Properties and Structures of Covalent and Ionic Compounds

Simple Molecular Compounds

Small molecules with low melting and boiling points.

Ionic Compounds

Composed of metals and nonmetals with ionic bonds.

Giant Ionic Lattices

Regular structures with strong electrostatic forces.

High Melting Points

Require energy to break strong ionic bonds.

Conductivity in Ionic Compounds

Conduct electricity when molten or dissolved.

Weak Intermolecular Forces

Cause low melting and boiling points in small molecules.

Covalent Bonds

Strong bonds formed by shared electron pairs.

Giant Covalent Structures

Solids with very high melting points and strong bonds.

Delocalised Electrons

Electrons free to move in metallic structures.

Metallic Bonds

Strong bonds due to delocalised electrons in metals.

Graphite Structure

Layers of hexagonal rings with weak intermolecular forces.

Diamond Structure

Each carbon bonded to four others, very hard.

Electrodes

Graphite conducts electricity, used in electrodes.

Lubricants

Graphite's slippery layers reduce friction.

Fullerenes

Carbon molecules with hollow shapes and rings.

Graphene

Single layer of graphite with unique properties.

Carbon Nanotubes

Cylindrical fullerenes with high aspect ratios.

Buckminsterfullerene (C60)

Spherical fullerene with 60 carbon atoms.

Solubility in Water

Some small molecules dissolve due to strong interactions.

High Boiling Points

Result from strong intermolecular forces in larger molecules.

Electrical Conductivity

Ability to conduct electricity depends on charge carriers.

Insoluble Metals

Most metals do not dissolve in water.

Soft and Slippery Graphite

Weak forces allow layers to slide easily.

Uses of Diamond

Cutting tools due to hardness and rigidity.

Uses of Nanotubes

Reinforcement in materials like tennis rackets.

Properties of Metals

High melting points and good electrical conductivity.