Hi, I just had a what I think should be simple question. Kaplan lists carboxylic acids as the highest priority functional group because it has the highest oxidation state. I was just wondering why it's considered to be so oxidized.
In my ochem book, I read that bonds to oxygen or electronegative atoms (as well as loss of bonds to hydrogen) are oxidizing because the carbon in question has less electron density. However, isn't the hydroxyl group electron donating? I'm pretty sure I'm mixing up something critical here.
I read here that for sigma bonds, the hydroxyl group is electron withdrawing because of electronegativity; however, for pi bonds, it can be electron donating depending on resonance. Aren't there resonance structures for carboxylic acids; if my guess is right, doesn't that mean that the hydroxyl group is electron donating?
Thank you in advanced.
In my ochem book, I read that bonds to oxygen or electronegative atoms (as well as loss of bonds to hydrogen) are oxidizing because the carbon in question has less electron density. However, isn't the hydroxyl group electron donating? I'm pretty sure I'm mixing up something critical here.
I read here that for sigma bonds, the hydroxyl group is electron withdrawing because of electronegativity; however, for pi bonds, it can be electron donating depending on resonance. Aren't there resonance structures for carboxylic acids; if my guess is right, doesn't that mean that the hydroxyl group is electron donating?
Thank you in advanced.
