1. Ionic Naming

2. Objective/Warm-up SWBAT name ionic compounds.
Criss-Cross the following:
Ca+2 and SO4-2
Na+1 and PO4-3
Al+3 and O-2
Mg+2 and N-3

3. Definitions
An IONIC COMPOUND consists of a metal cation bonded to a nonmetal anion. Electrostatic attraction holds them together.
Metal Cation Nonmetal anion
Na+ Cl-

4. A quick review
Do you remember how to find the charges on different elements from the periodic table?

5. Type I Binary Ionic Compounds
The metal cations in these compounds have only ONE possible charge.
Na+ Zn2+ Al3+ Ca2+
sodium zinc aluminum calcium
The charges are memorized or predicted using a periodic table!
The cations are bonded to nonmetal anions:
O2- N3- F- Br -
oxide nitride fluoride bromide
Notice that simple anions are always named with the suffix “ide”

6. In an ionic compound, the charges of the cations and anions must always cancel out.
Subscripts are used if more than one atom is needed to cancel the charges:
sodium chloride: Na+ and Cl- ® NaCl
lithium oxide: Li+ and O2- ® Li2O
aluminum bromide: Al3+ and Br - ® AlBr3
zinc nitride: Zn2+ and N3- ® Zn3N2
potassium iodide: K+ and I- ® KI
silver phosphide: Ag+ and P3- ® Ag3P

7. Lets do some practice

8. Examples: Type I Binary Ionic Compounds
Write the formulas:
potassium oxide
zinc chloride
silver sulfide
aluminum nitride
gallium oxide
calcium iodide

9. Potassium Nitride Silver Iodide Zinc Bromide Aluminum Oxide
Write the names:
K3N
AgI
ZnBr2
Al2O3
Ba3P2
LiH
Potassium Nitride
Silver Iodide
Zinc Bromide
Aluminum Oxide
Barium Phosphide
Lithium Hydride

10. Type II Binary Ionic Compounds
These are ionic compounds where the metal cation can form TWO different charges.
Fe2+ iron (II) Fe3+ iron (III)
Ni nickel (II) Ni nickel (III)
Co2+ cobalt (II) Co3+ cobalt (III)
Cu copper (I) Cu2+ copper (II)
Au gold (I) Au3+ gold (III)
Sn tin (II) Sn4+ tin (IV)
An older system uses suffixes and Latin names, -ous for the lower charge, -ic for the higher charge:
Ferrous & Ferric, Cuprous & Cupric, Stannous & Stannic

11. Why do transition metals have different charges?
Why do you think so?
Write the shorthand electron configuration for Iron and draw orbital diagrams for iron to see if you can figure it out.

12. Answer The shorthand electron configuration for Iron is
This shows that it has 2 valence electrons that it would like to lose so it explains why it can exist with a +2 charge.
If Iron loses 2 electrons its electron configuration will be This will make it easy for another electron to be lost because all electrons like to be alone rather than paired. See below.  

13. Examples: Type II Binary Ionic Compounds
Write the formulas:
iron (II) oxide
copper (II) chloride
tin (IV) sulfide
cupric nitride
nickel (III) oxide

14. Examples: Type II Binary Ionic Compounds
Write the names:
Fe2O3
SnS
NiBr2
CuS
Pb3P2
CuBr
FeCl3
iron (III) oxide
Tin (II) Sulfide
Nickel (II) Bromide
Copper (II) Sulfide
Lead (II) Phosphide
Copper(I) Bromide
iron (III) Chloride

15. Polyatomic (Complex) Ions
All of the cations and anions so far have been simple ions - single atoms that have lost or gained electrons.
A complex ion is a charged molecule. Complex ions may be cations or anions.
examples:
nitrate: NO3- sulfate: SO42- hydroxide: OH-

16. Things to Notice
Most complex ions are anions. Ammonium, NH4+, is the most common complex cation.
Several complex ions form a short series of ions. The ions differ only in the number of oxygen atoms:
perchlorate ClO4- sulfate SO42-
chlorate ClO3- sulfite SO32-
chlorite ClO2-
hypochlorite ClO- nitrate NO3-
nitrite NO2-

17. Lets do some practice
Use the handout to write the names for the following.

18. Writing formulas with Complex Ions
A. NH4Cl
B. Ag2SO4
C. Al(OH)3
D. Ca3(PO4)2
E. Fe(NO2)3
F. Cu(MnO4)2
G. (NH4)2Cr2O7
H. Zn(CH3COO)2
a) Ammonium chloride
b) Silver sulfate
c) Aluminum hydroxide
d) Calcium phosphate
e) Iron (III) nitrite
f) Copper(II) permanganate
g) Ammonium dichromate
h) Zinc acetate

19. Objective/ Warm-up SWBAT write formulas and name ionic compounds.
Please give the name for the following formulas:
(a) Ag3P (b) Fe2O3 (c) Ag2SO4
Please give formulas for the following names:
(a) Tin (II) Sulfide (b) Iron (III) nitrite

20. Closure
When do we need to use roman numerals in a name?