1. For each of the following species write the lowest energy Lewis structure, indicate the formal charge and oxidation number of each atom, show the geometric structure and estimate the bond angles, indicate the σ hybridization about the central atom, and give the point group. a) XeO₃, b) XeOF₂, c) XeO₆^4-, d) KrF₂, e) SeF₄.

a)

formal charges: O, 0; Xe, 0.
oxidation numbers: O, -2; Xe, +6.
geometric structure: pyramidal, O-Xe-O angles ~108^o
Xe hybridization: sp³
point group: C_3v

b)

formal charges: O, 0; Xe, 0; F, 0.
oxidation numbers: O, -2; Xe, +4; F, -1.
geometric structure: bent-T, O-Xe-F angles ~89^o
Xe hybridization: dsp³
point group: C_2v

c)

formal charges: =O, 0; -O, -1; Xe, 0.
oxidation numbers: O, -2; Xe, +8.
geometric structure: octahedral, all O-Xe-O angles 90^o
Xe hybridization: d²sp³
point group: O_h

d)

formal charges: F, 0; Kr, 0.
oxidation numbers: F, -1; Kr, +2.
geometric structure: linear, F-Kr-F 180^o
Kr hybridization: dsp³
point group: D_∞h

e)

formal charges: F, 0; Se, 0.
oxidation numbers: F, -1; Se, +4.
geometric structure: see-saw, F-Se-F angles of ~118^o and ~88^o
Se hybridization: dsp³
point group: C_2v