Match each transition metal ion with its condensed ground-state electron configuration. Mn2+ [Ar]4s23d5 Hf2+ [Xe]4f145d2 Co3+ [Ar]3d6 Fe3+ [Ar]3d5 Ag+ [Kr]4d10 Mo3+ [Kr]4d15s2
The Correct Answer and Explanation is:
Here is the correct matching of each transition metal ion with its condensed ground-state electron configuration:
- Mn²⁺ → [Ar]3d⁵
- Hf²⁺ → [Xe]4f¹⁴5d²
- Co³⁺ → [Ar]3d⁶
- Fe³⁺ → [Ar]3d⁵
- Ag⁺ → [Kr]4d¹⁰
- Mo³⁺ → [Kr]4d³
Now for a detailed explanation:
Transition metals typically lose their outermost electrons starting with the 4s or 5s orbitals, then from the 3d or 4d subshells. When forming cations, the electrons are removed in the order of orbital energies, which places s-orbitals above d-orbitals in atomic configuration despite their opposite order during filling. This pattern governs the configurations for each ion.
Manganese (Mn²⁺) begins as [Ar]4s²3d⁵. Losing two electrons from 4s leaves [Ar]3d⁵, which is a half-filled, stable arrangement.
Hafnium (Hf²⁺) has the neutral configuration [Xe]6s²4f¹⁴5d². It loses both 6s electrons, yielding [Xe]4f¹⁴5d², a common oxidation state for Hf.
Cobalt (Co³⁺) starts from [Ar]4s²3d⁷. Removing two 4s and one 3d electron results in [Ar]3d⁶.
Iron (Fe³⁺) is initially [Ar]4s²3d⁶. After losing two 4s and one 3d electron, it becomes [Ar]3d⁵, which is especially stable due to half-filled d-orbitals.
Silver (Ag⁺) has the neutral form [Kr]5s¹4d¹⁰. It loses the 5s electron, resulting in the filled-shell configuration [Kr]4d¹⁰.
Molybdenum (Mo³⁺) in the ground state is [Kr]5s¹4d⁵. Upon removing the 5s¹ and two 4d electrons, it stabilizes at [Kr]4d³.
Recognizing these patterns helps to predict reactivity, bonding, and magnetic behavior of transition metals in coordination chemistry and catalysis.
