Question

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.

Explanation:

Step1: Recall formal - charge formula

The formal - charge formula 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: Calculate formal charge of carbon

Carbon (C) has 4 valence electrons ($V = 4$). In the $C = S = S$ structure, carbon has 0 non - bonding electrons ($N = 0$) and 8 bonding electrons ($B = 8$). Using the formula $FC_C=4 - 0-\frac{8}{2}=4 - 4 = 0$.

Step3: Calculate formal charge of the first sulfur

Sulfur (S) has 6 valence electrons ($V = 6$). The first sulfur (connected to C) has 4 non - bonding electrons ($N = 4$) and 4 bonding electrons ($B = 4$). Using the formula $FC_{S1}=6 - 4-\frac{4}{2}=6 - 4 - 2=0$.

Step4: Calculate formal charge of the second sulfur

The second sulfur also has 6 valence electrons ($V = 6$). It has 4 non - bonding electrons ($N = 4$) and 4 bonding electrons ($B = 4$). Using the formula $FC_{S2}=6 - 4-\frac{4}{2}=6 - 4 - 2 = 0$.

Answer:

No non - zero formal charges need to be added.