Based on differences in electronegativity, how would you characterize the bonding in sulfur
dioxide, SO2?
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Solution
The atom with less electronegative is central atom and the atoms with more electronegtive are
terminal atoms.
So, Sulphur with less electronegative is central atom and Oxygens are terminal atoms.
S ( Z = 16 ) 1st excited state electronic configuration is,
1s2 s2 2p6 3s2 3p3 3d1
S in its first exicted state undergoes sp2 hybirdisation due ot which it has 1 paired sp2 hybrid
orbital and 2 unpaired sp2 hybrid orbitals. And also S has one p and one d orbital with unpaired
electrons.
O (Z = 8) E.C is 1s2 2s2 2p4
Each O has two unpaired electrons in its valence shell.
The each sp2 unpaired hybrid orbital of S overlaps with one of the unpaired p - orbital ofeach
oxygen along the internuclear axis to form single S - O sigma bond with each Oxygen.
The reamining unpaired pure p-orbitals of S overlaps with unpaired p - orbital of each oxygen
perpendicular to the internuclear axis to form one pi bonds with each oxygen.
Still S ia remained with one lone pair of electons.
Due to this SO 2 is in bent shape and has the bond angle < 120 0