1. Bonding
The force that holds two or more atoms together

2. Bond Types Ionic - metal and non metal salts oxides
Covalent between non metals only
Metallic between metals only
James

3. Ionic Bonds Between Metal and NON metal
Transfer of electrons from metal to non metal
creating positive CATIONS & negative ANIONS
Creates an electrostatic charge between
cation and anion
Electronegativity difference GREATER than 1.7
Basic Unit is the FORMULA UNIT

4. Properties of Ionic Bonds
Hard, brittle
Solids
Form crystals
Good conductors of heat and electricity ONLY in molten state or in SOLUTION.
Poor conductors in solid state.
High Melting Points
High Boiling Points

5. Terms to Know
Crystal Lattice - a three (3) dimensional geometric arrangement of particles
Lattice Energy- the energy required to separate one mole of ions in a crystal lattice.
(the energy to break apart a lattice structure)
Endothermic
Exothermic

6. Terms to Know (cont.)
Formula Unit- the simplest ratio of the ions represented in an ionic compound
Monatomic ion- a one atom ion
Ex: Na Mg Al+3

7. Terms to Know con’t Endothermic -- Takes in heat energy, absorbs heat
Exothermic-- Exits heat, releases heat, heat goes out
Electrolyte– An ionic compound that conducts
electricity

8. Examples OXIDES- Metal and oxygen
Salts- An ionic compound made from the cation
of a base and an anion from an acid
NaCl, MgSO4, CaCl2
Sodium chloride magnesium sulfate calcium chloride
OXIDES- Metal and oxygen
MgO, Na2O, CaO, Al2O3
magnesium oxide sodium oxide calcium oxide aluminum oxide