Manganese Electron Configuration
Interactive reference for manganese's electron configuration (1s² 2s² 2p⁶ 3s² 3p⁶ 3d⁵ 4s²), orbital box diagram, quantum numbers, and key atomic properties.
Manganese — Electron Configuration
Atomic number 25 · Transition metal · Period 4, Group 7 · d-block
Subshell Breakdown
| Subshell | Type | Electrons | Max Capacity | Notation |
|---|---|---|---|---|
| 1s | s orbital, shell n=1 | 2 | 2 | 1s² |
| 2s | s orbital, shell n=2 | 2 | 2 | 2s² |
| 2p | p orbitals, shell n=2 | 6 | 6 | 2p⁶ |
| 3s | s orbital, shell n=3 | 2 | 2 | 3s² |
| 3p | p orbitals, shell n=3 | 6 | 6 | 3p⁶ |
| 3d | d orbitals, shell n=3 | 5 | 10 | 3d⁵ |
| 4s | s orbital, shell n=4 | 2 | 2 | 4s² |
| Total | 25 | |||
Full Configuration
1s² 2s² 2p⁶ 3s² 3p⁶ 3d⁵ 4s²
All subshells written explicitly.
Noble-Gas Shorthand
[Ar] 3d⁵ 4s²
[Ar] = 1s² 2s² 2p⁶ 3s² 3p⁶ (the filled argon core).
Why the Half-Filled 3d⁵ Matters
The 3d subshell in manganese holds exactly 5 electrons — one per orbital, all with parallel spins. This half-filled arrangement maximizes exchange energy, making it particularly stable. It explains manganese's wide range of oxidation states (+2 through +7) and its role in biological processes such as photosynthesis (Mn in Photosystem II).
Shell Fill Summary
Shell 3 can hold up to 18 electrons (3s + 3p + 3d). Manganese uses 13 of them. Shell 4 can hold 32; only 2 are used.
Summary
Interactive reference for manganese's electron configuration (1s² 2s² 2p⁶ 3s² 3p⁶ 3d⁵ 4s²), orbital box diagram, quantum numbers, and key atomic properties.
How it works
- The Aufbau principle fills orbitals from lowest to highest energy: 1s → 2s → 2p → 3s → 3p → 4s → 3d.
- After the argon core (1s² 2s² 2p⁶ 3s² 3p⁶), the 4s subshell fills first (before 3d) because it is lower in energy for Z=25.
- The 3d subshell then receives 5 electrons — exactly one per orbital — giving a half-filled 3d⁵ configuration.
- Hund's rule maximizes spin multiplicity: each of the five 3d electrons occupies a separate orbital with parallel (all spin-up) spins.
- The half-filled 3d⁵ is unusually stable, explaining manganese's chemistry and its multiple oxidation states.
- Noble-gas notation replaces the argon inner core with [Ar], leaving [Ar] 3d⁵ 4s² as the abbreviated form.
Use cases
- Quick reference for chemistry homework or exam review on transition metals.
- Understand why the 3d subshell is half-filled in manganese and what that means.
- Learn how the 3d⁵ 4s² configuration gives manganese 7 valence electrons and multiple oxidation states.
- Visualize orbital filling across the d-block using the interactive orbital diagram.
- Compare manganese to neighboring transition metals (chromium, iron) for periodic trend study.
- Teaching aid for Aufbau principle, Hund's rule, and d-block chemistry lessons.
- Verify quantum numbers for all 25 electrons of manganese.