1. Chemistry

2. Transition Metals  can have more than one charge  charge of ion is shown in parenthesis as a roman numeral  (I) = +1  (II) = +2  (III) = +3  (IV) = +4  (V) = +5  Common Ion Table – on the back of your periodic table

3. Polyatomic Ions  The charge is given to the entire group of atoms that are bonded to each other (have covalent bonds)  act as an individual atom  NEVER change their subscripts – use parenthesis around the ion

4. Ionic Formula Writing Examples  use the criss-cross method  use parenthesis around polyatomic ions  examples:  Ag +1 OH -1  Mg +2 SO 4 -2  NH 4 +1 CO 3 -2

5. Naming Ionic Compounds  Compounds with polyatomic ions  name cation  name anion  Compounds with transition metals  determine charge of cation (reverse of criss-cross method)  name cation followed by the charge in roman numerals in parenthesis  name anion (-ide)

6. Naming Ionic Compounds Examples  Polyatomic Ions  Ba(NO 3 ) 2  (NH 4 ) 2 O  Transition Metals  FeCl 2  CuBr

7. Counting Atoms  Subscripts tell how many atoms of each element are present  If a formula has parenthesis with a number on the outside of the parenthesis (subscript), then use the distributive property (like math class)  If the formula has a large number in front of the formula (coefficient), then use the distributive property (like math class)

8. Counting Atoms Examples  2 H 2 SO 4  Fe(NO 3 ) 2  3 Be(CN) 2  4 Ba(NO 3 ) 2