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

Transition metals have a partially filled d−orbital. Therefore, the electronic configuration of transition elements is (n − 1)d^1-10 ns^0-2.

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 ns^1-2 or ns2 np1-6.

The general electronic configuration of a d-block elements is (n -1) d^1-10 ns^1-2.

Transition elements in its ground state or excited state will have a configuration of (n - 1) d^1-9 ns^0-2 ie. partly filled d orbitals whereas non transition elements will have a configuration of (n -1) d¹⁰ ns^0.2  i.e completely filled d- orbitals.

Transition elements have partially filled d-subshell belonging to penultimate energy level whereas non-transition elements do not have any partially filled d-subshell. In non-transition elements, the last electron enters the s or p-subshell whereas in transition elements the last electron enters the d-subshell of penultimate energy level.

Transition elements have partially filled d-subshell belonging to penultimate energy level whereas non-transition elements do not have any partially filled d- subshell. In non-transition elements, the last electron enters the s or p-subshell whereas in transition elements the last electron enters the d-subshell of penultimate energy level.