Answer: The number of valence electrons that are non-bonding for sulfur atom are 2.
Explanation:
Valence electrons are defined as the electrons that are present in outermost shell of an atom.
Non-bonded electrons are defined as the electrons that do not participate in the bonding. The pair of these electrons are known as lone pairs. They are determined by lewis dot structure of compound.
To calculate the hybridization of SO_2, we use the equation:
[tex]\text{Number of electron pair}=\frac{1}{2}[V+N-C+A][/tex]
where,
V = number of valence electrons present in central atom (S) = 6
N = number of monovalent atoms bonded to central atom = 0
C = charge of cation = 0
A = charge of anion = 0
Putting values in above equation, we get:
[tex]\text{Number of electron pair}=\frac{1}{2}[6]=3[/tex]
The number of electron pair around the central metal atom are 3. This means that the hybridization will be [tex]sp^2[/tex]
The number of bonded electrons of the compound = 8
Number of non-bonded electrons around the central metal atom which is sulfur = 2
Hence, the number of valence electrons that are non-bonding for sulfur atom are 2.
