(a)
H2O is
sp3 hybridized, and oxygen atom has 2 bond pair and 2 lone pair. So the angle between two
O−H bond is
104.5∘ (b) In
H2S molecule, central atom
S is a 3rd period element and according to Dragos rule, when a 3 rd period or higher period element overlap with a small element whose electronegetivity is low then that over lapping cannot be a effective overlapping, because of higher size of 3rd or higher periods element and smaller size of low electronegative element.
Here in
H2S,H atom has very low electronegativity and smaller in size so it create more negative charge around sulphur(s) atom and size of
S−2 ion increases, because of this higher size difference efficiency overlapping is not possible. So, any hybridization do not happen in between
S and
H atom. Lone pair electrons of
S atom is present in the pure orbital like s,
px,py,pz and it look like this :
As we know the angle between and
py is
90∘, so bond angle is
90∘.
(c)
NH3 has
sp3 hybridization and
N atom has 3 bond pair and one lone pair so bond angle is
107∘ (d)
SO2 is
sp2 hybridized and bond angle is
117∘.