Based on differences in electronegativity, how would you characterize the bonding in sulfur dioxide, SO2? Essay answers are limited to about 500 words (3800 characters maximum, including spaces). 3800 Character(s) remaining 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 .