(i)  Transition metals show paramagnetic behaviour. Paramagnetism arises due to the presence of unpaired electrons with each electron having a magnetic moment associated with its spin angular momentum and orbital angular momentum. However, in the first transition series, the orbital angular momentum is quenched. Therefore, the resulting
paramagnetism is only because of the unpaired electron.
(ii) Transition elements have high effective nuclear charge and a large number of
valence electrons. Therefore, they form very strong metallic bonds. As a result, the
enthalpy of atomization of transition metals is high.
(iii) Most of the complexes of transition metals are coloured. This is because of the
absorption of radiation from visible light region to promote an electron from one of the
d−orbitals to another. In the presence of ligands, the d-orbitals split up into two sets of
orbitals having different energies. Therefore, the transition of electrons can take place
from one set toanother. The energy required for these transitions is quite small and falls

in the visible region of radiation. The ions of transition metals absorb the radiation of a
particular wavelength and the rest is reflected, imparting colour to the solution.
(iv) The catalytic activity of the transition elements can be explained by two basic facts.
(a) Owing to their ability to show variable oxidation states and form complexes, transition
metals form unstable intermediate compounds. Thus, they provide a new path with lower activation energy, Ea, for the reaction.
(b) Transition metals also provide a suitable surface for the reactions to occur.