Carbon and sulfur form compounds with each other with the formulas \(\mathrm{CS}_{2}\) and \(\mathrm{C}_{3} \mathrm{S}_{2}\) . Draw a Lewis structure for each compound that has a formal charge of zero for all atoms in the structure.

First, we need to find the total number of valence electrons for each compound. Carbon (C) has 4 valence electrons and sulfur (S) has 6 valence electrons. For CS₂: There is 1 carbon atom and 2 sulfur atoms in the molecule, so the total number of valence electrons is: (1 x 4) + (2 x 6) = 4 + 12 = 16. For C₃S₂: There are 3 carbon atoms and 2 sulfur atoms in the molecule, so the total number of valence electrons is: (3 x 4) + (2 x 6) = 12 + 12 = 24.

We can start by placing Carbon (the central atom) in the center, surrounded by the two sulfur atoms. Then, we can distribute the 16 valence electrons to create a stable Lewis structure with the formal charge of zero for each atom. 1. Connect the central carbon atom to each sulfur atom using single bonds, using 2 electrons per bond (4 electrons total): S - C - S 2. Complete the octets for each sulfur atom by adding lone pairs of electrons: S: 6 - 2 = 4 remaining electrons (2 lone pairs) S - C - S: 16 - 4 = 12 remaining electrons 3. Distribute the remaining 12 electrons to complete the octets: :S - C - S: .. .. The formal charges for all atoms are zero, and we have reached a stable Lewis structure for CS₂.

For C₃S₂, we can start by placing the carbon atoms in the center with the two sulfur atoms bonded to the outermost carbons. Then, we can distribute the 24 valence electrons to create a stable Lewis structure with the formal charge of zero for each atom. 1. Connect the carbons and sulfurs using single bonds, using 2 electrons per bond (8 electrons total): S - C - C - C - S 2. Complete the octets for each sulfur atom by adding lone pairs of electrons: S: 6 - 2 = 4 remaining electrons (2 lone pairs) S - C - C - C - S: 24 - 8 = 16 remaining electrons 3. Distribute the remaining 16 electrons to complete the octets: :S - C - C - C - S: .. . . .. By connecting the central carbon atoms with double bonds, each atom attains a formal charge of zero. The final Lewis structure for C₃S₂ is: :S - C = C = C - S: .. .. We have now found Lewis structures for both CS₂ and C₃S₂, with the formal charge of zero for all atoms in the structure.