1. Unit 2 – Chapter 5 Ionic Compound Names
Ionic Compounds
Unit 2 – Chapter 5 Ionic Compound Names

2. Review (1 of 5) Ion: charged atoms. How does this happen?
Add or remove electrons…

3. Review (2 of 5) CATION-- ANION— Positive Charge Lose Electrons
Usually Metals
Plussycat
ANION—
Negative Charge.
Gain Electrons.
Usually Nonmetals
Ant-ion

5. +1 -3 -2 -1 +2 +3

6. Review (5 of 5)

7. Electrically Neutral = ZERO
Cation + Anion = Compound
REMEMBER:
Compounds are NEUTRAL.
Total Cation Charge = Total Anion Charge.
(0) net charge = Electroneutrality.

8. Binary Ionic Compounds.
“Binary” = Two elements together…
Rules:
Cation is written and named first.
Borrow names from the elements.
2 or more ions – Roman Numerals indicate charge.
Common Multiples: Cobalt, Copper, Iron, Lead, Nickel, Tin.
Anion is written second.
Borrow names from the elements PLUS “-ide”.

9. Binary Ionic Compounds.
Writing Formulas:
Sodium Chloride Potassium Iodide Calcium Fluoride Iron (II) Oxide Iron (III) Oxide
NaCl KI CaF2 FeO Fe2O3

10. Binary v. Polyatomic “Binary” = Two elements together…
NaCl, MgO, Li2S
“Polyatomic” = Two or more elements (bonded together) with a positive or negative charge.
NO3-, CO3-2, PO4-3, NH4+1
Rules: Same as BINARY…balance the charges!

11. Polyatomic Hints “-ide” = Binary “-ate” or “-ite” = Polyatomic
Sodium Nitride = Na3N
“-ate” or “-ite” = Polyatomic
Sodium Nitrate = NaNO3

12. Polyatomic Example Sodium carbonate Potassium sulfate Calcium nitrate
Na2CO3
K3SO4
Ca(NO3)2