State reasons to explain why covalent compounds:
$(i)$ are bad conductors of electricity?
$(ii)$ have low melting and boiling points?
$(i)$ are bad conductors of electricity?
$(ii)$ have low melting and boiling points?
(N/A) $(i)$ Covalent compounds are bad conductors of electricity because the bonding in these compounds does not give rise to any charged ions.
$(ii)$ Covalently bonded molecules have strong covalent bonds within the molecule,but the intermolecular forces of attraction between the molecules are very weak,which results in low melting and boiling points.
$(ii)$ Covalently bonded molecules have strong covalent bonds within the molecule,but the intermolecular forces of attraction between the molecules are very weak,which results in low melting and boiling points.
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