1. Chem 1 Chapter 8 Ionic Bonding
Last Updated November 14, 2018

2. Ionic Bonding Chemical Bond – Force that hold atoms together
e- arrangements are involved in chemical bonding and involve orbitals overlapping
e- dot structure is used to illustrate chemical bonds
Atoms attempt to achieve noble gas configurations

3. Ions Cation – (+) positively charged Anion – (-) negative charged
Monatomic Ions – single charged atom
Polyatomic Ions – groups of atoms that is charged and function as a single unit. (See the back of the B&W Periodic Table)

4. Ionic Bond
Force of attraction that holds oppositely charged particles together through the loss and gain of electrons
Most Ionic Compounds are called salts
Typically involve a metal with a non-metal or polyatomic ion.
Lost e- must = gained e-
See practice problems pg 217

5. Examples Magnesium + Chloride Strontium + Phosphorus Boron + Sulfur
Hint: Criss-Cross method

6. Properties of Ionic Compounds
Strong Bond
Form Crystal Lattice
Melting Point, Boiling Point, Hardness  due to strong bonds tend to be high
Good conductors of electricity when dissolved in water
Form electrolytes
Formation of ionic bonds is always exothermic

7. Lattice energy
Energy required to separate 1 mol of ions in ionic cmpd. (Strength holding ions in place)
The more negative the lattice energy the stronger the force of attraction
Related to the size of the ions bonded (LiCl has higher lattice energy than LiBr since atoms are closer together)

8. Naming and Formulas
Formula Unit  simplest ratio of ions represented in an ionic cmpd.
Already defined (monatomic and polyatomic ions)
The charge of a monatomic ion is its oxidation number also called oxidation state.
Do practice pg 224 and 225

9. Naming Name cation followed by anion
Monatomic cations use element name
Monatomic anions use their root name followed by –ide
Oxygen is oxide etc.
Transition metals often have more than 1 oxidation number and therefore use Roman Numerals
When using Polyatomic ions simply name ion

10. Metals Do not form compounds. with other metals.
Mixture of metals is known as an alloy
Form metallic bonds which involve delocalized electrons
Delocalized electrons are free moving electrons.