SolidsAMORPHOUS- THOSE WITH MUCH DISORDER IN THEIR STRUCTURE.CRYSTALLINE- HAVE A REGULAR ARRANGEMENT OF COMPONENTS IN THEIR STRUCTURE.

Ionic solids have ions at the points of the lattice. Ex: NaCl

Ionic Solids

Characteristics: Held together by strong electrostatic forces

a) the greater the charges of the ions, the greater the electrostatic forces.

EX: CaCl2 vs NaCl

b) The smaller the ions the greater the attraction.

EX: KBr vs. LiF

Ionic Solids

Molecular solids have molecules at the points of lattice. EX: Ice, sugar

Held together by dipole-dipole, hydrogen bonding or London dispersion forces-Intermolecular forces

Molecular Solids

Have atoms at the points of their lattice

Atomic Solids

Three Types:1) Metallic Solids - metal atoms at the points of lattice.Free moving “sea” of valence electrons

Atomic Solids

2) Network covalent - Nonmetals at the points of lattice. Only a few examples even exist:

C (graphite), C (diamond), Si, SiO2

3) Noble Gases / Group 8A

Examples

Types of Solids Ionic solids (ionic compounds - salt) ions at points in lattice

Molecular solids (molecular compounds - sugar) covalently bondedmolecules at each point in lattice

Atomic solids (metals, nonmetals, noble gases) metallic– delocalized covalent bondingnetwork – strong covalent bondingGroup 8A –London Dispersion Forces

1. London dispersion forces (LD)2. Dipole-dipole forces3. Hydrogen bonding4. Ionic compounds 5. Metallic6. Network covalent