Consider the following molecules: (I) POF_3,( | vedclass

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(C) $1$. Analyze the structures:$(I)$ $POF_3$: $P$ is $sp^3$ hybridized ($4$ orbitals). $P$ has $1$ $d\pi - p\pi$ bond with $O$. $P$ has $0$ lone pair

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Number of $d\pi - p\pi$ bonds in the respective molecule: $(I)$ One $	o$ $(II)$ Two $	o$ $(III)$ Three

Vedclass · Answer

(C) $1$. Analyze the structures:$(I)$ $POF_3$: $P$ is $sp^3$ hybridized ($4$ orbitals). $P$ has $1$ $d\pi - p\pi$ bond with $O$. $P$ has $0$ lone pairs.$(II)$ $SOF_4$: $S$ is $sp^3d$ hybridized ($5$ orbitals). $S$ has $1$ $d\pi - p\pi$ bond with $O$. $S$ has $0$ lone pairs.$(III)$ $IOF_5$: $I$ is $sp^3d^2$ hybridized ($6$ orbitals). $I$ has $1$ $d\pi - p\pi$ bond with $O$. $I$ has $0$ lone pairs.$2$. Evaluate the options:- Option $(A)$: $d-$orbitals involved: $P$ $(3d^1)$,$S$ $(3d^1)$,$I$ $(5d^1)$. This is incorrect as the number of $d-$orbitals involved in $\pi$ bonding remains $1$ for all.- Option $(B)$: Hybridization orbitals: $4 	o 5 	o 6$ is correct $(sp^3, sp^3d, sp^3d^2)$.- Option $(C)$: Number of $d\pi - p\pi$ bonds: All have $1$ $d\pi - p\pi$ bond. The sequence $1 	o 2 	o 3$ is $NOT$ observed.- Option $(D)$: Lone pairs: All have $0$ lone pairs. This is observed.$3$. Since both $(A)$ and $(C)$ describe changes that are not observed,and $(C)$ is a more direct contradiction to the bonding pattern,$(C)$ is the intended answer.

Column-$I$	Column-$II$
$(P)$ $\underline PCl_5 \to PCl_3 + Cl_2$	$(i)$ Change in hybridisation
$(Q)$ $\underline SO_3 \to \underline SO_2 + \frac{1}{2}O_2$	$(ii)$ Change in bond angle
$(R)$ $\underline NH_3 + H^{+} \to \underline NH_4^+$	$(iii)$ Change in shape
$(S)$ $H_2\underline O + H^{+} \to H_3\underline O^{+}$	$(iv)$ Change in oxidation state

Consider the following molecules: $(I)$ $POF_3$,$(II)$ $SOF_4$,$(III)$ $IOF_5$. On moving from $(I)$ to $(III)$,which of the following changes is $NOT$ observed?

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