The Structure and Properties of Solids

Ionic Crystals

Formed by electrostatic attraction of ions.

Metallic Crystals

Composed of cations in a sea of electrons.

Ionic Crystals

Formed by electrostatic attraction of ions.

Metallic Crystals

Composed of cations in a sea of electrons.

Molecular Crystals

Arranged by weak intermolecular forces between molecules.

Covalent Network Crystals

Atoms bonded by strong covalent bonds in a network.

Ionic Bonding

Electrostatic attraction between oppositely charged ions.

High Melting Points

Requires energy to overcome strong ionic bonds.

Brittle Nature

Shatters when like-charged ions repel under stress.

Conductivity in Ionic Compounds

Conducts electricity when dissolved or melted.

Metallic Bonding

Valence electrons shared among metal cations.

Sea of Electrons

Mobile electrons that allow conductivity in metals.

Diamond Structure

Each carbon bonded to four others in tetrahedral shape.

Graphite Structure

Carbon atoms in layers, bonded by weak forces.

Quartz Structure

Silicon bonded to four oxygen atoms in tetrahedral shape.

Hardness of Covalent Crystals

Very hard due to strong covalent bonds.

Low Melting Points in Molecular Crystals

Weak intermolecular forces lead to low melting points.

Malleability of Metals

Metals can be shaped without breaking.

Ductility of Metals

Metals can be drawn into wires.

Intermolecular Forces

Forces between neutral molecules in molecular crystals.

London Forces

Weak forces due to temporary dipoles.

Dipole-Dipole Forces

Attraction between polar molecules.

Hydrogen Bonding

Strong attraction between hydrogen and electronegative atoms.

Covalent Bonds

Strong bonds formed by sharing electrons.

Strength of Ionic Bonds

Determined by ion size and charge.

Properties of Ionic Crystals

High melting points, hard, brittle, non-conductive solids.

Properties of Metallic Crystals

Conductive, malleable, ductile, variable hardness.

Properties of Molecular Crystals

Soft, low melting points, non-conductive.