1. Unit 9 Chemical Compounds Chapter 6
P. Sci.
Unit 9
Chemical Compounds
Chapter 6

2. Compound Names and Formulas
Part 2
Compound Names and Formulas

3. Binary Compounds
Al(ClO3)3
P2O5
NaCl
Most of the compounds that you will have to name will have only 2 elements (called binary – bi meaning 2)
or an element and a polyatomic ion.
NaCl
CaCl2
P2O5
NaNO3
Al(ClO3)3
CaCl2
NaNO3

4. First you have to identify what type of compound it is :
Naming Compounds
First you have to identify what type of compound it is :
Ionic – metal and non-metal.
Covalent – two non-metals
Polyatomic - both
NaCl
N2O4
CaCO3

5. Write the name of the metal (cations = + ion)
Ionic Compounds
Write the name of the metal (cations = + ion)
Examples:
Na = Sodium
Ca = Calcium
Al = Aluminum

6. Ionic compounds cont.
Write the name of the non-metal (anion = - ion) but change the ending to “ide”.
Examples: Chlorine – Chloride
Fluorine – Fluoride
Oxygen – Oxide
Sulfur – Sulfide
Phosphorus – Phosphide
Iodine - Iodide

7. NaCl = Sodium chloride CaI2 = Calcium iodide CsBr = Cesium bromide
Examples
NaCl = Sodium chloride
CaI2 = Calcium iodide
CsBr = Cesium bromide
Al2O3 = Aluminum Oxide
For ionic compounds – pay no attention to the subscripts.

8. Now you try Name the following ionic compounds. LiF = MgO = SrCl =
K2S =
Ca3N2 =

9. Answers LiF = Lithium fluoride MgO = Magnesium oxide
SrCl = Strontium chloride
K2S = Potassium sulfide
Ca3N2 = Calcium Nitride

10. Covalent Compounds First Name
If there is only one atom of this element, just write the name of the element.
Example:
N = Nitrogen
C = Carbon
P = Phosphorus

11. Covalent compounds cont.
First Name cont.
If there is more than one atom of the element, write the name of the element with the pre-fix that tells how many atoms are there.

12. Pre-fixes 1 – mono 6 – hexa 2 – di 7 – hepta 3 – tri 8 – octa
4 – tetra 9 – nona
5 – penta 10 – deca

13. Examples: H2 – di-hydrogen
C3 – tri-carbon
Br4 – tetra-bromine

14. Covalent compounds cont.
Second Name – Always has a prefix.
Always starts with a prefix that tells how many atoms are there. (even if there is only one)

15. Covalent compounds cont.
Second Name cont.
ends in “ide”
Examples :
CO – carbon monoxide
CO2 – carbon dioxide
CO3 – carbon trioxide

16. Name the following covalent compounds.
Now you try
Name the following covalent compounds.
NO2 =
PBr3 =
AsCl =
H2O =
H2O2 =

17. Answers
NO2 = Nitrogen dioxide
PBr3 = Phosphorus tribromide
AsCl = Arsenic monochloride
H2O = Di-hydrogen monoxide
H2O2 = Di-hydrogen dioxide

18. Polyatomic Ions Compounds with both ionic and covalent bonds.
Acts the same as any other ion.

19. Examples: Ammonium NH4+ Hydroxide OH- Sulfate SO4+2 Carbonate CO3-2
Polyatomic ions cont.
Examples:
Ammonium NH4+
Hydroxide OH-
Sulfate SO4+2
Carbonate CO3-2

20. Follow step one for ionic compounds. (Write the name of the metal)
Polyatomic compounds
Follow step one for ionic compounds. (Write the name of the metal)
Write the name of the polyatomic ion (do not change to “ide”)
Examples:
NaNO3 = Sodium nitrate
Al(ClO3)3 = Aluminum chlorate

21. The
End