What is the formal charge on the sulphur atom | vedclass

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(D) The formal charge is calculated using the formula: $	ext{Formal Charge} = V - L - \frac{1}{2}B$, where $V$ is the number of valence electrons, $L

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(D) The formal charge is calculated using the formula: $	ext{Formal Charge} = V - L - \frac{1}{2}B$, where $V$ is the number of valence electrons, $L$ is the number of lone pair electrons, and $B$ is the number of bonding electrons.For the sulphur atom in $H_2SO_4$:$1$. Valence electrons $(V)$ = $6$.$2$. Lone pair electrons $(L)$ = $0$ (all valence electrons are involved in bonding).$3$. Bonding electrons $(B)$ = $12$ (sulphur forms $6$ bonds: $2$ double bonds with oxygen atoms and $2$ single bonds with hydroxyl groups).$4$. $	ext{Formal Charge} = 6 - 0 - \frac{1}{2}(12) = 6 - 6 = 0$.

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

What is the formal charge on the sulphur atom in a sulphuric acid $(H_2SO_4)$ molecule?

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