1. Covalent Compounds: Names & Formulas

2. Objectives By the end of the lesson you should be able to:
Describe the differences between covalent and ionic bonds
Name and make all types of ionic and covalent compounds

3. Ionic Compounds Always involve a metal and a non-metal
Electrons are always transferred from the metal to the non-metal
Create ions because losing and gaining electrons (charges result)

4. Covalent Compounds Always involves 2 or more non-metals
Electrons are shared between the non-metals
Occurs in all diatomic molecules
DO NOT form ions!

5. Covalent Compound Examples
Carbon monoxide CO
Carbon dioxide CO2
Water H2O
Dihydrogen dioxide H2O2
Dinitrogen tetrachloride N2Cl4
Phosphorus trihydride PH3
Can we see any patterns or notice anything interesting?

6. Naming Covalent Compounds
Name first element
Name second element with “ide” ending
Add any needed prefixes

7. Prefixes IF first atom is 1 DO NOT add “mono” Change any “oo” to “o”
Prefix # Atoms
Mono Di
Tri
Tetra
Penta
Hexa
Hepta
Octa
Nona
Deca
Change any “oo” to “o”
I.E. monooxide = monoxide

8. Naming Covalent Compounds
Examples
Eg. CO carbon monoxide
N2O3 dinitrogen trioxide
CS2 carbon disulphide
CCl4 carbon tetrachloride
P4O10 tetraphosphorus decaoxide

9. Making Covalent Compounds
Write each symbol
Add any subscripts according to prefixes
DO NOT reduce
Examples
Eg. Nitrogen tribromide NBr3
Dichlorine monoxide Cl2O
Dinitrogen tetrachloride N2Cl4

10. Naming Covalent Compounds With Hydrogen
Memorize:
CH4 = methane
NH3 = ammonia
H2O = water

15. Summary IONIC “ide” endings Multivalent = Roman numerals
transfer electrons
Metal + non metal
“ide” endings
Multivalent = Roman numerals
Polyatomics = brackets
COVALENT
Share electrons
Two non metals
“ide” endings
prefixes