1. Nomenclature (naming)

2. Definitions Ion: charged atom (ex: Cl-, Mg2+) Cation: + charged ion
Anion: - charged ion
Monoatomic ion: “1 atom” ion (ex: Ca2+)
Polyatomic ion: “many atoms” ion (ex: NO3-)

3. Rules for writing formulas
Use correct symbol for element
Use subscripts to indicate # atoms if there’s more than 1 atom
Write symbol for cation 1st (more metallic element)

4. Ionic Formula Writing Use criss cross method
Ex) Ca2+ and Cl- becomes CaCl2
Practice

5. Naming ionic compounds
Ionic = metal + nonmetal (ie NaCl)
Metal has + charge, nonmetal has – charge
Use periodic table to predict charges when possible (ie Br-, Al3+)

6. Rules for naming ionic compounds
Simply state the 1st element’s name (ie in Al2O3, say aluminum)
The 2nd elements’s last 1-2 syllables are dropped and replace with suffix –ide (ie oxygen becomes oxide)
This applies to monatomic ions ONLY
Polyatomic ions need to be memorized

7. Practice – name the following
Na2O
BaI2
NH4Cl
Mg(OH)2
Ga2(SO4)3

8. d-block Elements
Some monatomic ions’ charges can’t be predicted from periodic table
Common examples: Ag+ and Zn2+
Some monatomic ions have more than 1 ion possible (ie Cr2+ and Cr3+)
When naming compounds with more than 1 ion, must use Roman numerals in parentheses to indicate charge
EX: Fe2+ and Br- becomes FeBr2 and is called iron(II) bromide

9. Covalent (or Molecular) Nomenclature Rules
2 nonmetals bonded
1) Name it as you see it
2) Greek prefixes are used
3) 2nd element – drop ending and add –ide
4) if 1 is subscript in 1st element, don’t use mono-

10. Greek Prefixes:
Mono- 1
Di- 2
Tri- 3
Tetra- 4
Penta- 5
Hexa- 6
Hepta- 7
Octa- 8
Nona- 9
Deca- 10