1. COVALENT COMPOUNDS

2. Ionic vs. Covalent Compound
Ionic Compounds
Between a metal and a non-metal
Transfers electrons
Covalent Compounds
Between a non-metal and a non-metal
Electrons are shared

3. Covalent Compound
Nitrogen = non-metal
Oxygen = non-metal

4. Covalent Compounds
Hydrogen = non-metal
Carbon = non-metal
Look at the first element listed in the compound… notice that it is a NON-METAL
If both elements are non-metals, then it is a covalent bond. This means that rather than transferring electrons (like ionic compounds do), the two elements share their valence electrons

5. Naming Covalent Compounds
Prefixes are used to indicate how many of each atom are in the compound. Prefixes are written in front of each element
Prefixes
Prefixes
1 = mono
2 = di
3 = tri
4 = tetra
5 = penta
6 = hexa
7 = hepta
8 = octa
9 = nona
10 = deca

6. CO2 Naming Example Oxygen = non-metal Carbon = non-metal
Have 2 oxygens
CO2
2 = di
Name (in the order they appear)
Carbon dioxide
Change to “ide”

7. P4O10 Naming Example Oxygen = non-metal Phosphorus = non-metal
Have 10 oxygens
P4O10
10 = deca
Have 4 phosphorus’
4 = tetra
Name (in the order they appear)
Tetraphosphorus decaoxide
Change to “ide”

8. Formula Example CS2 Carbon disulfide C  only have 1
S  have 2 because it is “di”
Carbon disulfide
Formula (put them together in the order)
CS2

9. Formula Example C2Cl4 Dicarbon tetrachloride C  have 2 (di)
Cl  have 4 (tetra)
Dicarbon tetrachloride
Formula (put them together in the order)
C2Cl4

10. Diatomics
These are a type of covalent bond between two atoms of the same element
Example: two chlorine atoms bond together to form Cl2
“Gens” rule
Diatomics go by the GEN rule
HydroGEN, oxyGEN, nitroGEN, haloGEN
O2, N2, F2, Br2, Cl2, I2, H2