Use valence bond theory to explain the bonding in\({{\rm{F}}_2},{\rm{HF}}\), and\({\rm{ClBr}}\). Sketch the overlap of the atomic orbitals involved in the bonds.

Bonds are formed by the overlapped valence orbitals on different atoms, according to the Valence Bond Theory. The orbitals that overlap must be occupied one at a time.

It is generally used to describe bonding in organic molecules like\({{\rm{H}}_{\rm{2}}}{\rm{,\;}}{{\rm{F}}_{\rm{2}}}{\rm{,HCl,ClBr}}\)etc.

\({{\rm{F}}_{\rm{2}}}\): The single\({\rm{F - F}}\)sigma bond form from the sidewise overlap of the 2 p orbital in\({\rm{F}}\)atom with the 2 p orbital of the other\({\rm{F}}\)atom.

\({\rm{HF}}\): The single H-F sigma bond form from the sidewise overlap of the 1 s orbital of H atom with the 2 p orbital of the other F atom.

ClBr: The single Cl-Br sigma bond is formed by the sidewise overlap of the Cl atom's 3 porbital with the other Br atom's 4 porbital.

Therefore, the sketch is given below: