Question

Give reasons for the following:
(I) Transition metals exhibit catalytic properties.
(II) Transition metals have high melting points.
(III) Zn is a transition element, while Zn is not

Answer 1

(I) Reason: Transition metals exhibit catalytic properties due to their ability to exist in mul tiple oxidation states, which allows them to act as intermediaries in redox reactions. Their partially filled d-orbitals allow them to bond with reactants and facilitate reaction pathways, making them effective catalysts. Additionally, they provide surfaces for adsorption and reaction of molecules.
(II) Reason: Transition metals have high melting points due to the strong metallic bonding between atoms. The electrons in the d-orbitals are not fully localized and are instead delocal ized across the metal lattice, resulting in stronger bonds that require more energy to break, leading to high melting points. Additionally, the higher the number of unpaired electrons in the d-orbitals, the stronger the metallic bond.
(III) Reason: Zinc is not classified as a transition metal because it has a completely filled 3d10 subshell in its ground state. Transition metals are defined as elements that have an incomplete d-subshell in at least one of their oxidation states. Since zinc does not have an incomplete d-subshell, it does not qualify as a transition metal.