What is the formal charge on the sulphur atom | vedclass

Name: Exam Paper Generator | JEE NEET Paper Generator | Vedclass
Brand: Vedclass
Rating: 5 (35 reviews)

Question

(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

Vedclass · Accepted Answer

$0$

Vedclass · Answer

(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$.

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

Similar Questions

In the $BrF_3$ molecule,the equatorial lone pairs minimize which of the following?

The correct order of bond angle is

The shape of the $BF_3$ molecule is:

The correct statement regarding the number of lone pairs on the central atoms of the molecules $SF_4$,$CF_4$,and $XeF_4$ is:

Which of the following molecules has the smallest bond angle?

Vedclass Test Series

Exam Paper Generator

Online Exam Module