What is the orbital diagram for Ti 2+?
I got 1s two arrows, 2s two arrows, 2p 6 arrows, 3s two arrows, 3p six arrows, 4s two arrows but it is wrong. It said ions of d-block metals typically lack the outermost s electrons that are present in their neutral counterparts.
You omitted the 3d electrons.
Ti neutral is
1s2 2s2 2p6 3s2 3p6 3d2 4s2
For the Ti^2+, remove the two 4s electrons (the outermost electrons)
So it is 1s2 2s2 2p6 3s2 3p6 3d2 but it said it is wrong.
What I wrote is correct. Ti is 22 electrons and Ti^2+ is 2 electrons arranged as I've shown.
The database may have wanted you to show the arrows in the boxes; if so that would be 1s2arrows 2s2arrows 2p6arrows
3s2arrows 3p6arrows 3d1arrow 3d1arrow since the two 3d2 electrons are not paired.
To determine the orbital diagram for Ti 2+, it is essential to consider the electron configuration of the neutral atom of titanium (Ti).
The electron configuration of neutral Ti is [Ar] 3d2 4s2. Given that Ti 2+ has a +2 charge, we need to remove two electrons from the neutral state.
To do this, we begin by removing electrons from the outermost shell first. In this case, the 4s orbital is the outermost, so we start by removing two electrons from the 4s subshell. This leaves us with [Ar] 3d2 for Ti 2+.
Therefore, the orbital diagram for Ti 2+ is:
[Ar] 3d2
Please note that the incorrect response you received mentioned that "ions of d-block metals typically lack the outermost s electrons that are present in their neutral counterparts." This statement is accurate. The removal of the 4s electrons in the ion state is a common pattern among d-block metals.