1. Naming and Writing Formulas

2. Types of Compounds There are two types of compounds. Ionic: Covalent:
a metal and an nonmetal
Covalent:
contain two nonmetals

3. Ionic Compounds
Must contain a positive ion (cation) and negative ion (anion).
The cation (metal) is written first, the anion (nonmetal) is written second.
The total charge on the compound must equal 0.

4. Naming Binary Ionic Compounds
#1 – Name the metal (written on periodic table)
#2 – Name the nonmetal, changing the ending to –ide.
Examples:
MgO
CaCl2
NaBr
Sr3P2
magnesium oxide
calcium chloride
sodium bromide
strontium phosphide

5. Writing Formulas
The subscripts tell how many of each atom you have. (The overall charge must equal zero!!)
EXAMPLE: Write the chemical formula for the compound containing Al and Br.
#1 – determine the charges
Al Br-1

6. Al+3 Br-1 AlBr3 #2 – cross the charges.
#3 – Write the formula, simplify if needed
AlBr3 1 3

7. Try this one…
Write the chemical formula for the compound containing Mg and S
#1 – determine the charges
Mg S-2

8. Mg+2 S-2 Mg2S2 MgS #2 – cross the charges.
#3 – Write the formula, simplify if needed
Mg2S2
MgS 2 2

9. Ionic Compounds with Polyatomic Ions
#1 – name the 1st part of the compound
#2 – name the 2nd part
If it is a polyatomic ion, DO NOT change the ending
If it is a nonmetal, change to –ide.
Examples:
CaCO3
Na3SO4
(NH4)2S
Calcium carbonate
Sodium sulfate
Ammonium sulfide

10. Writing Formulas: Na+1 OH-1 NaOH
Same rules apply, except if the polyatomic ion gets a subscript you MUST use parentheses around it.
Example:
Write the formula for sodium hydroxide.
Na OH-1
NaOH 1 1

11. Writing Formulas for Polyatomic Compounds
Calcium phosphate
Ca PO4-3
Ca3(PO4)2 3 2

12. Aluminum nitrite
Al NO2-1
Al(NO2)3 1 3

13. Homework
Page 221
Problems 19, 20, 21 and 22
Page 233
Problem 83

14. Compounds Containing Metals with Variable Charges

15. Variable Charges (Transition Metals)
Metals in Group 1, Group 2, Zinc (+2), Silver (+1) and Aluminum only have one charge.
The rest have variable charges so we have to tell what charge the ion has in our compound when we name it.

16. Naming #1 – Name the metal.
#2 – Add a roman numeral telling the charge on the metal in parentheses.
I-1 II-2 III-3 IV-4 V-5 VI-6 VII-7
#3 – Name the negative ion as before.

17. Example CrO O is a -2 charge
To make a neutral compound, Cr must be a +2.
Chromium (II) oxide

18. FeCl3 Cl is a -1 charge There are 3 chlorine ions  -3
The ONE Fe must be a +3
Iron (III) chloride

19. CoCO3
Carbonate is a -2
Co is a +2
Cobalt (II) carbonate

20. Ni3(PO4)2 Phosphate = -3 x 2 = -6
There are 3 nickel atoms so each one = +2 to equal +6
Nickel (II) phosphate

21. Mn(SO4)2 Sulfate is -2, there are two  -4 so the ONE Manganese = +4
Manganese (IV) sulfate

22. Writing formulas:
Rules are the same as before.

23. copper (III) oxide
Cu+3 O-2
Cu2O3 2 3

24. Manganese (IV) sulfide
Mn+4 S-2
Mn2S4
MnS2 4 2

25. Iron (II) nitrate
Fe+2 NO3-1
Fe(NO3)2 1 2

26. Classwork
Page 223
Problems 28, 29, 30, 31 and 32
Page 233
Problem 82