Identify the set of molecules in which the ce | vedclass

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(A) To determine the number of lone pairs on the central atom,we use the formula: $	ext{Lone pair} = \frac{V - (M + C - A)}{2}$,where $V$ is the numb

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$BrF_5, SF_4, SnCl_2$

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(A) To determine the number of lone pairs on the central atom,we use the formula: $	ext{Lone pair} = \frac{V - (M + C - A)}{2}$,where $V$ is the number of valence electrons of the central atom,$M$ is the number of monovalent atoms,$C$ is the charge of the cation,and $A$ is the charge of the anion.MoleculeLone Pairs$BrF_5$$1$$SF_4$$1$$SnCl_2$$1$$XeF_4$$2$$NH_3$$1$$ClF_3$$2$Based on the calculation,the molecules $BrF_5$,$SF_4$,and $SnCl_2$ each contain exactly $1$ lone pair on the central atom.

Identify the set of molecules in which the central atom has only one lone pair of electrons in their valence shells.

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