Write Lewis structures for the following: (a) \({\rm{CI}}{{\rm{F}}_{\rm{3}}}\) (b) \({\rm{PC}}{{\rm{I}}_{\rm{5}}}\) (c) \({\rm{B}}{{\rm{F}}_{\rm{3}}}\) (d) \({\rm{P}}{{\rm{F}}_{\rm{6}}}^{\rm{ - }}\) .

A chemical bond is formed between atoms, ions, or molecules that allows formation of chemical compounds.

The following are the steps to drawing a Lewis structure:

(1) First, determine the total number of valence electrons, then deduct one electron for each positive charge if it is a cation, or add one electron for each negative charge if it is an anion.

(2) Now, arrange the atoms around the core atom to form a skeletal structure for the molecule. The least electronegative atom is typically chosen as the center atom. Connect each atom to the core atom with a single bond now.

(3) Now, on all atoms save the center atom, distribute the remaining electrons as lone pairs to complete their octet. (Except for hydrogen, which only takes two electrons to complete its duplet.)

(4) Now, arrange the remaining electrons around the central atom.

(5) Now, if any atom's octet is not full, draw several bonds with the central atom correspondingly.