1. Quiz What is the oxidation number for phosphorous in P4O6?
If sulfur becomes an ion, what is its oxidation number?
What is the name of the following chemical? CaBr2?
Write the following in the Stock method and Latin method: FeBr3
What is the chemical formula for lithium sulfate?

2. GC Quiz What is the oxidation number for phosphorous in P4O6?
What is the oxidation number for magnesium in MgCl2
If sulfur becomes an ion, what is its oxidation number?
What is the name of the following chemical? CaBr2?
What is the chemical formula for potassium nitride?

3. 3.2 Molecular Compounds
(Covalent Compound)

4. Please memorize the following polyatomic ions and their charges
Hydroxide OH-
Carbonate CO3 2-
Nitrate NO3-
Sulfate SO4 2-
Bromate BrO3 –
Phosphate PO4 3-
Ammonium NH4+

5. The most common polyatomic ion is simply “–ate”
Least amount of oxygen is “hypo—ite”
One more oxygen is “—ite”
One more oxygen is “—ate”
One more oxygen is “per–ate”

6. 1 more oxygen “Most common” 1 less oxygen 2 less oxygens Carbon
percarbonate
CO42-
Carbonate
CO32-
Carbonite
CO22-
hypocarbonite
CO2-
Bromine
Perbromate
BrO4-
Bromate
BrO3-
Bromite
BrO2-
Hypobromite
BrO-
Sulfur
persulfate
SO52-
sulfate
SO42-
Sulfite
SO32-
Hyposulfite
SO22-
Nitrogen
Nitrate
NO3-
Nitrite
NO2-
Phosphorus
Phosphate
PO43-
Phosphite
PO33-
Hypophosphite
PO23-

7. Molecular Compounds
Molecular compounds refer to compounds with covalent bonds
Covalent bonds form between two nonmetal elements
How do ionic compounds and molecular compounds differ?

8. Is Li2O a molecular compound?
No! It’s ionic. Because it is formed from a metal and a nonmetal
What is it called?
Is N2O a molecular compound?
Yes! A covalent bond forms between the two nonmetal elements.

9. How to name molecular compounds
When naming molecular compounds, you must state the number of atoms using numerical prefixes.
*The “mono-” prefix is never used for the first atom
1st non-metal + root of 2nd non-metal + -ide

10. Examples NO Nitrogen monoxide (why not mononitrogen?) N2O
Dinitrogen monoxide
S2Cl2
Disulfur dichloride
Cl2O7
Dichlorine heptoxide

11. BF3 NO
N2O5
PCl5
P4O6
Boron trifluoride
Nitrogen monoxide
Dinitrogen pentoxide
Phosphorus pentachloride
Tetraphosphorus hexoxide

12. Nitrogen Trifluoride
Nitrogen dioxide
Carbon dioxide
Triphosphorus tetrachloride
Dihydrogen monoxide
NF3
NO2
CO2
P3Cl4
H2O

13. Hydrates
Ionic crystals with a certain number of water molecules as part of its structures. Ex:
Name the ionic compound first, then add “hydrate” with proper Greek prefix to indicate number of water molecules

14. Practice BaCl2 • 2H2O Barium chloride dihydrate Na2CO3 • 10H2O
Sodium carbonate decahydrate
* CoSO4 • 6H2O
Cobalt (II) sulfate hexahydrate

15. Naming Acids Acids are compounds that produce H+ ions
There are 2 methods to name acids
1) Acids that do not contain oxygen
2) Acids that do contain oxygen

16. Acids that do not contain oxygen
Generally a binary acid (what does this mean?)
Hydro + root of non-metal + “ic” + acid
HCl
Hydrochloric acid
H2S
Hydrosulfuric acid
(dihydrogen monosulfide can also work, and is considered a ‘common name’)

17. Acids that do contain oxygen
These are acids with polyatomic ions
Use the anion molecule to name acid, and add “acid” at end

18. If anion ends with “–ate” add a “-ic”
If anion ends with “-ite” add a “-ous”
H2SO The anion is SO42-, or sulfate
Sulfuric acid
H2SO The anion is SO32-, or sulfite
Sulfurous acid
“Hydro-” is used on acids without oxygen only.

19. Examples Acid Anion acid name Nitric acid Nitrous acid Phosphoric acid
Phosphorous acid
HNO3
HNO2
H3PO4
H3PO3
Nitrate, NO3-
Nitrite, NO2-
Phosphate PO43-
PhosphitePO33-