What is the electron configuration of #"Ti"^(2+)#?
1 Answer
Explanation:
A good place to start when trying to figure out the electron configuration of an ion is the electron configuration of the neutral parent atom.
In this case, titanium,
This means that a neutral titanium atom will contain
Therefore, the electron configuration of a neutral titanium atom must account for
The electron configuration of a neutral titanium atom looks like this
#"Ti: " 1s^2 2s^2 2p^6 3s^2 3p^6 4s^2 3d^2#
Now, it's important to keep in mind that this notation for the electron configuration is useful when adding electrons to build an atom "from scratch" because in that case, the
That happens because the empty
However, once the
#"Ti: " 1s^2 2s^2 2p^6 3s^2 3p^6 3d^2 4s^2#
Therefore, the two electrons that are lost when the
#color(green)(|bar(ul(color(white)(a/a)color(black)("Ti"^(2+): 1s^2 2s^2 2p^6 3s^2 3p^6 3d^2)color(white)(a/a)|)))#
If you want, you can use the noble gas shorthand notation to write
#color(green)(|bar(ul(color(white)(a/a)color(black)("Ti"^(2+): ["Ar"] 3d^2)color(white)(a/a)|)))#
Here