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QUESTION

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

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

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

Phosphorus, "P", is located in period 3, group 15 of the , and has an equal to 15. This means that a neutral phosphorus atom will have 15 electrons surrounding its nucleus.

Therefore, the of a neutral phosphorus atom will show 15 electrons

"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 3 electrons in the neutral atom, these incoming electrons will be placed there.

Therefore, the electron configuration of the "P"^(2-) anion will be

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

Using the , you will get

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