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.

$I. SnCl_2$	$II. BeF_2$
$III. SO_2$	$IV. NO_2^+$
$V. C_2H_2$

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

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