Chapter 7 Acids and Bases; Intermolecular Attractions.
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Transcript of Chapter 7 Acids and Bases; Intermolecular Attractions.
![Page 1: Chapter 7 Acids and Bases; Intermolecular Attractions.](https://reader035.fdocuments.us/reader035/viewer/2022062407/56649f495503460f94c6a876/html5/thumbnails/1.jpg)
Chapter 7Chapter 7Acids and Bases; Acids and Bases; Intermolecular AttractionsIntermolecular Attractions
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Skip section 7.4, 7.10, and 7.14Read (no lecture) Section 7.11, 7.12 and 7.13In Text: 1 a, b, g, h, 2b, 6b, 8a, 11b, c
14, 15, 18 through 2224, 25, 27, 28, 31, 32, 33, 34
End of Chap: 36, 38, 42, 43, 45 a, b, e, 48 through 52 54, 55, 56, 58, 59,
62, 63
Problems for Chapter 7
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HA + B- A- + BHacid base
conjugate base
conjugate acid
Section 7.1Section 7.1Bronsted-Lowry TheoryBronsted-Lowry Theory
+H+
-H+
acid = proton donorbase = proton acceptorConjugate Acid = Base + ProtonConjugate Base = Acid - Proton
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pKa = - log Kaa
Strong acid = large Ka = small pKaa
Weak acid = Weak acid = small Ka = large pKaa
Section 7.2 pKa
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HClO4 ClO4
_stronger
weaker
ACIDSTRENGTH
weaker
stronger
BASESTRENGTH
ACID CONJ. BASE Ka pKa
10 -1010
10 -5
10-10
10 50-50
5
-
10
10 16-16
OH O
CH3 C OH
O
CH3 C O
O
CH3 CH3 CH3 CH2
_
CH3CH2O-H CH3CH2O
Sect. 7.2 Relative Acid and Base Strengths
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Strong Acid Conjugate base is weak pKa is small
Weak Acid Conjugate base is strong pKa is large
Acid Strengths
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Section 7.3: Lewis Acid-Base theory
B: electron-pair donor
BASE
A ACIDelectron-pair acceptor
Some Lewis Acids: Fe3+ BF3 H3O+
Some Lewis Bases: NH3 H2O
more general than Bronsted theory
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Section 7.5Section 7.5Electronegativity Electronegativity and Size Effects and Size Effects
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C N O F
P S Cl
Br
I
Se
Si
electronegativity increases acidityincreased
increased
size
increasesacidity
Sect. 7.5: Electronegativity and Size
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Effect of Atomic Size on AcidityEffect of Atomic Size on Acidity
R C
O
OH
R C SH
O
R C SH
S
HOH
HSH
HSeH
HTeH
HF
HCl
HBr
HI
increasingatom size pKa Values
3.5
-7
-9
-10
16
7
4
3
5
F- Cl- Br- I-
1.36 A 1.81 A 1.95 A 2.16 A
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CH4
NH3
H2O
HF
RCH3
RNH2
ROH
R C
O
CH3
R C NH2
O
R C OH
O
>45
34
16
3.5
45
35
18
20
15
5
Effect of Electronegativity on AcidityEffect of Electronegativity on Acidityincreasing electronegativity pKa Values
CH
H
H
H N
H
H O F_ _ _ _
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Section 7.6 Section 7.6 Resonance EffectsResonance Effects
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Take Away Lession:
Resonance strengthens acidResonance weakens base
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CH3 C O
O
H-H+
CH3 C
O
O
CH3 CO
O
base
_
_
acetate ion
Resonance in the Acetate Resonance in the Acetate IonIon
acetic acid
equivalent structurescharge on oxygens
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Phenolate ion ResonancePhenolate ion Resonance
O
-
_
_
_
_
_
O O
OOO
non-equivalent structurescharge on carbon and oxygen
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NitrophenolsNitrophenols
Placing a nitro group on the benzene ringof a phenol increases its acidity.
The effect is largest when the nitro groupis placed in an ortho or a para position onthe ring, and considerably smaller for themeta position.
Multiple nitro groups at the ortho and parapositions can increase the pKa of a phenolto the point that it becomes a very strong acid.
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OH
O2N
NO2OH
NO2
OH
NO2
OH
NO2
OH OH
NO2O2N
NO2
10
7.2
7.3
0.4
pKa Values of NitrophenolspKa Values of Nitrophenols
9.3 4.0
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_Resonance in Resonance in pp--NitrophenolNitrophenol
_
_
_
_
O
NO2
O
NO2
O
NO O
O
NO2
O
NO2
O
NO O
_
_ _+
extrastructure
When in an orthoor para positiona nitro group canparticipate inresonance.
+
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Section 7.7Section 7.7Alpha Hydrogen Alpha Hydrogen compoundscompounds
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Acid pKa
CH3CH2CH2CH2-H
H
H
H
H
R H
O
OCH2CH3H
O
CH3H
Acid pKa
O
OCH2CH3CH3CH2O
O
H
~50
44
25
24
20
13
O
CH3H3C
O
H
9
10H-CH2NO2CNH 25
CNNC11
H
NO2O2N4
H
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Take Away Lession:
Resonance strengthens acidResonance weakens base
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Section 7.8Section 7.8Inductive EffectsInductive Effects
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Resonance operates through the bonding system. It doesn’t drop off with distance.
Inductive effect operates through the sigma bonding system. It drops off with increasing distance.
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Cl-
C CH3
-
C
ELECTRONWITHDRAWINGGROUPS
ELECTRONDONATINGGROUPS
F, Cl, Br, NO2 , NR3+ R, CH3
Types of Inductive Types of Inductive EffectsEffects
electronegative elements take electron densityfrom cabon. This strenthens the acidity.
alkyl groups donate electron density to carbon. This weakensthe acidity.
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Cl C C C-
- + - +
O
O
Inductive Effects on Inductive Effects on HaloacidsHaloacids
The effect diminishes with distance - it carries for about 3 bonds.
Cl C
O-Chlorine helps
to stabilize -CO2-
by withdrawingelectrons
O
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Inductive Effects Inductive Effects
I CH2COOH
Br CH2COOH
Cl CH2COOH
F CH2COOH
CH3 COOH
Cl CH2 COOH
Cl CH COOH
Cl
Cl C COOH
Cl
Cl
3.13
2.87
2.81
2.66
4.75
2.81
1.29
0.65
pKa Valuesincreasingelectronegativity
multiplesubstituents
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CH3CH2CH2 COOH
COOHCH2CH
Cl
CH3
COOHCH
Cl
CH3CH2
COOHCH2CH2CH2
Cl
COOHH
COOHCH3
COOHCH3CH2
COOHCH3CH2CH2
COOHCCH3
CH3
CH3
Inductive EffectsInductive Effects
pKa Values
3.75
4.75
4.87
4.81
5.02
4.8
4.5
4.0
2.9
distance
Alkyl groups release electrons.This decreases acidity
When the chlorine atom is moved further away from the carboxyl group,acidity decreases
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Section 7.9Section 7.9Hybridization EffectsHybridization Effects
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Effect of HybridizationEffect of Hybridization
C C HH
C C HH
H H
C HH
H
H
sp3
sp2
sp
ca. 50
35
25
sp orbitals are more electron withdrawing than sp3 orbitals (sp orbitals have more s character). sp > sp2 > sp3
pKa values
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Section 7.11Section 7.11Solvent Effects Solvent Effects
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CO
O-
H
OH
H
OH
H
OHH
O H
H
O H
Solvation EffectsSolvation Effects
4.75
4.87
4.81
Notice that these are all similar
COOHCH3
COOHCH3CH2
COOHCH3CH2CH2
COOHCCH3
CH3
CH3
5.02
….but this one has a larger pKa
This is probably a solvation effect. Solvation lowers the energy of the ion.
The bulkyt -butyl groupis not as wellsolvated.
StrongerAcid
WeakerAcid
unbranched
steric hindrance
CO
O
-H
OH
H
OH
H
OHO
H
H
H
O H
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Sect. 7.12: Intermolecular Attractions•hydrogen bonding•dipole-dipole attractions•London forces or van der Waals attractions
Sect. 7.13: Solubility
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SUMMARYSUMMARY
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Electronegativity of atom bearing acidic hydrogen; more electronegative = more acidic
Size of atom bearing acidic hydrogen; larger = more acidic.
Resonance: greater charge delocalization in conjugate base = more acidic.
alpha-hydrogens: carbonyls, nitro, cyano, etc. Greater charge delocalization in conjugate base = more acidic.
Inductive effect: electronegative atoms withdraw electrons making the acid more acidic.
Hybridization; more s-character = more acidic
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40 20 10 5 0
HCl
HBr
HIR CH3 C C
H
H
H
R
R NH2
H2SO4
HClO4
HNO3
weak acids strong acids
Classification of Weak and Strong Acids Classification of Weak and Strong Acids by Functional Groupby Functional Group
pKa
inorganic acidsoxyacids
carboxylic acidsnitrophenols
phenols-diketones
alcoholsketonesamidesalkynes
alkenesamines
alkanes
C C HR
OH
R
O
CH2 R
OR C
O
OH
nitrophenolsdi- and tri-R C CH3
O
R C NH2
OR OH
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Electron-Withdrawing Effects Electron-Withdrawing Effects Strengthen AcidsStrengthen Acids
R C
O
O
C
O
O
O R S
O
O
O
Any effect that “bleeds” electron density away from the negatively-charged end of the conjugate base willstabilize (lower the energy) of the conjugate base and make it a weaker base.The parent acid will be a stronger acid.
- -
- -
-
(-) (-)
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Electron-Donating Effects Electron-Donating Effects Weaken AcidsWeaken Acids
R C
O
O
C
O
O
O R S
O
O
O
Any effect that “pushes” extra electron density toward the negatively-charged end of the conjugate base willdestabilize (increase the energy) of the conjugate baseand make the base weaker. The parent acid will be stronger.
- -
- --
-
(-) (-)
Conversely …..