Limited access

Upgrade to access all content for this subject

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 explains 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

$H_{2}O$ does not have the same type of intermolecular forces as the other molecules.

D

$H_{2}O$ is ionicly bonded while the others are covalently bonded.

Select an assignment template