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
Answered by Niall S. Chemistry tutor

37648 Views

See similar Chemistry IB tutors

Related Chemistry IB answers

All answers ▸

What is the limiting reagent and thus the mass of product for the reaction: P4O10 + 6H2O --> 4H3PO4 if 5.00 g of P4O10 react with 1.50 g of water?


How are Van der Waals interactions formed between molecules?


Explain which molecule has the highest boilng point HCL, water ot CH4?


Describe and compare three features of the structure and bonding in the three allotropes of carbon: diamond, graphite and C60 fullerene.


We're here to help

contact us iconContact usWhatsapp logoMessage us on Whatsapptelephone icon+44 (0) 203 773 6020
Facebook logoInstagram logoLinkedIn logo

© MyTutorWeb Ltd 2013–2025

Terms & Conditions|Privacy Policy
Cookie Preferences