\nIn my previous post<\/a> I mention the carboxylic acid functional group. Yet, why is the carboxyl group acidic?<\/p>\n \nThe reason I’ve heard is that the carboxyl group, being -COOH, is a carbon double-bonded to one oxygen atom and then single-bonded with another. This leads to very high electronegativity centred on the C atom. The result: the electron theoretically shared between the O and the H atom is drawn much toward the O atom. From the outside, therefore, the H atom appears as an unshielded proton, which attracts the negative end of a polar solvent like water.<\/p>\n \nIn turn, the solvent molecules surround the H nucleus, their negative sides towards it, and pull it from the O. Said H nucleus, being just a proton, is the active ingredient of acidity in the context.<\/p>\n \nSource:<\/p>\n \nSolomons, T.W. Graham. Organic Chemistry,<\/em> fourth edition. Toronto: John Wiley & Sons, 1988.<\/p>\nJack of Oracle Tutoring by Jack and Diane,<\/a> Campbell River, BC.\n","protected":false},"excerpt":{"rendered":" Tutoring chemistry, concepts arise. The tutor mentions an idea behind the acidity of the carboxyl group. In my previous post I mention the carboxylic acid functional group. Yet, why is the carboxyl group acidic? The reason I’ve heard is that …<\/p>\n