Chemical Bonding - Result Question 63
####38. The hybridisation of sulphur in sulphur dioxide is $(1986,1 M)$
(a) $s p$
(b) $s p^{3}$
(c) $s p^{2}$
(d) $d s p^{2}$
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Solution:
- In $SO _2$, the Lewis-dot structure is
$$ O=\ddot{S}=O $$
Electron pairs at $S=2(\sigma$-bonds $)+1$ (lone-pair) $=3$ $s p^{2}$ hybridised.
NOTE
$\pi$-bonded electrons are not present in hybrid orbitals, therefore not counted in electron pairs. Rather $\pi$ bonds are formed by lateral overlapping of pure $p$-orbitals.
