Question
Discuss the structure of sulfur dioxide.
✓
Answer
(i) $SO _2$ molecule has a bent V shaped structure with $S - O - S$ bond angle $119.5^{\circ}$ and bond dissoClation enthalpy is 297 $kJ mol { }^{-1}$.
(ii) Sulphur in $SO _2$ is $sp ^2$ hybridised forming three hybrid orbitals. Due to lone pair electrons, bond angle is reduced from $120^{\circ}$ to $119.5^{\circ}$.
(iii) In $SO _2$, each oxygen atom is bonded to sulphur by $\sigma$ and a $\pi$ bond.
(iv) a bond between S and O are formed by $sp ^2- p$ overlapping.
(v) One of $\pi$ bonds is formed by $p \pi-p \pi$ overlapping while other $n$ bond is formed by $p \pi-d \pi$ overlap.
(vi) Due to resonance both the bonds are identical having observed bond length $143$ pm due to resonance,
(ii) Sulphur in $SO _2$ is $sp ^2$ hybridised forming three hybrid orbitals. Due to lone pair electrons, bond angle is reduced from $120^{\circ}$ to $119.5^{\circ}$.
(iii) In $SO _2$, each oxygen atom is bonded to sulphur by $\sigma$ and a $\pi$ bond.
(iv) a bond between S and O are formed by $sp ^2- p$ overlapping.
(v) One of $\pi$ bonds is formed by $p \pi-p \pi$ overlapping while other $n$ bond is formed by $p \pi-d \pi$ overlap.
(vi) Due to resonance both the bonds are identical having observed bond length $143$ pm due to resonance,
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