What is the correct electron configuration for Zn 2+

Answer is [Ar] 4s^0 3d^10

From topscore. What is an easy way to figure this out I thought it was [Ar]4s^2 3d^8 but was wrong... What am I doing wrong? Thanks!

Your methods are right, but I believe in transition metals, ionization simply starts from the s orbitals

If possible, elements would rather have the d orbital full rather than the s. So for the element that ALMOST have 5 or 10 electrons in the d orbital, the s orbital will donate electrons in order to fully stabilize the d orbital.

What is the correct electron configuration for Zn 2+

Answer is [Ar] 4s^0 3d^10

From topscore. What is an easy way to figure this out I thought it was [Ar]4s^2 3d^8 but was wrong... What am I doing wrong? Thanks!

ask yourself this qustion? which orbital(s) fill up first, 4s or 3d?
the orbital(s) filling up first, will loose electron first.
Good luck

So p orbitals do this too? And only when the d or p shell is almost filled? If so what would be the cut off with the almost filled concept?

Thanks Guys!