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What is the hybridization of the central atom in [tex]$SO_2$[/tex]?

a) [tex]sp[/tex]
b) [tex]sp^2[/tex]
c) [tex]sp^3d[/tex]
d) [tex]sp^3d^2[/tex]
e) [tex]sp^3[/tex]

Sagot :

GinnyAnsweridn
To determine the hybridization of the central atom in \( \text{SO}_2 \), let's analyze the molecule step-by-step.

1. Identify the central atom: In \( \text{SO}_2 \), the central atom is sulfur (S).

2. Count the number of valence electrons:
- Sulfur has 6 valence electrons.
- Each oxygen atom has 6 valence electrons (2 oxygens contribute \( 6 \times 2 = 12 \) electrons).

3. Determine the bonding and lone pairs around the central atom:
- In \( \text{SO}_2 \), sulfur forms a double bond with each oxygen atom.
- Sulfur has one lone pair of electrons remaining.

4. Calculate the steric number (the number of regions of electron density):
- Sulfur has 2 double bonds + 1 lone pair = 3 regions of electron density.

5. Determine the hybridization based on the steric number:
- A steric number of 3 corresponds to \( sp^2 \) hybridization.

Therefore, the hybridization of the central atom in \( \text{SO}_2 \) is \( sp^2 \).

So, the correct answer is:
b) [tex]\( sp^2 \)[/tex]
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