Understanding the scientific rationale behind Silicon's position in the periodic table:
Belongs to Group 14 because it has 4 valence electrons (3s² 3p²).
Belongs to Period 3 because its outermost occupied shell is n=3.
Belongs to the p-block because its valence electrons fill 3p subshells.
Classified as a metalloid due to its lustrous metallic appearance combined with brittle mechanical nature and semiconductor bandgap (1.1 eV).
Hover or tap any shell orbit ring to inspect electron counts and 2n² capacities.
Educational Note: This Niels Bohr planetary model visually illustrates principal quantum energy shells ($n=1, 2, 3\dots$) and electron counts. In modern quantum mechanics (Schrödinger model), electrons do not orbit in fixed circular planetary tracks, but exist as 3D probability clouds (orbitals: $s, p, d, f$) governed by the Heisenberg uncertainty principle.
Neutral ground state configuration. Valence electrons: 4.
Extensively present throughout Earth's mantle and crust as silica (SiO₂ / quartz) and silicate minerals (feldspar, granite).
From Latin 'silex' or 'silicis' meaning flint stone
Elemental silicon is non-toxic, but chronic inhalation of crystalline silica dust causes silicosis, a progressive irreversible lung disease.