In what way is the electronic configuration of the transition elements different from that of the non transition elements?
The electronic configuration of transition elements is characterized by partly filled d orbitals in their ground state or in their common oxidation states. This incomplete filling of orbitals distinguishes them from non-transition elements.
In contrast, non-transition elements have either completely filled d orbitals or no d orbital involvement in their valence shell. For instance, elements like zinc, cadmium, and mercury have the general electronic configuration with completely filled d orbitals in both their ground state and common oxidation states, and therefore are not regarded as transition elements.
The involvement of electrons in transition elements imparts distinct characteristics such as variable oxidation states, paramagnetic behaviour, catalytic properties, and formation of coloured ions and complexes.
Explanation
The textbook context clearly establishes that transition elements are defined by incompletely filled d orbitals. The context states: 'On the basis of incompletely filled 3d orbitals in case of scandium atom in its ground state (3d¹), it is regarded as a transition element.' Conversely, for zinc: 'zinc atom has completely filled d orbitals (3d¹⁰) in its ground state as well as in its oxidised state, hence it is not regarded as a transition element.' The key distinction is the presence of partially filled d orbitals in transition elements versus completely filled or absent d orbitals in non-transition elements.