1. 9.1 Naming Ions Cations: metals in 1A,2A,3A charges = group #
Anions: group A nonmetals, group # -8
Transition metal ions (1B-8B) multiple cations/charges see table 9.1 Pg 255
Polyatomic ions end in –ite or –ate (have oxygen, -ite has 1 less oxygen then –ate)see table 9.3 pg257
Write symbol/ charge and classify(anion/cation)
Arsenic:
Beryllium:

2. 9.2 Naming/Writing Formulas for ionic compounds
Binary compound: cation then anion
Cs2O= cesium oxide
Formulas: symbol for cation and then anion, use subscripts to balance charges
Cu2+ S2- =CuS
Compounds: uses parentheses
Calcium nitrate= Ca(NO3)2
Compounds of polyatomic ions
Sodium Perchlorate= NaClO4
Calcium Acetate= Ca(C2H3O2)2

3. 9.3 naming/writing formulas for molecular compounds
Naming: prefix tells how many atoms of each element
CO2= Carbon dioxide; 9.4 pg 269
Writing formulas: prefix tells you the subscript for each element
Diphospohorous trioxide= P O
Iodine heptafluoride= I F

4. 9.4 Naming/Writing formulas for acids/bases
Acid; pH 0-6; higher concentration of H+
1: If anion ends in –ide, acid names begins with hydro- and has suffix –ic, followed by acid
2:If anion name ends in –ite, acid name is stem with suffix –ous, followed by acid
3:If anion ends in in –ate, acid name is stem with suffix –ic, followed by acid.
Use rules in reverse to write formulas!
** Pg 272 rules printed in bold!

5. 9.4 cont’d Bases; pH 8-14; higher concentration OH-
Name: cation followed by anion
Just like ionic compounds
Name Acids:
HNO3
Name Bases:
Al(OH)3

6. 9.5 Laws Governing Formulas/Names
Law of Definite Proportions: in samples of any chemical compound, the masses of the elements are always in the same proportions (masses don’t change!)
H2O and H2O2; mass of H is for both
Law of Multiple Proportions: if same 2 elements form more than 1 compound, the different masses of 1 element combine with other element are a ratio
CO2 vs CO (12amu+32amu vs 12amu+16amu); ratio of oxygen is 2:1