D
deleted647690
Hi, I know this is a really basic question
"Which of the following changes to n-propanol would NOT result in a lower pKa than n-propanol?
A. Oxidizing carbon 1 by four electrons, resulting in a pi bond to oxygen instead of two sigma bonds to hydrogen
B. Replacing oxygen with a sulfur atom
C. Replacing the propyl group with a phenyl ring
D. Replacing the OH group with an amine group."
The answer was D. For B, they said that the larger atomic radius of Sulfur allows for easier loss of the proton, which means that it is more acidic.
Then, for D, they said that the nitrogen in the amine group is less electronegative than oxygen, and thus it will not draw electrons as readily.
I was confused by this, because if you are looking at it as acid vs. base, couldn't you say that, because Nitrogen is less electronegative, it holds protons more weakly and thus will give them up more easily? (Thus making it a stronger Bronsted Lowry acid)
But if you look at it as nucleophilic base vs. electrophilic acid, their explanation makes more sense.
Why do they explain choice B in terms of Bronsted Lowry acid/base but choice D in terms of Lewis acid/base (electrophilicity/nucleophilicity)
(IE, proton donation vs. electron acceptance)?
"Which of the following changes to n-propanol would NOT result in a lower pKa than n-propanol?
A. Oxidizing carbon 1 by four electrons, resulting in a pi bond to oxygen instead of two sigma bonds to hydrogen
B. Replacing oxygen with a sulfur atom
C. Replacing the propyl group with a phenyl ring
D. Replacing the OH group with an amine group."
The answer was D. For B, they said that the larger atomic radius of Sulfur allows for easier loss of the proton, which means that it is more acidic.
Then, for D, they said that the nitrogen in the amine group is less electronegative than oxygen, and thus it will not draw electrons as readily.
I was confused by this, because if you are looking at it as acid vs. base, couldn't you say that, because Nitrogen is less electronegative, it holds protons more weakly and thus will give them up more easily? (Thus making it a stronger Bronsted Lowry acid)
But if you look at it as nucleophilic base vs. electrophilic acid, their explanation makes more sense.
Why do they explain choice B in terms of Bronsted Lowry acid/base but choice D in terms of Lewis acid/base (electrophilicity/nucleophilicity)
(IE, proton donation vs. electron acceptance)?