The molecular shapes of SF_4,CF_4,and XeF_4 a | vedclass

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(D) To determine the molecular shapes and lone pairs,we calculate the number of lone pairs on the central atom for each molecule:$1$. For $SF_4$: The

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Different with $1, 0$ and $2$ lone pairs of electrons on the central atom,respectively

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(D) To determine the molecular shapes and lone pairs,we calculate the number of lone pairs on the central atom for each molecule:$1$. For $SF_4$: The central atom $S$ has $6$ valence electrons. It forms $4$ bonds with $F$ atoms. Lone pairs = $(6 - 4) / 2 = 1$ lone pair. The shape is see-saw.$2$. For $CF_4$: The central atom $C$ has $4$ valence electrons. It forms $4$ bonds with $F$ atoms. Lone pairs = $(4 - 4) / 2 = 0$ lone pairs. The shape is tetrahedral.$3$. For $XeF_4$: The central atom $Xe$ has $8$ valence electrons. It forms $4$ bonds with $F$ atoms. Lone pairs = $(8 - 4) / 2 = 2$ lone pairs. The shape is square planar.Since the shapes and the number of lone pairs are different for all three,option $D$ is correct.

Column $I$	Column $II$
$(a) \ XeO_6^{4-}$	$(P)$ Tetrahedral
$(b) \ ClO_2$	$(Q) \ V\text{-shape}$
$(c) \ NH_4^+$	$(R)$ Trigonal Bipyramidal
$(d) \ XeO_3F_2$	$(S)$ Octahedral

The molecular shapes of $SF_4$,$CF_4$,and $XeF_4$ are

Similar Questions

In which of the following,are the molecules arranged in the increasing order of their bond angles?

In the molecule $I_2Cl_6$,choose the $CORRECT$ statement$(s)$.

In which of the following molecules,the maximum number of lone pairs is present on the central atom?

Match the column for molecular shape?

Column $I$ Column $II$

$(a) \ XeO_6^{4-}$ $(P)$ Tetrahedral

$(b) \ ClO_2$ $(Q) \ V\text{-shape}$

$(c) \ NH_4^+$ $(R)$ Trigonal Bipyramidal

$(d) \ XeO_3F_2$ $(S)$ Octahedral

What is the molecular shape of $BrF_3$?

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