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

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

3. Characteristics: Held together by strong electrostatic forces a) the greater the charges of the ions, the greater the electrostatic forces. EX: CaCl 2 vs NaCl b) The smaller the ions the greater the attraction. EX: KBr vs. LiF Ionic Solids

4. 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

5. Have atoms at the points of their lattice Atomic Solids

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

7. 2)Network covalent - Nonmetals at the points of lattice. Only a few examples even exist:  C (graphite), C (diamond), Si, SiO 2

8. 3)Noble Gases / Group 8A

9. Examples

10. Types of Solids Ionic solids (ionic compounds - salt) ions at points in lattice Molecular solids (molecular compounds - sugar) covalently bonded molecules at each point in lattice Atomic solids (metals, nonmetals, noble gases) metallic– delocalized covalent bonding network – strong covalent bonding Group 8A –London Dispersion Forces

11. 1. London dispersion forces (LD) 2. Dipole-dipole forces 3. Hydrogen bonding 4. Ionic compounds 5. Metallic 6. Network covalent