Chemical Forums
Chemistry Forums for Students => Organic Chemistry Forum => Topic started by: NewtoAtoms on March 22, 2009, 03:28:20 AM
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Hello Organic Chemists,
Would someone please shed some light on this question for me? I have done most of the leg work but I am stuck between two choices
Which amine is the weakest base?
1. CH3CH2NH2 5.6 x 10-4 pKb = 3.2 STRONG BASE
2. (CH3)2NH 5.1 x 10-4 pKb = 3.3 STRONG BASE
3. C6H5CH2NH2 (benzyl amine) pKb = 4.67 STRONG BASE
4. C6H5NH2 (Aniline) pKb = 9.42 WEAK BASE
5. C6H5CH2NHCH3 (N-methyl benzyl amine) ???
Now I know that arylamines are weaker bases than alkylamines, therefore 1,2 are eliminated.
My issue is between 4,5. I am leaning toward Aniline being the weakest bast, however I have researched N-methyl benzyl amine extensively and I can't find out about it.
Can anyone shed some light on this for me.
I would be so grateful and thank you for your time.
Newtoatoms
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You should not need pkb information for this (in fact it's a crutch). You should be able to evaluate these compounds qualitatively. I imagine that's actually what this problem is expecting as well.
What is the difference between aniline and N-methyl benzyl amine? How does this group (think about sterics, resonance and induction) affect the resulting cation that forms when the nitrogen takes a proton?
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Hello macman,
Steric hinderance decreases nucleophile strength and increases base strength.
Therefore if I were to compare the structures and their substitutents, without comparing Pkb values I would conclude:
H
l
C6H5-N: Aniline
l less sterically hindered
H
H
l
C6H5 - N N-methyl benzyl amine
l more sterically hindered
HCH
H
Because N-methyl benzyl amine is more sterically hindered it is the stronger base, because "Steric hinderance decreases nucleophile strength and increases base strength"
I find this very confusing, and I have tried to understand it here, am I at all correct?
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N-methyl benzyl amine should be more basic, but not because of steric hindrance. Think about inductive effects. Which way is the dipole in the C-N bond of the methyl group? Does that increase or decrease electron density, and how does that affect the stability of a positive charge on the nitrogen (when it acts as a base).