Give the orbital configuration of the phosphorus (p) atom.

1s^22s^22p^63s^23p^3

Explanation:

Assuming that orbital configuration is the same as electron configuration this is the answer.

Explanation:

The Electronic Configuration of the elements is the arrangement of all electrons of an element in energy levels and sub-levels (orbitals).  

There are 7 energy levels, numbered from 1 to 7, and in which electrons are distributed, logically in order according to their energy level. Each level is divided into sub-levels. These sub-levels into which each level is divided can be up to 4, called: s, p, d, f. In the sub-level s there can only be a maximum of 2 electrons, in p there can be a maximum of 6 electrons, in the sub-level d 10 electrons and finally in the sub-level f there can be a maximum of 14 electrons.

In level 1 there is only one sub-level, which will be the s. In level 2 there are 2 sub-levels, the s and the p. At level 3 there are 3 sub-levels s, p and d. And at level 4 there are 4 sub-levels, the s, the p, the d and the f.

Aufbau's principle is a principle of atomic physics, which explains how electrons are accommodated in their orbits around the nucleus of the atom. This principle states that the filling of these orbitals occurs in increasing order of energy, that is, from the orbitals of lower energy to those of higher energy.

The simplest of the sub-levels is 1s. If you fill the 1s you can start filling the 2s. After the 2s sub-level is satisfied, the 2p can begin to fill and so on.  

The atomic number Z of the element represents the number of protons of the element, and in a neutral atom it also indicates the number of electrons.  

So, given that the atomic number of the phosphorus is 15, and everything that has been said before, it is possible to say that the electrons that it has in the orbitals will be placed as follows:

1s² 2s² 2p⁶ 3s² 3p³

Finally, the orbital configuration of the phosphorus atom (P) will be as the image shows.