1. Topic: Names, Formulas, Equations, & Reactions
Aim: How do we name & write formulas for ionic compounds?
Do now:
Name these: P4O10, NH3, NO2, AlBr3
HW:

2. Naming Ionic Compounds with Polyatomic Ions
See Table E!!
Three options
Metal name + name of polyatomic ion OR
Polyatomic ion + nonmetal (w/ “-ide”) OR
Polyatomic ion + polyatomic ion
Same deal as binary ionic – NO PREFIXES.
Never change name or ending of a poly. ion.

3. Naming Ionic Compounds with Polyatomic Ions
KNO3
NH4Cl
KOH
MgCO3
Al2(SO4)3
Na3PO4
Potassium nitrate
Ammonium chloride
Potassium hydroxide
Magnesium carbonate
Aluminum sulfate
Sodium phosphate

4. Naming Ionic Compounds with Polyatomic Ions
NH4NO3
Ca(NO3)2
LiNO3
K2Cr2O7
Mg(C2H3O2)2
(NH4)2SO3
Ammonium nitrate
Calcium nitrate
Lithium nitrate
Potassium dichromate
Magnesium acetate
Ammonium sulfite

5. Formulas – Ionic Compounds with Polyatomic Ions
No prefixes, so…CRISS-CROSS METHOD AGAIN
Take oxidation state of the element & of the ENTIRE polyatomic ion & criss-cross them to get your formula
**If you end up with more than one polyatomic ion, enclose it in parentheses!! & put the subscript outside
Do not include charge in the final formula Al +3
SO4 -2 Al
(SO4) 2 3

6. Formulas of Ionic Compounds with Polyatomic Ions
Sodium hydroxide
Potassium nitrate
Potassium phosphate
Magnesium sulfate
Magnesium hydroxide
NaOH
KNO3
K3PO4
MgSO4
Mg(OH)2

7. Formulas of Ionic Compounds with Polyatomic Ions
Aluminum phosphate
Aluminum nitrate
Ammonium nitrate
Ammonium sulfite
Sodium carbonate
AlPO4
Al(NO3)3
NH4NO3
(NH4)2SO3
Na2CO3

8. Topic: Names, Formulas, Balancing
Aim: How do you name and write formulas for ionic compounds using the stock system?
Do Now:
Name the following: P2O5, Mg(NO3)2
Write formulas for:
lithium oxide, disulfur tetroxide
HW:

9. Ionic Compounds – Stock System
Some metals have >1 oxidation state
Which ones?
Transition metals

10. Ionic Compounds – Stock System
A ROMAN NUMERAL tells the ox. state to use for the metal.
Example: Iron (Fe) can be +2 or +3
So: Iron (II) chloride tells the reader that Fe has a +2 charge
Formula is Fe+2Cl- (criss-cross)  FeCl2
So: Iron (III) chloride tells the reader that Fe has a +3 charge
Formula is Fe+3Cl- (criss-cross)  FeCl3

11. Formulas – Ionic Compounds – Stock System
Iron II oxide
Tin II sulfide
Lead II nitrate
Iron III oxide
Tin IV oxide
FeO
SnS
Pb(NO3)2
Fe2O3
SnO2

12. Formulas – Ionic Compounds – Stock System
Copper I chloride
Mercury II iodide
Copper II nitrite
Lead IV oxide
Gold I oxide
CuCl
HgI2
Cu(NO2)2
PbO2
Au2O

13. Naming Ionic Compounds – Stock System
When writing the name from the formula, use the NONMETAL (with known oxidation #) to figure out the METAL (b/c there is more than 1 option for the oxidation #)
You have to do a little bit of math.

14. Naming Ionic Compounds – Stock System
Ex: FeO
Fe can be +2 (Iron II) or +3 (Iron III)
Oxygen is -2
1 oxygen x -2 charge = -2 total charge
1 iron x _?_ charge = +2 total charge (to cancel out the -2)
? = +2
So it is Iron II Oxide

15. Naming Ionic Compounds – Stock System
Ex: Fe2O3
Fe can be +2 (Iron II) or +3 (Iron III)
Oxygen is -2
3 oxygens x -2 charge = -6 total charge
2 iron x _?_ charge = +6 total charge (to cancel out the -6)
? = +3
So it is Iron III Oxide

16. Naming Ionic Compounds – Stock System
CuCl
FeS
HgI2
Pb(NO3)2
Sn(OH)2
Copper I chloride
Iron II sulfide
Mercury II iodide
Lead II nitrate
Tin II hydroxide

17. Naming Ionic Compounds – Stock System
Cu(NO3)2
Fe2O3
PbI4
SnO2
FeCO3
Copper II nitrate
Iron III oxide
Lead IV iodide
Tin IV oxide
Iron II carbonate