1. Chemical Bonding
Ionic Compounds

2. Lewis Structures
Ionic – show transfer of e-

3. Things to know about Ionic
Ionic compounds are made up of?
The electrons are being?
What is written first?
Opposite charges will?

4. How to write a formula S.O.C.S Ionic Formulas
Overall net charge must equal zero.
S.O.C.S
Symbols -> Oxidation # -> Crisscross -> Simplify
Don’t show charges in the final formula.

5. Writing Formula Practice
Potassium Chloride
K+ Cl-
 KCl
Aluminum Bromide
Al+3 Br-
 AlBr3
Beryllium Sulfide
Be+2 S-2
 BeS = Reduce

6. How to Name an Ionic Compound
Ionic Nomenclature
How to Name an Ionic Compound
Write the name of the Cation (Metal) first. It comes straight off the periodic table.
Change ending of the Anion (Nonmetal) to end in -ide.

7. Naming Practice
Al2O3
Aluminum Oxide
CaS
Calcium Sulfide
Na3P
Sodium Phosphide

8. Polyatomic Ions
When you have a compound that involves more than 2 elements, you must look at a Polyatomic Chart for help.
When writing formulas, keep these ions in parentheses
These ions will also have different endings (-ate) (-ite)
Helpful for determining between individual atoms and polyatomic ions

9. Writing a Formula
You need to determine if a Polyatomic Ion is present!
Look at the ending of the name
(-ATE) or (-ITE)
What are some exceptions???
What if the ending is (-IDE)?
What will you do then?

10. Writing Polyatomics Potassium Nitrate KNO3 Aluminum Sulfide Al2S3
Barium Phosphite
Ba3(PO3)2
Calcium Hydroxide (careful with this)
Ca(OH)2

11. Naming Polyatomics
Look for more than two elements. That means a Polyatomic is present.
Match up the polyatomics and write the correct names and ending straight from the chart.

12. Practice w/ Polyatomics
CaSO4
Calcium Sulfate
Ga(IO3)3
Gallium Iodate

13. Writing with Transitions
When a Transition metal is involved in the bond, you must identify which form of the atom is bonding.
These atoms can have different oxidation numbers.
Look for the Roman Numeral in the name when writing the formula. The Roman numeral is the oxidation number of the transition metal.

14. Practice Writing Transitions
Copper (II) Fluoride
CuF2
Zinc (I) Phosphate
Zn3PO4
Nickel (IV) Oxide
NiO2 (Simplified formula)

15. Naming Transitions
When Naming the compound, you must balance the total charge, must be zero!
Look at the Anion. Determine the total sum of the charge provided by the Anion.
Look at the Cation. Remembering that the sum of the ionic compound must equal zero, determine the positive charge, and roman numeral.

16. Au2S Gold(I) Sulfide Co2O3 Cobalt(III) Oxide AgN Silver(III) Nitride
Practice Naming Trans
Au2S
Gold(I) Sulfide
Co2O3
Cobalt(III) Oxide
AgN
Silver(III) Nitride

17. Molecular Nomenclature
Prefix System (binary compounds)
Recognize these because they’re made up of 2 nonmetals. Where are nonmetals found???
Add prefixes to indicate # of atoms.
3. Change the ending of the second element to -ide.

18. C. Molecular Nomenclature
PREFIX
mono-
di-
tri-
tetra-
penta-
hexa-
hepta-
octa-
nona-
deca-
NUMBER 1 2 3 4 5 6 7 8 9 10

19. Special Rules with Mono
If there is only one of the first element, then the prefix mono is not used.
If there is only one of the second element, then the prefix mono is necessary.
Ex.
CO – Carbon Monoxide
CO2 – Carbon Dioxide
C2O – Dicarbon Monoxide

20. Also…. CI2 - Carbon Diiodide N3O6 - Trinitrogen Hexaoxide
There is no reducing for covalent compounds. What you see is what you get. If you reduced, you would change the chemical formula and ratio of the elements in the bond….Not good….
C2I4 - Dicarbon Tetraiodide
CI2 - Carbon Diiodide
N3O6 - Trinitrogen Hexaoxide
NO2 - Nitrogen Dioxide

21. C. Molecular Nomenclature
CCl4
N2O
SF6
carbon tetrachloride
dinitrogen monoxide
sulfur hexafluoride

22. C. Molecular Nomenclature
arsenic trichloride
dinitrogen pentoxide
tetraphosphorus decoxide
AsCl3
N2O5
P4O10

23. C. Molecular Nomenclature
The Seven Diatomic Elements
I2 Br2 Cl2 F2 O2 N2 H2 H N O F Cl Br I