Using Structure to Predict Acidity/Basicity
[Pages:3]Using Structure to Predict Acidity/Basicity
Strong acid ? relatively unstable acid ? relatively stable conjugate base
Weak acid ? relatively stable acid ? relatively unstable conjugate base
Strong base ? relatively unstable base ? relatively stable conjugate acid
Weak base ? relatively stable base ? relatively unstable conjugate acid
Effect of Structure on pKa I
1. Charged vs. noncharged species a charged molecule is more acidic than a neutral molecule
NH4 + pKa = 9.4
NH3 + H+
NH3 pKa = 36
NH2- + H+
2. Electronegativity of the atom attached to H the more EN the attached atom, the more acidic the molecule
C < N < O < F
relative electronegativity
-CH3 < -NH2 < HO- < F-
relative stability of conjugate bases
CH4 < NH3 < H2O < HF relative acidity
CH3OH vs pKa = 15.5
CH3NH2 pKa = 40
1
Effect of Structure on pKa II
3. Size of attached atom the larger the attached atom, the more acidic (down column)
I > Br > Cl > F
relative size
I- > Br- > Cl- > F-
relative stability of conjugate bases
HI > HBr > HCl > HF relative acidity
4. Inductive electron withdrawal a. Magnitude of electronegativity (the more EN, the more acidic) b. Distance away from (-) charged conjugate base (closer = more acidic)
O
H3C OH pKa = 4.76
O
I C OH H2 pKa = 3.15
O
Br C OH H2
pKa = 2.86
O
Cl C OH H2
pKa = 2.81
O
F C OH H2
pKa = 2.66
Example: N vs O vs S
H H3C S
H pKa = -6.8
H3CH2C S H pKa = 10.6
H H3C O
H pKa = -2.4
H3CH2C O H pKa = 15.9
H H3C N H
H pKa = 9.8
H H3CH2C N
H pKa = 35
Nitrogen is most effective at stabilizing a positive charge and least effective at stabilizing a negative charge
Sulfur is most effective at stabilizing a negative charge and least effective at stabilizing a positive charge
2
Effect of Structure on pKa III
5. Hybridization (sp, sp2, sp3)
Relative Acidity
sp 50% s character
>
sp2 33% s character
>
sp3 25% s character
H
H
HC C H
>
H2C
> H3C C H
H
H
pKa = 25
pKa = 44
pKa = 50
Conjugate base has negative charge, which is stabilized by orbitals with greater s character
Effect of Structure on pKa IV
6. Resonance resonance stabilizes the negative charge of the conjugate base the more resonance contributors, the more stable the molecule
H3C OH pKa = 15.9
O H3C OH
pKa = 4.76
H3C
O + H+
O
O
H3C O
H3C O
electron delocalization
+ H+
3
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