Full configuration
1s² 2s² 2p⁶ 3s² 3p⁶ 3d¹⁰ 4s² 4p⁶ 4d¹⁰ 5s² 5p²
In the short form, [Kr] stands for the 36 electrons of krypton, the noble gas before tin. Only the electrons after it are written out.
Orbital diagram
Outer subshells only. Each box is an orbital; electrons fill singly first (Hund's rule), then pair up with opposite spins.
What the configuration tells you
Tin is in group 14, period 5, in the p-block. It has 2 unpaired electrons in the ground state, so the atom is paramagnetic.
Configuration of tin ions
| Ion | Configuration | Unpaired | Moment (BM) |
|---|---|---|---|
| Sn²⁺ | [Kr] 4d¹⁰ 5s² | 0 | 0.00 |
| Sn⁴⁺ | [Kr] 4d¹⁰ | 0 | 0.00 |
Moment is the spin-only magnetic moment μ = √(n(n + 2)) Bohr magnetons, where n is the number of unpaired electrons.
Nearby elements
| Z | Element | Configuration |
|---|---|---|
| 47 | Silver | [Kr] 4d¹⁰ 5s¹ |
| 48 | Cadmium | [Kr] 4d¹⁰ 5s² |
| 49 | Indium | [Kr] 4d¹⁰ 5s² 5p¹ |
| 51 | Antimony | [Kr] 4d¹⁰ 5s² 5p³ |
| 52 | Tellurium | [Kr] 4d¹⁰ 5s² 5p⁴ |
| 53 | Iodine | [Kr] 4d¹⁰ 5s² 5p⁵ |
Questions students ask
What is the electronic configuration of tin?
[Kr] 4d¹⁰ 5s² 5p², or in full, 1s² 2s² 2p⁶ 3s² 3p⁶ 3d¹⁰ 4s² 4p⁶ 4d¹⁰ 5s² 5p². Tin has atomic number 50.
How many electrons are in each shell of tin?
2, 8, 18, 18, 4 (K, L, M, N… shells in order).
How many unpaired electrons does tin have?
2 in the ground state, so tin atoms are paramagnetic.
What is the electronic configuration of Sn²⁺?
[Kr] 4d¹⁰ 5s², with 0 unpaired electrons.