene
55
Heteroatom functional groups have (sigma/pi/both) bonds and every atom is (sp/sp2/sp3) hybridized.
sigma bonds + sp3
56
What are the 3 types of alkanes?
linear, branched, and cycloalkanes
57
Simple def of linear alkane Ex of linear alkanes
2 ends methane, ethane, propane, butane, pentane
58
Simple def of branched alkanes
3+ ends
59
Def: cycloalkane
0 ends ring
60
A ring has 8 C's. What is it called?
cyclooctane
61
Alkane properties
non-polar not soluble -relatively low bp
62
Boiling point is a measure of
total intermolecular forces
63
As IMF increases, BP (decreases/increases)
IMC inc, BP inc
64
What type of forces do alkanes have?
Only dispersion forces - temporary dipoles due to random e- movement
65
BP increases with
-size -more atoms -more dipole -more surface area -more dispersion -more IMF
66
C10 has (less/more) IMF than C2.
more
67
Def: staggered
front and back atoms are 60 degrees apart
68
Def: eclipsed
Front and back atoms are 0 degrees apart
69
Def: anti
Central atoms are across each other (180 degrees)
70
Def: gauche
Central atoms are 60 degrees apart, bumping into each other
71
Def: big groups passing
Used to describe eclipsed conformation where the central atoms are sterically hindering each other
72
Def: steric hindrance
2 parts of the molecule are bumping / bulkiness bumps into each other
73
Def: torsional strain
electrons in sp3 of adjacent central atoms line up and repel
74
Def: torsional angle
60 degrees
75
Order from lowest E to highest E Staggered gauche Eclipsed big groups passing Stagged anti Eclipsed
Staggered anti < staggered gauche < eclipsed < eclipsed big groups
76
T/F We must go through eclipsed conformation to get to staggered conformation
T
77
Why are all staggered conformations lower in E compared in eclipsed conformations?
Eclipsed conformations have a torsional/eclipsing strain that is higher in E
78
Why are anti conformations lower in E than gauche conformations?
steric hindrance - prefer structures with fewer gauche groups
79
Why are large groups passing H lower in energy than large groups passing each other?
due to steric hindrance
80
Order from least hindrance to most: 1* Carbon, 2* Carbon, and 3* Carbon
1 Carbon, 2 Carbon, and 3 Carbon 3C has the more steric hindrance because it is the bulkiest and takes up the most space
81
T/F Cyclohexanes are drawn planar but they are actually puckered
T
82
Each C in a chair has 1/2/3 H atoms
2 H atoms
83
Each C has one ______ H and one _______ H
1 ax H + 1 eq H 1 up H + 1 down H
84
T/F axial and eq groups stay the same when rotating bonds in the chair
F
85
T/F up and down groups switch when rotating bonds in the chair
F
86
Def: transannular strain
When there is steric hindrance in a chair conformation
87
What has higher energy? Chair or Boat?
Boat --- has a torsional/eclipsing strain

CHE118A (4 decks)

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