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

Answer: Option (a) is the correct answer.

Step-by-step 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.

Answer 2

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.