Tin Electron Configuration

Reference for tin's electron configuration ([Kr] 4d¹⁰ 5s² 5p²), orbital box diagram, valence electrons, and key atomic data for Sn (Z=50).

Z = 50 Sn Tin

Tin — Electron Configuration

Atomic number 50 · Post-transition metal · Period 5, Group 14 · p-block

1s² 2s² 2p⁶ 3s² 3p⁶ 3d¹⁰ 4s² 4p⁶ 4d¹⁰ 5s² 5p² [Kr] 4d¹⁰ 5s² 5p² 50 electrons 4 valence e⁻ Normal Aufbau

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
4p p orbitals, shell n=4 6 6 4p⁶
4d d orbitals, shell n=4 10 10 4d¹⁰
5s s orbital, shell n=5 2 2 5s²
5p p orbitals, shell n=5 (valence) 2 6 5p²
Total 50

Full Configuration

1s² 2s² 2p⁶ 3s² 3p⁶ 3d¹⁰ 4s² 4p⁶ 4d¹⁰ 5s² 5p²

All subshells written explicitly.

Noble-Gas Shorthand

[Kr] 4d¹⁰ 5s² 5p²

[Kr] = 1s²…4p⁶ (krypton core, Z=36, 36 electrons).

Valence Electrons

5s² 5p²

4 valence electrons — forms Sn²⁺ and Sn⁴⁺ ions.

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 3d¹⁰ 18 / 18 electrons (100%)
Shell 4 (n=4) — 4s² 4p⁶ 4d¹⁰ 18 / 32 electrons (56%)
Shell 5 (n=5) — 5s² 5p² 4 / 50 electrons (8%)

Shell 5 can hold up to 50 electrons (5s + 5p + 5d + 5f + 5g). Tin occupies 4 slots — 5s² 5p². The next element, antimony (Z=51), adds one electron to 5p to reach 5p³.

Group 14 — ns² np² Pattern

Element Z Noble-gas configuration Valence
Carbon (C) 6 [He] 2s² 2p² 4
Silicon (Si) 14 [Ne] 3s² 3p² 4
Germanium (Ge) 32 [Ar] 3d¹⁰ 4s² 4p² 4
Tin (Sn) 50 [Kr] 4d¹⁰ 5s² 5p² 4
Lead (Pb) 82 [Xe] 4f¹⁴ 5d¹⁰ 6s² 6p² 4

All Group 14 elements share the ns² np² valence pattern. The stable +2 oxidation state becomes more common down the group due to the inert pair effect — Sn²⁺ is common, Pb²⁺ is dominant.

Ion Electron Configurations

Sn²⁺ (Stannous)

[Kr] 4d¹⁰ 5s²

Loses the two 5p electrons. The 5s² pair is retained — inert pair effect stabilizes this ion.

Sn⁴⁺ (Stannic)

[Kr] 4d¹⁰

Loses all four valence electrons (5s² 5p²). The stable 4d¹⁰ core remains intact.

Summary

Reference for tin's electron configuration ([Kr] 4d¹⁰ 5s² 5p²), orbital box diagram, valence electrons, and key atomic data for Sn (Z=50).

How it works

  1. The Aufbau principle fills subshells in order of increasing energy: 1s, 2s, 2p, 3s, 3p, 4s, 3d, 4p, 5s, 4d, 5p.
  2. Tin (Z=50) follows normal Aufbau filling — no anomaly like copper or silver.
  3. The krypton core [Kr] accounts for 36 electrons across 1s through 4p.
  4. After [Kr], the 4d subshell fills completely with 10 electrons, then 5s with 2, then 5p with 2.
  5. The shorthand [Kr] 4d¹⁰ 5s² 5p² captures the 14 electrons beyond the noble-gas core.
  6. Four valence electrons (5s² 5p²) allow tin to form Sn²⁺ (losing 5p²) and Sn⁴⁺ (losing all 5s² 5p²) ions.

Use cases

  • Quick reference for chemistry homework on Period 5 p-block elements.
  • Understand how tin forms Sn²⁺ (stannous) and Sn⁴⁺ (stannic) oxidation states.
  • Visualize orbital filling for tin using the orbital box diagram.
  • Compare tin's configuration to neighboring elements germanium and lead.
  • Teaching aid for Aufbau principle and p-block electron filling.
  • Verify valence electron count for tin in bonding and Lewis structure problems.
  • Learn why tin has two allotropes related to its electronic structure.

Frequently Asked Questions

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