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: Determine valence electrons of each atom

Carbon ($C$) has 4 valence electrons, sulfur ($S$) has 6 valence electrons.

Step3: Analyze bonding and non - bonding electrons for carbon

Assume a Lewis structure with single bonds. For carbon in $C - S - S$, if we consider the bonding and non - bonding electrons, let's assume the structure has the appropriate number of valence electrons distributed. If carbon has 2 single bonds (4 bonding electrons, $B = 4$) and 2 non - bonding electrons ($N=2$), then $FC_C=4 - 2-\frac{4}{2}=0$.

Step4: Analyze the first sulfur

Let the first sulfur (connected to carbon) have 2 single bonds ($B = 4$) and 4 non - bonding electrons ($N = 4$). Then $FC_{S1}=6 - 4-\frac{4}{2}=0$.

Step5: Analyze the second sulfur

The second sulfur has 1 single bond ($B = 2$) and 6 non - bonding electrons ($N = 6$). Then $FC_{S2}=6 - 6-\frac{2}{2}=- 1$.

Step6: Add formal charges

We add a negative 1 formal charge to the terminal sulfur atom.

Answer:

Add a negative 1 formal charge to the terminal sulfur atom.