Final answer:
The electron configuration of a transition element in the ground state is represented by the electron configuration notation, such as [Ar]3d6 4s² for iron (Fe). The 4s sublevel is filled before the 3d sublevel, but the outermost s electrons are the first to be removed in the process of forming transition metal ions. The given electron configuration [Ar]3d10 4s2 4p includes the 4p orbital, which is not part of the ground state electron configuration for a transition element.
Step-by-step explanation:
The electron configuration of a transition element in the ground state is represented by the electron configuration notation. For example, the electron configuration of iron (Fe) in the ground state is [Ar]3d6 4s². The notation [Ar] represents the electron configuration of argon, which is the preceding noble gas. The numbers 3d6 and 4s² represent the distribution of electrons in the d and s orbitals, respectively.
Transition elements are located in the d-block of the periodic table and have partially filled d orbitals. The electron configurations of transition elements follow a general pattern, where the 4s sublevel is filled before the 3d sublevel. However, in some cases, the 4s electrons are removed before the 3d electrons when forming transition metal ions.
It is important to note that the electron configuration of a transition element may vary depending on its oxidation state or ionization. The given electron configuration, [Ar]3d10 4s2 4p, does not match the ground state electron configuration of a transition element, as it includes the 4p orbital. The correct representation for a transition element in the ground state would be in the form of [Ar]3dX 4s2, where X represents the number of electrons in the d orbital.