Question

In what way is the electronic configuration of the transition elements different from that of the non-transition elements?

Answer 1

The transition elements contain partially filled d-orbitals whereas non-transition elements have no d-orbitals or have completely filled d-orbitals.
The non-transition elements may have fully filled d- orbital ${d^{10}}$ or it may not have a d orbital.
Those elements which end up having zero unpaired electrons in d block series are known as non-transition elements.

Complete step by step answer:
Transition elements (also known as transition metals) are those elements that have d orbitals filled with electrons or it is partially filled. IUPAC defines transition elements as an element having a d subshell that is partially filled with electrons, or an element that can form stable cations with an incompletely filled d orbital.
The main difference in oxidation states, between transition elements and other elements is that oxidation states are known in which there is a single atom of the elements and one or more unpaired electrons.
Transition metals have a partially filled d-orbital. Therefore, the electronic configuration of transition series can be written as $(n - 1){d^{1 - 10}}n{s^{0 - 2}}$
As we know that the non-transition elements either do not have a d-orbital or have a fully filled d-orbital. Therefore, the electronic configuration of non-transition elements is
$n{s^{1 - 2}}$ or $n{s^2}n{p^{1 - 6}}$
The general valence shell configuration of s-block (group 1 and 2) elements is $n{s^{1 - 2}}$ and for p-block elements (group 13 to 18) $n{s^2}n{p^{1 - 6}}$.
The valence shell electronic configuration of transition elements can be written as $(n - 1){d^{1 - 9}}n{s^{1 - 2}}$.
In respective elements, the last shell is not completely filled and in transition elements, the last two shells are filled and are incomplete.

Note: The f-block elements that have incompletely filled f-orbitals are often referred to as inner transition elements or inner transition metals.
An electron from the ‘s’ orbital jumps into the d orbital in certain cases, to increase stability.