# What is the electron configuration for a phosphorous anion with a charge of #-2#?

##### 1 Answer

#### Explanation:

Your starting point here will be the electron configuration of a *neutral* phosphorus atom.

Phosphorus, *neutral* phosphorus atom will have

Therefore, the electron configuration of a neutral phosphorus atom will show

#"P: " 1.2^2 2s^2 2p^6 3s^2 3p^3#

Now, in order for the phosphorus atom to become a *phosphorus anion*, it must **gain** two electrons. Since the **3p-subshell** only holds

Therefore, the electron configuration of the

#"P"^(2-): 1s^2 2s^2 2p^6 3s^2 3p^5#

Using the noble gas shorthand notation, you will get

#"P"^(2-): ["Ne"] 3s^2 3p^5#