Question

How many single covalent bonds must a phosphorus atom form to have a complete octet in its valence shell? how many single covalent bonds must a phosphorus atom form to have a complete octet in its valence shell? 3 1 4 0 2?

Answer 1

Phosphorus   atom require to  form    3  single  covalent  bond  to  have  a  complete  octet  in  its  valence  shell.   Phosphorus  has  a  electron  configuration  2.8.5  hence  require  to  gain  three electrons  to  acquire  the octet  electron  configuration that  is an  electron  configuration  of  2.8.8.

Answer 2

Answer: Option (a) is the correct answer.

Explanation:

Atomic number of phosphorous is 15 and its electronic configuration is $[Ne]3s^{2}3p^{3}$.

As there are 3 valence electrons in a single phosphorous atom. Therefore, to attain stability it will readily lose three electrons and thus forms a $P^{3+}$ charge.

For example, in $PCl_{3}$ there will be sharing of electrons between the phosphorous and chlorine atom.

Hence, a phosphorous atom can share its three valence electrons and thus forms three covalent bonds to have a complete octet in its valence shell.