Deduce the bond angle in ${\mathrm{CCl}}_4, {\mathrm{NH}}_3$ and ${\mathrm{CS}}_2$.

Deduce the hybridization state of the central atom in ${\mathrm{CCl}}_4, {\mathrm{NH}}_3$ and ${\mathrm{CS}}_2$.

Deduce the molecular polarity of ${\mathrm{CCl}}_4, {\mathrm{NH}}_3$ and ${\mathrm{CS}}_2$.

Deduce the electron-domain geometry of ${\left[{\mathrm{NO}}_3\right]}^{-}, {\left[{\mathrm{SiF}}_6\right]}^{2-}, {\left[{\mathrm{IF}}_4\right]}^{-}$ and ${\mathrm{SCl}}_4$.

Deduce the molecular geometry of ${\left[{\mathrm{NO}}_3\right]}^{-}, {\left[{\mathrm{SiF}}_6\right]}^{2-}, {\left[{\mathrm{IF}}_4\right]}^{-}$ and ${\mathrm{SCl}}_4$.

Deduce the bond angle(s) in ${\left[{\mathrm{NO}}_3\right]}^{-}, {\left[{\mathrm{SiF}}_6\right]}^{2-}, {\left[{\mathrm{IF}}_4\right]}^{-}$ and ${\mathrm{SCl}}_4$.

Draw an appropriate Lewis (electron dot) structure and calculate the formal charge on each atom in ${\left[{\mathrm{NO}}_3\right]}^{-}, {\left[{\mathrm{SiF}}_6\right]}^{2-}, {\left[{\mathrm{IF}}_4\right]}^{-}$, and ${\mathrm{SCl}}_4$.

The following reactions take place in the ozone layer by the absorption of ultraviolet light.

I ${\mathrm{O}}_3\to {\mathrm{O}}_2+{\mathrm{O}}^{\bullet }$
II ${\mathrm{O}}_2\to {\mathrm{O}}^{\bullet }+{\mathrm{O}}^{\bullet }$

State and explain, by reference to the bonding, which of the reactions, I or II, requires a shorter wavelength.