Question

draw the lewis structure for the disulfur monoxide (s₂o) molecule. be sure to include all resonance structures that satisfy the octet rule.

Explanation:

Step1: Calculate valence - electrons

S has 6 valence electrons and O has 6 valence electrons. For \(S_2O\), the total number of valence electrons is \(2\times6 + 6=18\).

Step2: Arrange atoms and form single bonds

Place the oxygen atom in the middle and connect it to the two sulfur atoms with single bonds (\(S - O - S\)). This uses 4 electrons, leaving \(18 - 4 = 14\) electrons.

Step3: Distribute remaining electrons as lone - pairs

Distribute the 14 remaining electrons as lone - pairs to satisfy the octet rule. Each S and O should have 8 electrons around them. We can have the following resonance structures:

• Structure 1: \(S=\ddot{O}=S\) with two double bonds and each atom has 2 lone - pairs.
• Structure 2: \(\overset{-}{S}-\overset{+}{O}\equiv S\) and its mirror image \(\overset{+}{S}\equiv\overset{-}{O}-S\)

Answer:

The resonance structures of \(S_2O\) are \(S=\ddot{O}=S\), \(\overset{-}{S}-\overset{+}{O}\equiv S\) and \(\overset{+}{S}\equiv\overset{-}{O}-S\)