A) \[NC{{l}_{3}}\]
B) \[NB{{r}_{3}}\]
C) \[N{{H}_{3}}\]
D) \[N{{I}_{3}}\]
Correct Answer: C
Solution :
Electronegativity difference between \[N(3.0)\]and \[Cl\,(3.0)\] is zero and hence \[N-Cl\] bonds are non-polar. As a result, the overall dipole moment of \[NC{{l}_{3}}\] molecule and its direction is just the dipole moment of the lone pair of electrons. On the other hand,\[N-Br\,(3.0-2.8),\] \[N-I\,(3.0-2.5)\] and \[N-H\,(3.0-2.1)\] are polar and hence contribute towards the overall dipole moment of the respective molecules. Since the EN difference is highest in case of \[N-H\]bonds, therefore, \[N{{H}_{3}}\] has the highest dipole moment.You need to login to perform this action.
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