Question

Molecular solids generally have low melting points and boiling points due to relatively weak intermolecular attractions that hold the molecules in their solid form.

Molecular Solid	Boiling Point ${(}^{\circ }C)$
$H_{2}Te$	$0$
$H_{2}Se$	$-50$
$H_{2}S$	$-75$
$H_{2}O$	$100$

Which of the following reasons explain why $H_{2}O$ does not appear to follow this fact?

• A. $H_{2}O$ is relatively small compared to the other molecules
• B. $H_{2}O$ is not a molecular solid
• C. $H_{2}O$ have hydrogen bonding
• D. $H_{2}O$ is ionicly bonded while the others are covalently bonded

Answer 1

The correct option is C $H_{2}O$ have hydrogen bonding

$H_{2}O$ is a polar molecular solid, still has a melting point of ${100}^{o}C$. This is due to the presence of hydrogen bonding between the water molecules which holds the water molecules very strongly due to which it has high melting point.