Question

The best Lewis structure for sulfuric acid has zero formal charges, sulfur as the central atom, and no bonds between S and H. How many single and double bonds, respectively, are there in this Lewis structure? 2 single, 4 double 6 single, 0 double 4 single, 2 double 4 single, 4 single 0 single, 4 double 4 single, 0 double 4 single, 4 double

Answer 1

Answer: In a lewis structure of sulfuric acid there are 4 single, 2 double bonds.

Explanation:

Chemical formula of sulfuric acid is $H_{2}SO_{4}$. So, there are two hydrogen atoms, one sulfur atom and four oxygen atoms.

It is known that formula to calculate formal charge is as follows.

             Formal charge = Valence electrons - nonbonding electrons -$\frac{\text{bonding}}{2}$

Hence, formal charge on each atom present in sulfuric acid whose structure is depicted in the picture will be as follows.

Formal charge on atom 1 = 1 - 0 - $\frac{2}{2}$ = 1 - 1 = 0

Formal charge on atom 2 = 6 - 4 - $\frac{4}{2}$ = 6 - 6 = 0

Formal charge on atom 3 = 6 - 4 - $\frac{4}{2}$ = 6 - 6 = 0

Formal charge on atom 4 = 6 - 0 - $\frac{12}{2}$ = 6 - 6 = 0

Formal charge on atom 5 = 6 - 4 - $\frac{4}{2}$ = 6 - 6 = 0

Formal charge on atom 6 = 6 - 4 - $\frac{4}{2}$ = 6 - 6 = 0

Formal charge on atom 7 = 1 - 0 - $\frac{2}{2}$ = 1 - 1 = 0

Therefore, total charge on a molecule of sulfuric acid is zero.

Hence, in total there are 4 single bonds and 2 double bonds present in a molecule of sulfuric acid.