# Why alcohols don't behave as acids?

If I understand everything correctly, carboxylic acids behave like acids because oxygen is much more electronegative than hydrogen, so it takes his electron and releases H+. The problem is that alcohols have an OH group too, so why don't they behave like acids?

• Although the answer is fine, there is still something weird when we got into inorganic acids. How would we justify that $\ce{HClO4}$ is so acid when it has no resonance structures (hibridisation is $sp^3$)? – santimirandarp Oct 12 '18 at 16:01
• @santimirandarp The $\ce{ClO4}$ anion is highly resonance stabilized (just google for drawings). This enhanced stability of the perchlorate anion explains why the acid is so highly ionized. – ron Oct 15 '18 at 19:46
• There is no resonance without using $d$ orbitals. That's my point.. – santimirandarp Oct 15 '18 at 19:47
• @santimirandarp Sorry, perhaps I'm not following you. You asked why $\ce{HClO4}$ is so acidic and I said because of resonance stabilization of the perchlorate anion. Hybridization $\ce{sp^3}$ for chlorine is OK, no need for d-orbitals. – ron Oct 15 '18 at 20:02
• No problem. Perchlorate anion has four simple bonds, so it is $sp^3$ and all oxygens are with same partial charge $-1$ there is no resonance...just one structure. Am I wrong? If we say there is a double bond, the only way possible is by means of $d$ orbitals... – santimirandarp Oct 15 '18 at 20:06