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(C) $I. XeF_5^-$: Central atom $Xe$ has $8$ valence electrons. It forms $5$ bonds with $F$ and has $1$ negative charge,total $9$ electrons. $5$ are us

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$I$ and $II$

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(C) $I. XeF_5^-$: Central atom $Xe$ has $8$ valence electrons. It forms $5$ bonds with $F$ and has $1$ negative charge,total $9$ electrons. $5$ are used in bonding,leaving $4$ electrons,which equals $2$ lone pairs.$II. BrF_3$: Central atom $Br$ has $7$ valence electrons. $3$ are used in bonding with $F$,leaving $4$ electrons,which equals $2$ lone pairs.$III. XeF_2$: Central atom $Xe$ has $8$ valence electrons. $2$ are used in bonding,leaving $6$ electrons,which equals $3$ lone pairs.$IV. H_3S^{+}$: Central atom $S$ has $6$ valence electrons. $3$ are used in bonding with $H$,and $1$ is lost due to positive charge,leaving $2$ electrons,which equals $1$ lone pair.$V. CH_2$: Central atom $C$ has $4$ valence electrons. $2$ are used in bonding with $H$,leaving $2$ non-bonding electrons (radical),which equals $0$ lone pairs.Thus,$XeF_5^-$ and $BrF_3$ both have $2$ lone pairs.

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)

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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)