Write the condensed electron configuration for the manganese atom. When writing your answers, do not add spaces and do not try to italicize the orbitals. Mn and Mn3+
The correct Answer and Explanation is:
The condensed electron configuration for a manganese (Mn) atom is: [Ar]4s23d5
For the Mn³⁺ ion, the electron configuration is: [Ar]3d4
Explanation:
Manganese is a transition metal with atomic number 25, meaning it has 25 electrons when neutral. The electron configuration follows the order dictated by the Aufbau principle, which states that electrons fill orbitals from lowest to highest energy. The condensed configuration uses argon’s electron configuration ([Ar]) as a core to avoid listing all lower-energy orbitals explicitly.
Neutral Mn Atom:
Manganese has electrons in both the 4s and 3d orbitals. Despite 4s orbitals filling before 3d orbitals, transition metals like manganese often exhibit electron configurations influenced by stability considerations. In Mn, the 3d orbitals hold 5 electrons, a half-filled stable arrangement that minimizes electron repulsion.
Mn³⁺ Ion:
When Mn loses three electrons to form Mn³⁺, it follows the general rule that transition metals first lose electrons from their highest principal energy level (n=4). This means the 4s electrons are removed first, followed by one from the 3d orbital. Removing three electrons from Mn results in the configuration [Ar]3d4, meaning the 4s electrons are completely lost, leaving only the d-shell electrons.
The change in electron configuration significantly impacts manganese’s chemical behavior. Mn³⁺ is commonly found in coordination complexes and oxidation reactions, with its 3d⁴ electron configuration contributing to its role as a catalyst and in biological systems. Transition metals, including manganese, exhibit variable oxidation states due to their ability to lose different numbers of d-electrons, making them essential in many industrial and biochemical processes.
