1. NAMING IONIC COMPOUNDS

2. Naming Binary Ionic Compounds • Binary ionic compounds contain only 2 types of elements. CaCl2 1. Name cation first. Cation name is the name of the element. • Ca2+ = calciumion 2. Name anion second. Anion name is the name of the element with ending changed to –ide. Anion = root + -ide Chlorine = Chloride 3. Combine names. The cation is always listed 1st. CaCl2= calcium chloride

3. Common Anion Names • Fluorine • Fluoride • Chlorine • Chloride • Bromine • Bromide • Iodine • Iodide • Oxygen • Oxide • Sulfur • Sulfide • Nitrogen • Nitride • Phosphorus • Phosphide

4. Naming Ionic Compounds With Transition Metals • Use Roman numeralto represent charge in name. Determine charge based on TOTAL charge of anions. • NOTE: If metal is not aluminum or a group 1 or 2 element, it must have a Roman numeral. • PbCl2 • Pb2+is cation • PbCl2 = lead (II) chloride

5. Naming Ionic Compounds with Polyatomic Ions • Polyatomic ions are groups of bonded atoms that have an overall charge. • Use regular name of polyatomic ion. • Mg3(PO4)2 • PO43-is phosphate • Mg3(PO4)2 = magnesium phosphate

6. Common Polyatomic Ions • Ammonium • NH4+ • Chlorate • ClO3- • Bicarbonate • HCO3- • Hydroxide • OH- • Cyanide • CN- • Nitrate • NO3- • Acetate • C2H3O2- • Sulfate • SO42- • Carbonate • CO32- • Phosphate • PO43-

7. Determining Formula from Name Iron (III) Carbonate • 1. Write formula of cation. • If cation is a transition metal, use Roman numeral to determine charge. • Fe3+ • 2. Write formula of anion. • CO32- • 3. Criss-cross charges to determine formula. • Fe2(CO3)3