Which of the following molecules has no lone | vedclass

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(B) The number of lone pairs on the central atom can be calculated using the formula: $	ext{Lone pairs} = \frac{1}{2} [V - B]$,where $V$ is the numbe

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$SF_6$

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(B) The number of lone pairs on the central atom can be calculated using the formula: $	ext{Lone pairs} = \frac{1}{2} [V - B]$,where $V$ is the number of valence electrons of the central atom and $B$ is the number of bonding electrons (or bonds formed). For $SF_6$: The central atom Sulfur $(S)$ has $6$ valence electrons and forms $6$ bonds with Fluorine atoms. $	ext{Lone pairs} = \frac{1}{2} [6 - 6] = 0$. For $SO_2$: Sulfur has $6$ valence electrons,forms $4$ bonds with Oxygen,leaving $1$ lone pair. For $NH_3$: Nitrogen has $5$ valence electrons,forms $3$ bonds with Hydrogen,leaving $1$ lone pair. For $SF_4$: Sulfur has $6$ valence electrons,forms $4$ bonds with Fluorine,leaving $1$ lone pair. Thus,$SF_6$ has no lone pair on the central atom.

List-$I$	List-$II$
$(A)$ $PCl_3$	$(I)$ Square planar
$(B)$ $BF_3$	$(II)$ $T$-shape
$(C)$ $ClF_3$	$(III)$ Trigonal pyramidal
$(D)$ $XeF_4$	$(IV)$ See-saw
	$(V)$ Trigonal planar

Which of the following molecules has no lone pair of electrons on the central atom?

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