Which one of the following general electronic configurations correctly represent a transition metal element?

The general electronic configuration of transition metal elements is represented as (n – 1) d1–10 ns0–2. Transition metals are located in the d-block of the periodic table, specifically groups 3 to 12. The notation (n – 1) signifies that the d-subshell being filled belongs to an energy level one lower than the outermost valence shell (n). The d-orbital can accommodate between 1 and 10 electrons, while the outermost s-orbital typically contains 0 to 2 electrons. While IUPAC defines a transition element specifically as one with an incomplete d-subshell in its neutral or ionic state, the general d-block formula (n – 1) d1–10 ns0–2 is the standard representation for these elements. Other options represent f-block elements or main group configurations.