Question

What is the total number of p electrons in a single phosphorus atom in its ground state?
A. 3
B. 5
C. 9
D. 15

Answer 1

Phosphorus is a p-block element. Because the last electron enters in the p-orbital. Velocity is calculated by total numbers of electrons and is calculated by counting numbers of unpaired electrons present in orbitals.

Complete step by step answer:
Phosphorus element belongs to group 15
Atomic number of phosphorus is 15
Its electronic configuration is 2, 8, 5 or $1{s^2},{\text{ }}2{s^2},{\text{ }}2{p^6},{\text{ }}3{s^2},{\text{ }}3{p^3}$
If this configuration is represented in the form of box, we have

Here, we see that the total number of electrons in s-orbital is 9
2p orbital has 6 electrons and 3p orbital has 3 electrons.
Therefore, total electrons are $6 + 3 = 9$electrons.
Electron filling takes place in an orbital according to aufbau principle. Electrons occupy the orbitals according to increasing energy levels. Energy level of 1s orbital is least so electrons enter in 1s orbital first. Energy level of orbitals is as follows.
1s < 2s < 2p < 3s < 3p < 4s < 3d < 4p > 5s and so on
It also obeys Hund’s rule of maximum multiplicity.
According to this rule electron pairing in p, d and f orbitals cannot occur until each orbital of given subshell contains one electron each or singly occupied subshell in p, d and f are as follows

Note:
White filling electrons in orbitals should obey aufbau principle and Hund’s rule of maximum multiplicity while counting no of electrons in different orbitals. Be careful to note that 4s is filled before 3d.