How does the interaction of polar covalent bonds allow hydrogen bonds to form?

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How does the interaction of polar covalent bonds allow hydrogen bonds to form?

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Md Ariful Islam · Answer 1 · Apr 02, 2024 09:48:30

When hydrogen is bound to a strongly electronegative element, i.e. $O, N, F$, charge separation occurs as the heteroatom polarizes electron from the bond to acquire a partially negative charge. And of course if the charge is partially negative, there must be a partial positive charge developed on the hydrogen.

And thus a molecular dipole is generated, and in the bulk solution the dipoles line up to given an extra, potent intermolecular force that is known as $"hydrogen bonding"$.

For hydrogen fluoride, we could represent this interaction as $stackrel(delta+)H-stackrel(delta-)F$ $cdotsstackrel(delta+)H-stackrel(delta-)Fcdotsstackrel(delta+)H-$

And see this

And compare the boiling points of water, ammonia, and hydrogen fluoride with those of the lower group hydrides. The boiling points of these materials are absurdly high.

How does the interaction of polar covalent bonds allow hydrogen bonds to form?

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