What is the electron configuration for #"Al"^(3+)#?

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Aug 4, 2016

Answer:

#"Al"^(3+): 1s^2 2s^2 2p^6#

Explanation:

Your starting point here will be the electron configuration of a neutral aluminium atom, #"Al"#.

Aluminium is located in period 3, group 13, and has an atomic number equal to #13#. This tells you that the electron configuration of a neutral aluminium atom must account for a total of #13# electrons.

The electron configuration of the neutral atom looks like this

#"Al: " 1s^2 2s^2 2p^6 3s^2 3p^1#

Now, when aluminium forms #3+# cations, #"Al"^(3+)#, it loses #3# electrons from its outermost energy shell.

In this case, the #3# electrons will come from the third energy shell. To be precise, these electrons will come from

  • one 3p orbital #-> "1 e"^(-)#
  • the 3s orbital #-> "2 e"^(-)#

This means that the electron configuration of the aluminium cation looks like this

#color(green)(|bar(ul(color(white)(a/a)color(black)("Al"^(3+): 1s^2 2s^2 2p^6)color(white)(a/a)|)))#

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