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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 SolidBoiling Point (C)
H2Te0
H2Se50
H2S75
H2O100
Which of the following reasons explain why H2O does not appear to follow this fact?

A
H2O is relatively small compared to the other molecules
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B
H2O is not a molecular solid
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C
H2O have hydrogen bonding
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D
H2O is ionicly bonded while the others are covalently bonded
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Solution

The correct option is C H2O have hydrogen bonding
H2O is a polar molecular solid, still has a melting point of 100oC. 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.

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