Question

what is the formal charge for the s in the following compound? h h—c—s—h h a) +1 b) 0 c) +2 d) -2 e) -1

Explanation:

Step1: Recall formal - charge formula

Formal charge = Valence electrons - Non - bonding electrons - $\frac{1}{2}$Bonding electrons

Step2: Determine S valence electrons

Sulfur (S) is in Group 16 of the periodic table, so it has 6 valence electrons.

Step3: Count non - bonding and bonding electrons

In the given structure, S has 4 non - bonding electrons (2 lone pairs) and 4 bonding electrons (2 single bonds).

Step4: Calculate formal charge

Formal charge of S = 6 - 4-$\frac{4}{2}$ = 6 - 4 - 2=0

Answer:

B. 0