Draw the Lewis structures of S2^2- ions giving all the steps.

The Correct Answer and Explanation is:

To draw the Lewis structure of the S22−S_2^{2-}S22− ion (a di-sulfide anion with a charge of -2), we follow these steps:

Step 1: Determine the total number of valence electrons

Sulfur (S) is in group 16 of the periodic table, so each sulfur atom has 6 valence electrons. For the S22−S_2^{2-}S22− ion, the total number of electrons is: 6(from each sulfur)×2(atoms)+2(extra electrons from the -2 charge)=14 electrons6 (\text{from each sulfur}) \times 2 (\text{atoms}) + 2 (\text{extra electrons from the -2 charge}) = 14 \, \text{electrons}6(from each sulfur)×2(atoms)+2(extra electrons from the -2 charge)=14electrons

Step 2: Sketch the basic structure

Start by placing the two sulfur atoms next to each other, as they are bonded in the ion. Each sulfur atom will form a bond with the other sulfur atom.

Step 3: Distribute the electrons

Place a single bond (which consists of two electrons) between the two sulfur atoms.
This leaves 12 electrons (14 – 2 = 12) to be distributed as lone pairs around the atoms.

Step 4: Complete the octets

Give each sulfur atom 3 lone pairs of electrons (6 electrons per sulfur atom), which accounts for 12 electrons (6 electrons per sulfur × 2 atoms).
After placing the lone pairs, each sulfur atom will have 8 electrons, satisfying the octet rule.

Step 5: Check for formal charges

In the structure, each sulfur atom has 6 valence electrons in lone pairs and 2 electrons in the bond with the other sulfur. This means each sulfur atom has 7 electrons, which leads to a formal charge of -1 on each sulfur.
The total charge on the ion is -2, so the formal charges are correct.

Final structure:

The structure consists of a single bond between two sulfur atoms, each surrounded by 3 lone pairs. The overall charge of the ion is -2.

Lewis Structure:

ruby:S:S:

Each sulfur atom has three lone pairs of electrons, and there is a single bond between them, with the overall charge being -2.