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Carbon, Silicon, Silicates, and Materials

Chemistry Grade 12 Difficulty 4/5

Beginning of the lesson

Carbon, Silicon, Silicates, and Materials

The same elements can produce radically different properties when bonding and long-range structure change.

Learning goals: connect carbon allotrope structure to properties; compare carbon and silicon networks; explain semiconductor behavior; build silicate structures from $SiO_4$ tetrahedra; distinguish crystalline, glassy, and ceramic materials.

1. Carbon structures

Carbon forms strong covalent bonds and many allotropes. In diamond, each carbon is tetrahedrally bonded to four others in a continuous 3D network, giving high hardness, high melting temperature, electrical insulation, and brittleness. In graphite, each carbon bonds to three others in a planar hexagonal layer. Delocalized electrons move within each layer, while weak forces between layers allow sliding. Graphene is one such sheet: strong and conductive in-plane without weak interlayer interfaces.

Structure controls property

Chemical formula alone is insufficient. Diamond and graphite both contain only carbon, yet coordination, dimensionality, and electron delocalization produce different mechanical and electrical behavior.

2. Silicon and semiconductors

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