1. Naming Ionic Compounds
Ionic Bonding
Naming Ionic Compounds

2. Naming Ionic Compounds
The same as naming individual ions.
Cation, Electron Donor, or Metal in compound is said first.
Anion name is changed to …….ide and said second.

3. Examples Sodium Chloride Magnesium Oxide Lithium Nitride
Potassium Bromide

4. Using the correct Name K2S 7) SrS 2) LiBr 8) Al2O3 3) Sr3P2 9) MnO
4) BaCl2 10) ZnO
5) NaBr 11) ZnCl2
6) MgF2 12) Cu2O

5. Notation Ionic Notation 3 Na+1 1 PO4-3 Ionic Compound Formula NaCl
CaCl2
Na3(PO4)

6. Formulas Rules for Writing Formulas
Metallic Donor is always written first.
Nonmetallic Receiver is written second.
Write the number of atoms required to balance the formula as subscripts after the element in compound.
NaCl
MgO
MgCl2

7. The Ionic Compound
NaCl

8. Writing & Naming Ionic Compounds
Na+1 & Br-1

9. Writing & Naming Ionic Compounds
Ca+2 & Br-1

10. Writing & Naming Ionic Compounds
K+1 & O-2

11. Writing & Naming Ionic Compounds
Li ? & N ?

12. HW: Write the Name of the Compound
MgS 7) KBr
2) Ba3N2 8) FeO
3) NaI 9) SrF2
4) Li2S 10) CaO
5) Na3P 11) Al2O3
6) KCl 12) Fe2O3

13. Formulae of binary ionic compounds
Binary – only two elements present
The rules –
symbol for the cation first, followed by the symbol for the anion.
Determine the lowest whole number ratio of ions that will provide a net charge of zero
The ‘crossover’ method is another way to determine formulae (check page 79)
Work through the Sample Problems page 80,81

14. Review
Complete the revision questions page 81 (13 – 16)

15. Ions of Variable Charge
Some transition metals have quite complicated arrangement of electrons and may be able to form more than one ion. Such ions have different charges.
This is very significant as ions of the same element with different charges have different physical and chemical properties.
Eg – a solution of Cr6+ is orange, whereas a solutions of Cr3+ is yellow.

16. Ions of Variable Charge
Iron can form FeO (black) and Fe2O3 (brown), each with different physical and chemical properties. Therefore you must name them differently.
They cannot each be called iron oxide.
Therefore black FeO containing Fe2+ ions is called iron (II) oxide.
The brown Fe2O3 contains Fe3+ ions and is name iron (III) oxide.

17. Ions of Variable Charge
Metal ions that form more than one cation include iron (II) and (III), copper (I) and (II), and mercury (I) and (II).
Note the roman numeral do not indicate the numbers of ions present in the compound, only the charge of the ion.

18. Ions of Variable Charge
Work through the Sample Problem page82

19. Review
Complete the revision questions page 82 (17,18)

20. HW: Write the Correct Formula
Magnesium Oxide
2) Lithium Bromide
3) Calcium Nitride
4) Sodium Sulfide
5) Copper (I) Sulfide
6) Copper (II) Sulfide

21. Practice Exercise #1 Which will donate, Which will receive?
How many will be donated/received?
Write the Ionic Notation of each.
Write the formula for each of the following.
Lithium Oxide
Potassium Chloride
Sodium Nitride
Calcium Chloride
Magnesium Sulfide
Barium Nitride
Aluminum Fluoride
Aluminum Oxide
Aluminum Nitride

22. Polyatomic ions
A polyatomic ion is a group of tightly bound atoms that behaves as a single unit and carries an overall charge. It may be a positively or negatively charged ion.
The carbonate ion is composed of one carbon atom and three oxygen atoms.
The whole group of four atoms carries a negative two charge.

23. Polyatomic Ions Compound Ions
A group of COVALENTLY bonded atoms that have a net charge (anion or cation)
Most, but not all are Anions.

24. Polyatomics SO4-2 Sulfate SO3-2 Sulfite NO3-1 Nitrate NO2-1 Nitrite
CO3-2 Carbonate
CN-1 Cyanide
OH-1 Hydroxide
NH4+1 Ammonium

25. Na3PO4 Na P O

26. Phosphate can accept 3 electrons.
PO4-3 O
When it does it has a negative 3 charge. P O O
It is therefore called a……….. O

27. Sodium Phosphate O Na O P O Na O
Na3PO4 Na

28. Practice Exercise #3 Give the Ionic Notation and Formula for each.
Potassium Sulfate
Magnesium Sulfite
Aluminum Nitrate
Sodium Nitrite
Lithium Carbonate
Sodium Cyanide
Barium Hydroxide
Ammonium Chloride
Ammonium Hydroxide
Draw/Diagram Magnesium Sulfite

29. Practice Exercise #4
Write out the Ionic Notation, Formula and Names of the following ionic compounds:
Li and F - Na and CO3-2
Na and S - Li and OH-1
K and Br - NH4+1 and Cl
Rb and O - Ca and SO4-2
Ca and Cl - NH4+1 and OH-1
Mg and SO Na and CN-1
Al and NO NH4+1 and SO4-2

30. Polyatomic ions
Work through the Sample Problem pages 84, 85

31. Review
Complete the revision questions page 85 (19 – 21)

32. Hydrated ionic compounds
A number of ionic compounds, called hydrates, produce water when they decompose upon heating. When the formula of a hydrated compound is written, the number of water molecules is also included.
Eg. – the formula for iron(II) sulphate octahydrate is written as FeSO4 . 8H2O.
This formula indicates that eight molecules of water are bonded within the ionic crystal for every one formula unit of FeSO4
Work through the Sample Problem page 86

33. Review Complete the revision question page 86 (22)
Complete the multiple choice questions pages 86, 87
Complete review questions 1, 3, 5, 6, 8, 10, 11, 13
Complete the Exam Practice Questions
Try this ionic compound construction kit - Ionic Compounds