Giant Covalent structures

Simple Molecules

H2O + O2 + NH3 + F2

Diamond

Covalent bond between carbon atoms, each carbon forms 4 covalent bonds

→ tetrahedral shape

Forms a massive lattice of very strong covalent bond that holds lost of energy to break

Properties of Diamond

• High melting point ( 3700 K )

• Doesn’t conduct electricity cuz there’s no delocalised electrons to carry a charge

• Hard + Insoluble 4 very staring covalent bond

• Good thermal conductor

Graphite

Each carbon atom form 3 covalent bonds to other c atoms, the 4 th c atom is an electron in the p orbital.

Shaped in multiple layers held by intermolecular force / Van Der Waals forces

Properties of Graphite

• Can conduct electricity, cuz there’s p orbital delocalised electrons in between the layers to carry a charge

• Soft + Slippery, weak VDW forces + intermolecular forces in between the graphite layers. → easy to break

• High melting point ( 3900 K ) + 3 strong covalent bond

• Insoluble

uses of graphite + graphene

Graphite : Pencils + Lubricant + Polishes

Graphene : single / one atom thick layers of commonly found mineral graphite

energy storage + electronic

Buckminsterfullerene

C 60 → 60 carbon atoms arranged into a spherical shape

Mixture of pentagon + hexagon rings

Uses of Buckminsterfullerene

1. Surface coating to improve water resistance

2. use in Medina as antioxidant