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!