The molecular shapes of SF_4, CF_4 and XeF_4 | vedclass

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(D) To determine the molecular shapes and lone pairs ($L$.$P$.) on the central atoms:$1$. For $SF_4$: The central atom $S$ has $6$ valence electrons.

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different with $1, 0$ and $2$ lone pairs of electrons on the central atoms, respectively

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(D) To determine the molecular shapes and lone pairs ($L$.$P$.) on the central atoms:$1$. For $SF_4$: The central atom $S$ has $6$ valence electrons. It forms $4$ bonds with $F$ atoms, leaving $1$ 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, leaving $0$ 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, leaving $2$ lone pairs. The shape is square planar.Thus, the shapes are different with $1, 0$ and $2$ lone pairs of electrons on the central atoms, respectively.

Molecule	Geometry
$(A)$ $XeF_2$	$1$. Trigonal pyramidal
$(B)$ $XeO_3$	$2$. Distorted octahedral
$(C)$ $XeF_6$	$3$. Linear
$(D)$ $XeOF_4$	$4$. Square pyramidal

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

Similar Questions

Match the following molecules with their respective geometries and choose the correct code.
Molecule Geometry
$(A)$ $XeF_2$ $1$. Trigonal pyramidal
$(B)$ $XeO_3$ $2$. Distorted octahedral
$(C)$ $XeF_6$ $3$. Linear
$(D)$ $XeOF_4$ $4$. Square pyramidal

Which of the following is the correct decreasing order of the repulsive interaction of electron pairs in a molecule?

Which of the following compounds have the same number of lone pairs on their central atom?
$I. XeF_5^- \quad II. BrF_3 \quad III. XeF_2 \quad IV. H_3S^{+} \quad V. CH_2$ (Methylene)

Which of the following statements is correct about $I^{+}_3$ and $I^{-}_3$ molecular ions?

The shape of a molecule of $NH_3$,in which the central atom contains a lone pair of electrons,is

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