The carbon-oxygen bond in phenol is slightly stronger than that in methanol. Why?
(N/A) In phenol,the lone pair of electrons on the oxygen atom is involved in resonance with the benzene ring.
This resonance gives the $C-O$ bond a partial double bond character.
In contrast,there is no such resonance in methanol,where the $C-O$ bond is a pure single bond.
Additionally,the carbon atom attached to oxygen in phenol is $sp^2$ hybridized,while in methanol,it is $sp^3$ hybridized.
The $sp^2$ hybridized carbon is more electronegative and holds the electron pair more tightly,contributing to a shorter and stronger bond compared to the $sp^3$ hybridized carbon in methanol.
This resonance gives the $C-O$ bond a partial double bond character.
In contrast,there is no such resonance in methanol,where the $C-O$ bond is a pure single bond.
Additionally,the carbon atom attached to oxygen in phenol is $sp^2$ hybridized,while in methanol,it is $sp^3$ hybridized.
The $sp^2$ hybridized carbon is more electronegative and holds the electron pair more tightly,contributing to a shorter and stronger bond compared to the $sp^3$ hybridized carbon in methanol.
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