Why is zinc not considered a transition metal?
The electron configuration of zinc is [Ar]4s23d10. The only oxidative state which zinc has is Zn2+ in which its configuration is [Ar] (4s0)3d10, as the 4s sub-level empties first. The definition of a transition metal is that it must have an incomplete d sub-level in one or more of is oxidation states. As zinc has a complete d sub level at all oxidative states it can't be considered a transition metal.
NS
Related Chemistry IB answers
All answers ▸Define three element properties and explain how they change across the periodic table.
I don't understand how to calculate initial rates of reaction based on experimental data
Explain why successive ionization energies of an element increase and how they account for the existence of three main energy levels in the sodium atom
What is a difference between gas and liquid and solid on a molecular level?