Zinc Electron Configuration
Reference tool for zinc's electron configuration (1s² 2s² 2p⁶ 3s² 3p⁶ 3d¹⁰ 4s²), abbreviated as [Ar] 3d¹⁰ 4s², with orbital box diagram, subshell table, and element facts.
Zinc — Electron Configuration
Atomic number 30 · d-block metal · Period 4, Group 12 · Post-transition metal
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 | 10 | 10 | 3d¹⁰ |
| 4s | s orbital, shell n=4 | 2 | 2 | 4s² |
| Total | 30 | |||
Full Configuration
1s² 2s² 2p⁶ 3s² 3p⁶ 3d¹⁰ 4s²
All subshells written explicitly.
Abbreviated (Noble-Gas)
[Ar] 3d¹⁰ 4s²
[Ar] = 1s² 2s² 2p⁶ 3s² 3p⁶ (18 electrons).
Valence Electrons
4s² = 2 e⁻
Only 4s electrons participate in bonding; 3d¹⁰ is inert.
Shell Fill Summary
Shells 1–3 are completely filled in zinc. Shell 4 only has 4s filled; the 4p, 4d, and 4f subshells are empty at ground state.
Period 4 d-Block Neighbors
| Element | Z | Configuration | Unpaired e⁻ | Follows Aufbau? |
|---|---|---|---|---|
| Nickel (Ni) | 28 | [Ar] 3d⁸ 4s² | 2 | Yes |
| Copper (Cu) | 29 | [Ar] 3d¹⁰ 4s¹ | 1 | No (anomaly) |
| Zinc (Zn) ← this element | 30 | [Ar] 3d¹⁰ 4s² | 0 | Yes |
| Gallium (Ga) | 31 | [Ar] 3d¹⁰ 4s² 4p¹ | 1 | Yes |
Copper (Z=29) is anomalous: it promotes one 4s electron to 3d to achieve a fully filled 3d¹⁰ subshell, which is extra stable. Zinc (Z=30) already achieves 3d¹⁰ with a normal Aufbau fill, so no such promotion is needed.
Why Zinc's Configuration is Straightforward
Zinc sits one position past copper in the periodic table. While copper needs an anomalous 4s→3d promotion to reach the stable 3d¹⁰ 4s¹ state, zinc naturally arrives at 3d¹⁰ 4s² by normal Aufbau filling — no exception required.
The completely filled 3d¹⁰ subshell means all five d orbitals hold paired electrons. There are no unpaired electrons, so zinc is diamagnetic. It is also the reason zinc does not display variable oxidation states: with 3d fully paired, removing d electrons is energetically costly, leaving Zn²⁺ (losing both 4s electrons) as the only common ion.
Because zinc's 3d¹⁰ subshell is never partially filled in any stable oxidation state, the IUPAC debate classifies zinc as a post-transition metal rather than a true transition metal, even though it sits in the d-block.
Summary
Reference tool for zinc's electron configuration (1s² 2s² 2p⁶ 3s² 3p⁶ 3d¹⁰ 4s²), abbreviated as [Ar] 3d¹⁰ 4s², with orbital box diagram, subshell table, and element facts.
How it works
- The Aufbau principle fills subshells in order of increasing energy: 1s → 2s → 2p → 3s → 3p → 4s → 3d.
- The [Ar] core (1s² 2s² 2p⁶ 3s² 3p⁶) represents 18 electrons identical to the argon noble-gas configuration.
- 4s fills before 3d because 4s has slightly lower energy at lower atomic numbers.
- Zinc's 3d subshell receives all 10 electrons, achieving a completely filled 3d¹⁰ state — no anomaly needed (contrast with copper).
- Total electrons: 2 + 2 + 6 + 2 + 6 + 10 + 2 = 30, matching zinc's atomic number.
- Use the tabs below to explore the subshell table, orbital box diagram, and element properties.
Use cases
- Quickly verify zinc's full or abbreviated configuration for homework and exams.
- Understand why zinc has no unpaired electrons and is diamagnetic.
- Use the [Ar] 3d¹⁰ 4s² shorthand when writing configurations in inorganic chemistry.
- Compare zinc with neighboring copper (anomalous 3d¹⁰ 4s¹) and nickel (3d⁸ 4s²).
- Visualize that all five 3d orbitals are doubly occupied (completely filled).
- Teaching aid for Aufbau principle, completed d-subshells, and post-transition metal behavior.