1. Binary Ionic Compounds

2. Ionic Compounds ions of opposite charge chemically bonded together
Electrons are transferred from one element to the next
bonds form between anions (-) and cations (+)
OR bonds form between metals and nonmetals
bonded together so that the net charge (oxidation number) of the atom is zero

3. Atoms will combine in compounds to make every element have a total of 8 valence

4. Basic Properties of Ionic Compounds
Electrolytes
Conduct electricity in aqueous solution
Dissolve well in water
Solid crystal at room temperature
Strong interparticle forces

5. Binary Ionic Compounds
Ionic compound formed from two elements (can contain more than one atom of each element)
Examples:
NaCl
MgBr2

6. Naming Binary Ionic Compounds
Name metal first (positive ion)
Then add the name of the nonmetal (negative ion) but change the ending to “ide”
Ending is usually the last syllable
Example: sodium (Na) and chlorine (Cl)
Name: Sodium Chloride
Chemical Formula: NaCl

7. Practice Problem 1:
Name the ionic compound shown below: MgF2 Magnesium fluoride

8. Practice Problem 2:
Name the ionic compound shown below: Li2O Lithium oxide

9. Writing Chemical Formulas for Binary Ionic Compounds
Write the symbol for each element with it’s oxidation number (charge)
Remember: write metal first
Chemical formulas of ionic compounds are always neutral (so oxidation numbers must balance)
Add subscripts to the symbols for the ions until the sum of the charges is equal to zero
No subscripts are needed if only one ion is present

10. Example: Calcium Chloride
Ca+2 Cl-1
CaCl2

11. Practice Problem 3:
Write the chemical formula for aluminum bromide.

12. Practice Problem 4:
Write the chemical formula for magnesium nitride.

13. Practice Problem 5
Write the chemical formula for calcium oxide.