Question

2nd attempt
part 1 (1 point)
add any nonzero formal charges to the atoms as applicable for the lewis structure shown with connectivity c - s - s. all valence electrons have been included, and this structure follows the octet rule. if formal charges are equal to zero, they should not be included.
c—s—s

Explanation:

Step1: Recall formal - charge formula

The formula for formal charge is $FC = V - N - \frac{B}{2}$, where $V$ is the number of valence electrons, $N$ is the number of non - bonding electrons, and $B$ is the number of bonding electrons.

Step2: Determine valence electrons of each atom

Carbon has 4 valence electrons ($V_C=4$), and sulfur has 6 valence electrons ($V_S = 6$).

Step3: Analyze bonding and non - bonding electrons in C - S - S structure

For the carbon atom in C - S - S: It has 4 bonding electrons ($B_C = 4$) and 0 non - bonding electrons ($N_C=0$). Using the formal - charge formula $FC_C=V_C - N_C-\frac{B_C}{2}=4 - 0-\frac{4}{2}=2$.
For the central sulfur atom: It has 4 bonding electrons ($B_{S1}=4$) and 4 non - bonding electrons ($N_{S1}=4$). Using the formula $FC_{S1}=V_S - N_{S1}-\frac{B_{S1}}{2}=6 - 4-\frac{4}{2}=0$.
For the terminal sulfur atom: It has 2 bonding electrons ($B_{S2}=2$) and 6 non - bonding electrons ($N_{S2}=6$). Using the formula $FC_{S2}=V_S - N_{S2}-\frac{B_{S2}}{2}=6 - 6-\frac{2}{2}=- 1$.

Answer:

Carbon has a formal charge of + 2, and the terminal sulfur has a formal charge of - 1.