Among the following, the CORRECT combinations are

A. $\mathrm{IF}_3 \rightarrow \mathrm{~T}$-shaped ( $\mathrm{sp}^3 \mathrm{~d}$ )

B. $\mathrm{IF}_5 \rightarrow$ Square pyramidal $\left(\mathrm{sp}^3 \mathrm{~d}^2\right)$

C. $\mathrm{IF}_7 \rightarrow$ Pentagonal bipyramidal $\left(\mathrm{sp}^3 \mathrm{~d}^3\right)$

D. $\mathrm{ClO}_4{ }^{-} \rightarrow$ Square planar ( $\mathrm{sp}^2 \mathrm{~d}$ )

Choose the correct answer from the options given below:

Which statements are NOT TRUE about $\mathrm{XeO}_2 \mathrm{~F}_2$?

A. It has a see-saw shape.

B. Xe has 5 electron pairs in its valence shell in $\mathrm{XeO}_2 \mathrm{~F}_2$.

C. The $\mathrm{O}-\mathrm{Xe}-\mathrm{O}$ bond angle is close to $180^{\circ}$.

D. The $\mathrm{F}-\mathrm{Xe}-\mathrm{F}$ bond angle is close to $180^{\circ}$.

E. Xe has 16 valence electrons in $\mathrm{XeO}_2 \mathrm{~F}_2$.

Choose the correct answer from the options given below :

Identify the molecule $(X)$ with maximum number of lone pairs of electrons (obtained using Lewis dot structure) among $\mathrm{HNO}_3, \mathrm{H}_2 \mathrm{SO}_4, \mathrm{NF}_3$ and $\mathrm{O}_3$. Choose the correct bond angle made by the central atom of the molecule $(X)$.

Among $\mathrm{H}_2 \mathrm{~S}, \mathrm{H}_2 \mathrm{O}, \mathrm{NF}_3, \mathrm{NH}_3$ and $\mathrm{CHCl}_3$, identify the molecule $(\mathrm{X})$ with lowest dipole moment value. The number of lone pairs of electrons present on the central atom of the molecule $(X)$ is :