A an excellent place come start when trying to figure out the electron construction of one ion is the electron construction of the neutral parental atom.

In this case, titanium, #"Ti"#, is located in period 4, team 4 the the regular table and has one atomic number of #22#.

This means that a neutral titanium atom will certainly contain #22# protons in the nucleus and also #22# electrons bordering its nucleus.

Therefore, the electron configuration of a neutral titanium atom should account for #22# electrons. Consequently, the electron construction of the titanium(II) cation, #"Ti"^(2+)#, need to account for #20# electrons, since this cation is developed when a neutral titanium atom loses #2# electrons.

The electron configuration of a neutral titanium atom looks choose this

#"Ti: " 1s^2 2s^2 2p^6 3s^2 3p^6 4s^2 3d^2#

Now, it"s important to store in mind the this notation because that the electron configuration is useful when adding electrons to build an atom "from scratch" since in the case, the #4s# orbital is to fill before the #3d# orbitals.

That happens because the empty #3d# orbitals are actually higher in power than the empty #4s# orbital, as watched here

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However, once the #4s# orbit is filled, it becomes higher in power than the #3d# orbitals.


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This way that once titanium loses electrons, the does therefore from the #4s# orbital first.

#"Ti: " 1s^2 2s^2 2p^6 3s^2 3p^6 3d^2 4s^2#

Therefore, the two electrons the are lost when the #"Ti"^(2+)# is created will come native the #4s# orbital, which method that the electron configuration of the cation is

#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 #<"Ar"># to represent the electron configuration of argon, the noble gas that comes automatically before titanium in the routine table.