Transition Metals

Transition metal: an element whose atoms have incomplete d-sublevels or that can give rise to cations with incomplete d-sublevels

• d-orbitals that are not completely filled

They are found in the d-block of the periodic table.

Zinc is NOT considered to be a transition metal

Transition metals have variable oxidation states

Transition metals form complexes

Central transition metal ion is surrounded by ligands

Ligands have a lone pair of electrons. They can make co-ordinate covalent bonds with the transition metal ion

Together, the central ion and the ligands form a complex

Transition metal complexes are coloured

Ligands split d-orbitals (more on this tomorrow)

When light is shone on the complex, light of a particular wavelength is absorbed as an electron is promoted. The colour that we see is white light minus whatever colour is absorbed.

Transition metals are catalysts

Catalysts increases the rate of a reaction without being consumed in the process.

Transition metals exhibit magnetism

Magnetic strength depends on the number of unpaired electrons in the d-orbitals