A) \[{{H}_{2}}O>Sb{{H}_{3}}>As{{H}_{3}}>P{{H}_{3}}>N{{H}_{3}}\]
B) \[{{H}_{2}}O>N{{H}_{3}}>Sb{{H}_{3}}>As{{H}_{3}}>P{{H}_{3}}\]
C) \[{{H}_{2}}O>Sb{{H}_{3}}>N{{H}_{3}}>As{{H}_{3}}>P{{H}_{3}}\]
D) \[{{H}_{2}}O>P{{H}_{3}}>As{{H}_{3}}>Sb{{H}_{3}}>N{{H}_{3}}\]
Correct Answer: C
Solution :
\[{{H}_{2}}O\] and \[N{{H}_{3}}\] have abnormally high boiling points because of their tendency to form hydrogen bonds. \[N{{H}_{3}}\] has higher boiling point than phosphine and then boiling point increases down the group because of increase in size. Hence, the order of boiling point will be \[{{H}_{2}}O>Sb{{H}_{3}}>N{{H}_{3}}>As{{H}_{3}}>P{{H}_{3}}\].
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