Answer:
Both \[N{{H}_{3}}\] and \[P{{H}_{3}}\] are the hydrides of nitrogen and phosphorus which are present in group 15. Nitrogen is more electronegative (3.0) as compared phosphorus (2.1).
As a result, the shared electron pairs lie closer to the nitrogen atom in \[N{{H}_{3}}\] than to the phosphorus atom in \[P{{H}_{3}}\]. Therefore, the electron density around the nitrogen atom is more than around the phosphorus atom. This results in greater repulsion in the electron pairs around nitrogen atom than around phosphorus atom. As a result, bond angle in\[N{{H}_{3}}\] is more than in\[P{{H}_{3}}\].
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