Question

question 9 (1 point)
which compound is capable of hydrogen bonding with itself in the liquid state?
a) chcl₃
b) hcn
c) beh₂
d) ch₃oh
e) h₂co

Explanation:

Hydrogen bonding occurs when a hydrogen atom is bonded to a highly electronegative atom (such as N, O, or F). For a compound to hydrogen - bond with itself, it must have both a hydrogen atom bonded to an electronegative atom (to act as a hydrogen - bond donor) and a lone pair on an electronegative atom (to act as a hydrogen - bond acceptor).

• For \(CHCl_3\):

The hydrogen is bonded to carbon. Carbon is not as electronegative as N, O, or F. So, it cannot form hydrogen bonds with itself.

• For \(HCN\):

The hydrogen is bonded to carbon. Carbon is not as electronegative as N, O, or F. So, it cannot form hydrogen bonds with itself.

• For \(BeH_2\):

Beryllium is not electronegative. The hydrogen is bonded to beryllium, so it cannot form hydrogen bonds.

• For \(CH_3OH\) (methanol):

The hydrogen is bonded to oxygen (\(O - H\) group). Oxygen is highly electronegative. The oxygen also has lone pairs. So, \(CH_3OH\) can act as both a hydrogen - bond donor (\(O - H\) bond) and a hydrogen - bond acceptor (lone pairs on O).

• For \(H_2CO\) (formaldehyde):

The hydrogens are bonded to carbon. Carbon is not as electronegative as N, O, or F. So, it cannot form hydrogen bonds with itself.

Answer:

d) \(CH_3OH\)