Silicon Electron Configuration
Interactive reference for silicon's electron configuration (1s² 2s² 2p⁶ 3s² 3p²), orbital box diagram, quantum numbers, and semiconductor context.
Use the Silicon Electron Configuration
Silicon — Electron Configuration
Atomic number 14 · Metalloid (semiconductor) · Period 3, Group 14 · p-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 | 2 | 6 | 3p² |
| Total | 14 | |||
Full Configuration
1s² 2s² 2p⁶ 3s² 3p²
All subshells written explicitly.
Noble-Gas Shorthand
[Ne] 3s² 3p²
[Ne] = 1s² 2s² 2p⁶ (the filled neon core).
Shell Fill Summary
Shell 3 can hold up to 18 electrons (3s + 3p + 3d). Silicon uses only 4 of those 18 slots.
Why Silicon Is a Semiconductor
With four valence electrons (3s² 3p²), each silicon atom bonds to four neighbors in a tetrahedral diamond-cubic lattice. The resulting band gap of ~1.1 eV is ideal for electronics: large enough to block current at low voltages, small enough for controlled conduction when doped with phosphorus (n-type, adds electrons) or boron (p-type, adds holes). This configuration is the physical foundation of virtually every transistor and integrated circuit.
Summary
Silicon (Si) has atomic number 14 and the ground-state electron configuration 1s² 2s² 2p⁶ 3s² 3p², condensed to [Ne] 3s² 3p² in noble-gas notation. This tool shows a full orbital box diagram with correct Hund's-rule electron placement, a quantum-number table for all 14 electrons, a subshell breakdown, and key data explaining why silicon's four valence electrons make it the foundation of modern semiconductor technology.
How it works
- The Aufbau principle fills orbitals from lowest to highest energy level.
- Silicon's 14 electrons occupy five subshells: 1s, 2s, 2p, 3s, and 3p.
- The inner 10 electrons (1s² 2s² 2p⁶) form the neon core, written [Ne] in shorthand.
- The 3s subshell holds 2 paired valence electrons; the 3p subshell holds 2 unpaired electrons.
- Hund's rule places the two 3p electrons in separate orbitals with parallel spins before pairing.
- Four total valence electrons (3s² 3p²) allow silicon to form four covalent bonds — the basis of its semiconductor properties.
Use cases
- Quick reference for chemistry homework or exam review on silicon.
- Understand why silicon has four valence electrons and forms tetrahedral bonds.
- Visualize Hund's rule with the two unpaired 3p electrons.
- Compare silicon to its neighbors aluminium (Z=13) and phosphorus (Z=15).
- Learn how the [Ne] 3s² 3p² configuration explains silicon's semiconductor band gap.
- Teaching aid for introductory atomic structure and periodic trends lessons.
- Verify quantum numbers for each of silicon's 14 electrons.
- Understand why silicon is in Group 14 and Period 3 of the periodic table.