- #1
ngu9997
- 27
- 2
So in my organic chem class we learned how to choose the most acidic hydrogens on a molecule based on the stability of the conjugate base of that molecule. And then we used various factors to determine the stability of the conjugate base such as resonance (how resonance may help the negative charge from deprotonation become spread over a larger area).
For vitamin C there's three atoms that can be deprotonated to become the conjugate base. And in these 3 situations, resonance is all present. Two of the situations are an OH becoming deprotonated and one situation is a carbon becoming deprotonated. Typically CH bonds are never really seen as acidic hydrogens. Could someone explain why this is so - and in terms of the logic my class has been using would be especially appreciated (in terms of the stability of the conjugate base).
For vitamin C there's three atoms that can be deprotonated to become the conjugate base. And in these 3 situations, resonance is all present. Two of the situations are an OH becoming deprotonated and one situation is a carbon becoming deprotonated. Typically CH bonds are never really seen as acidic hydrogens. Could someone explain why this is so - and in terms of the logic my class has been using would be especially appreciated (in terms of the stability of the conjugate base).