Question

part 2 (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. if formal charges are equal to zero, they should not be included. (this structure is a resonance form of the structure in part 1.)

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 of the neutral atom, $N$ is the number of non - bonding electrons, and $B$ is the number of bonding electrons.

Step2: Calculate formal charge of C

Carbon (C) has 4 valence electrons ($V = 4$). In the given Lewis structure, it has 2 non - bonding electrons ($N = 2$) and 4 bonding electrons ($B = 4$). Using the formula $FC = V - N-\frac{B}{2}$, we get $FC=4 - 2-\frac{4}{2}=4 - 2 - 2=0$.

Step3: Calculate formal charge of left - hand S

Sulfur (S) has 6 valence electrons ($V = 6$). In the given Lewis structure, it has 4 non - bonding electrons ($N = 4$) and 4 bonding electrons ($B = 4$). Using the formula $FC = V - N-\frac{B}{2}$, we get $FC = 6-4 - \frac{4}{2}=6 - 4 - 2=0$.

Step4: Calculate formal charge of right - hand S

Sulfur (S) has 6 valence electrons ($V = 6$). In the given Lewis structure, it has 4 non - bonding electrons ($N = 4$) and 4 bonding electrons ($B = 4$). Using the formula $FC = V - N-\frac{B}{2}$, we get $FC=6 - 4-\frac{4}{2}=6 - 4 - 2=0$.

Answer:

No non - zero formal charges to add.