Nickel Electron Configuration

Reference tool for nickel's electron configuration (1s² 2s² 2p⁶ 3s² 3p⁶ 3d⁸ 4s²), abbreviated as [Ar] 3d⁸ 4s², with orbital box diagram, quantum numbers, and element facts.

Z = 28 Ni Nickel

Nickel — Electron Configuration

Atomic number 28 · Transition metal · Period 4, Group 10 · d-block

[Ar] 3d⁸ 4s² 1s² 2s² 2p⁶ 3s² 3p⁶ 3d⁸ 4s² 28 electrons 10 valence e⁻ 2 unpaired e⁻

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 8 10 3d⁸
4s s orbital, shell n=4 2 2 4s²
Total 28

Full Configuration

1s² 2s² 2p⁶ 3s² 3p⁶ 3d⁸ 4s²

All subshells written explicitly.

Abbreviated (Noble-Gas)

[Ar] 3d⁸ 4s²

[Ar] = 1s² 2s² 2p⁶ 3s² 3p⁶ (18 electrons).

Valence Electrons

3d⁸ 4s² = 10 e⁻

Both 3d and 4s electrons participate in bonding.

Shell Fill Summary

Shell 1 (n=1) — 1s² 2 / 2 electrons (100%)
Shell 2 (n=2) — 2s² 2p⁶ 8 / 8 electrons (100%)
Shell 3 (n=3) — 3s² 3p⁶ 3d⁸ 16 / 18 electrons (89%)
Shell 4 (n=4) — 4s² 2 / 32 electrons (6%)

Shell 3 can hold 18 electrons (3s + 3p + 3d); nickel has 16. 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⁻
Cobalt (Co) 27 [Ar] 3d⁷ 4s² 3
Nickel (Ni) ← this element 28 [Ar] 3d⁸ 4s² 2
Copper (Cu) 29 [Ar] 3d¹⁰ 4s¹ 1
Zinc (Zn) 30 [Ar] 3d¹⁰ 4s² 0

Copper is anomalous: it promotes one 4s electron to 3d to achieve a fully filled 3d¹⁰ subshell, which is extra stable. Nickel has no such driving force and stays at 3d⁸ 4s².

Summary

Reference tool for nickel's electron configuration (1s² 2s² 2p⁶ 3s² 3p⁶ 3d⁸ 4s²), abbreviated as [Ar] 3d⁸ 4s², with orbital box diagram, quantum numbers, and element facts.

How it works

  1. The Aufbau principle fills subshells in order of increasing energy: 1s → 2s → 2p → 3s → 3p → 4s → 3d.
  2. The [Ar] core (1s² 2s² 2p⁶ 3s² 3p⁶) represents 18 electrons identical to the argon noble-gas configuration.
  3. 4s fills before 3d because 4s has slightly lower energy at lower atomic numbers.
  4. The 3d subshell receives 8 electrons: by Hund's rule, three orbitals are doubly occupied and two hold one electron each.
  5. Total electrons: 2 + 2 + 6 + 2 + 6 + 8 + 2 = 28, matching nickel's atomic number.
  6. Use the tabs below to explore the subshell table, orbital box diagram, and element properties.

Use cases

  • Quickly verify nickel's full or abbreviated configuration for homework and exams.
  • Understand why nickel has 2 unpaired 3d electrons and is paramagnetic.
  • Use the [Ar] 3d⁸ 4s² shorthand when writing configurations in inorganic chemistry.
  • Visualize which 3d orbitals carry paired vs. unpaired electrons per Hund's rule.
  • Compare nickel with neighboring transition metals cobalt (3d⁷ 4s²) and copper (3d¹⁰ 4s¹).
  • Teaching aid for Aufbau principle, Hund's rule, and d-block electron filling.

Frequently Asked Questions

Last updated: 2026-07-08 · Reviewed by Nham Vu