[eRReR]

I'm a bit confused about certain electron configurations. If, for example, I want to write the electron configuration for Ti3+, it would be 1s^2 2s^2 2p^6 3s^2 3p^6 3d^1, or [Ar]3d^1, because, due to the movement of the energy levels, 4s is slightly higher than 3d so the 4s electrons are removed first.

This is my question: what is the electron configuration for Ti+? I know that titanium doesn't want to form a 1+ ion, so it's really a theoretical question. Should I remove the 4s electron and have [Ar]4s^1 3d^2? I can't remember where I read this, but I read that transition metal ions do not have s-electrons and, therefore, the electrons will shuffle around to give [Ar]3d^3. Which is right? Thanks in advance!

[Schrödinger]

First, you remove the electrons from the s orbital. Later they shuffle, because 3d³ is stable in an octahedral field. (Half filled t_2g level)

[eRReR]

Thank you for your *delete me*

[jens825]

The thing that your missing is that transition metals LOSE THEIR S ELECTRONS FIRST. All Transition metals start off with two s electrons, in this case, Ti⁺, it only loses one electron, so it will still have 1 s electron