Question

Question #4a20d

Answer 1

Start by looking at the neutral argon atom, this will give you an idea about how the electron configuration of the `Ar^(+)` ion will look like.

Argon is located in period 3, group 18 of the periodic table, and has an atomic number equal to 18. This means that a neutral argon atom will have 18 electrons surrounding its nucleus.

Since you're dealing with the `Ar^(+)` ion, which has one less electron than neutral argon, the number of electrons that surround its nucleus will be 17.

`"Ar"^(+): 1s^(2) 2s^(2) 2p^(6) 3s^(2) 3p^(5)`

Using the noble gas shorthand notation, this electron configuration will be

`"Ar"^(+): ["Ne"] 3s^(2) 3p^(5)`