1. Chemical Nomenclature according to IUPACthe International Union of Pure and Applied Chemistry

2. Binary Ionic Compounds Made of 2 element Made of 2 element Metal bonded to nonmetal Metal bonded to nonmetal Metallic cations have the same name as the metal Metallic cations have the same name as the metal If a metal can form different oxidation states use a Roman Numeral, known as Stock System, following the metal name to indicate the oxidation state. If a metal can form different oxidation states use a Roman Numeral, known as Stock System, following the metal name to indicate the oxidation state. Or the Latin System using a Latin root and suffix. Or the Latin System using a Latin root and suffix. Lower oxidation state – ous Lower oxidation state – ous Higher oxidation state – ic Higher oxidation state – ic Nonmetal anions: Nonmetal anions: drop the ending and add –ide. drop the ending and add –ide. The Rule: Unchanged cation name + anion name (drop ending) + ide Examples: NaCl: Sodium chloride CaBr 2 : Calcium bromide Multiple oxidation states FeS: Iron (II) sulfide or Ferrous sulfide Fe 2 S 3 : Iron (III) sulfide Ferric sulfide

3. Other Elements that use the Latin System Iron (ferrous and ferric) Iron (ferrous and ferric) Lead (plumbous and plumbic) Lead (plumbous and plumbic) Mercury (Mercurous and Mercuric) Mercury (Mercurous and Mercuric) Nickel (Nickelous and Nickelic) Nickel (Nickelous and Nickelic) Chromium (Chromous and Chromic) Chromium (Chromous and Chromic) Manganese (Manganous and Manganic) Manganese (Manganous and Manganic) Cobalt (Cobaltous and Cobaltic) Cobalt (Cobaltous and Cobaltic) Tin (Stannous and Stannic) Tin (Stannous and Stannic) Antimony (Antimonious and Antimonic) Antimony (Antimonious and Antimonic) Copper (Cuprous and Cupric) Copper (Cuprous and Cupric)

4. Binary Covalent Compounds Made of 2 elements Made of 2 elements 2 Nonmetals bonded 2 Nonmetals bonded Element farthest to the left in the Periodic Table is the positive oxidation state. Element farthest to the left in the Periodic Table is the positive oxidation state. Prefix to indicate number of atoms + unchanged nonmetal with the positive oxidation state + prefix to indicate number of atoms + nonmetal with negative oxidation state (drop ending) + ide. Prefix to indicate number of atoms + unchanged nonmetal with the positive oxidation state + prefix to indicate number of atoms + nonmetal with negative oxidation state (drop ending) + ide. Rule of double vowel contraction: Rule of double vowel contraction: Drop the -a or -o before an -a or – o. Drop the -a or -o before an -a or – o. Keep all other double vowels. Keep all other double vowels. Example: Pentoxide not pentaoxide Example: Pentoxide not pentaoxide Example: Diiodide not diodide Example: Diiodide not diodide Examples: CO 2 :Carbon dioxide N 2 0 5 : Dinitrogen pentoxide Prefixes: Mono- Di- Tri- Tetra- Penta- Hexa- Hepta- Octa- Nona- Deca- Enna- Dodeca-

5. Ternary Compounds Made of 3 or more elements Made of 3 or more elements Ternary compounds – compounds of polyatomic ions Ternary compounds – compounds of polyatomic ions Polyatomic ions – ions made of more than one atom Polyatomic ions – ions made of more than one atom The Rule: Cation name + anion name. Cation name + anion name. Examples: Examples: KNO 3 KNO 3 Postassium nitrate Postassium nitrate Rb 2 SO 4 Rb 2 SO 4 Rubidium sulfate Rubidium sulfate Metals with multiple oxidation states Metals with multiple oxidation states Pb 3 (PO 3 ) 2 Pb 3 (PO 3 ) 2 Lead (II) phosphite Lead (II) phosphite Or Plumbous phosphite Or Plumbous phosphite Pb 3 (PO 3 ) 4 Pb 3 (PO 3 ) 4 Lead (IV) phosphite Lead (IV) phosphite Or Plumbic phosphite Or Plumbic phosphite

6. Binary Acids Made of 2 elements (hydrogen and one other element) Made of 2 elements (hydrogen and one other element) Acid – hydrogen compounds of an monoatomic anion in water solution Acid – hydrogen compounds of an monoatomic anion in water solution Binary acids – acids made of two elements Binary acids – acids made of two elements Acids whose names end in –ide Acids whose names end in –ide Rule: Rule: Add hydro to the beginning of the nonmetal’s name drop the ending and add –ic acid. Add hydro to the beginning of the nonmetal’s name drop the ending and add –ic acid. Hydro (nonmetal root) ic acid Hydro (nonmetal root) ic acid Examples: Examples: HCl HCl Hydrogen chloride (if pure substance) = hydrochloric acid (in water) Hydrogen chloride (if pure substance) = hydrochloric acid (in water) H 2 S H 2 S Hydrogen sulfide (if pure substance) = hydrosulfuric acid (in water) Hydrogen sulfide (if pure substance) = hydrosulfuric acid (in water)

7. Ternary Acids Ternary acid – hydrogen compounds of polyatomic anions in water solution Ternary acid – hydrogen compounds of polyatomic anions in water solution Acids whose names end in –ite or –ate Acids whose names end in –ite or –ate Rule: Rule: If the ending is –ite, replace it with –ous acid If the ending is –ite, replace it with –ous acid If the ending is –ate, replace it with –ic acid\ If the ending is –ate, replace it with –ic acid\ Do not use hydro- at the beginning Do not use hydro- at the beginning Examples: Examples: H 2 SO 4 is sulfuric acid not hydrosulfuric acid H 2 SO 4 is sulfuric acid not hydrosulfuric acid HNO 2 is nitrous acid not hydronitrous acid HNO 2 is nitrous acid not hydronitrous acid

8. Polyatomic Oxoanion Rules Oxygen can form a series of polyatomic oxoanions formed from nonmetals and end in –ite and –ate Oxygen can form a series of polyatomic oxoanions formed from nonmetals and end in –ite and –ate Example: Example: ClO -1 hypochlorite (assigned to lowest oxidation state of nonmetal) ClO -1 hypochlorite (assigned to lowest oxidation state of nonmetal) ClO 2 -1 chlorite ClO 2 -1 chlorite ClO 3 -1 chlorate ClO 3 -1 chlorate ClO 4 -1 perchlorate (assigned to highest oxidation state of nonmetal) ClO 4 -1 perchlorate (assigned to highest oxidation state of nonmetal) Series oxoanions: (usually) Series oxoanions: (usually) If 1 in the series use -ate If 1 in the series use -ate If 2 in the series use -ate and –ite If 2 in the series use -ate and –ite If 3 in the series use -ate, -ite, and per___ate If 3 in the series use -ate, -ite, and per___ate If 4 in the series use -ate, -ite, per___ate, and hypo____ite If 4 in the series use -ate, -ite, per___ate, and hypo____ite An additional series of ions can be formed by adding hydrogen to oxoanoins An additional series of ions can be formed by adding hydrogen to oxoanoins Examples Examples PO 4 -3 Phosphate ion PO 4 -3 Phosphate ion HPO 4 -2 Monohydrogen phosphate ion or hydrogen phosphate ion HPO 4 -2 Monohydrogen phosphate ion or hydrogen phosphate ion H 2 PO 4 -1 Dihydrogen phosphate ion or bihydrogen phosphate H 2 PO 4 -1 Dihydrogen phosphate ion or bihydrogen phosphate

9. Other Polyatomic Ion Rules Some polyatomic ions end in –ide by convention Some polyatomic ions end in –ide by convention OH -1 hydroxide OH -1 hydroxide CN -1 cyanide CN -1 cyanide N 3 -1 azide N 3 -1 azide Polyatomic ions of the same element Polyatomic ions of the same element Add per- Add per- O -2 is oxide O -2 is oxide O 2 -2 is peroxide O 2 -2 is peroxide S -2 is sulfide S -2 is sulfide S 2 -2 is persulfide S 2 -2 is persulfide Polyatomic cations formed from nonmetals end –ium Polyatomic cations formed from nonmetals end –ium Examples Examples NH 4 +1 – Ammonium NH 4 +1 – Ammonium H 3 0 +1 – Hydronium H 3 0 +1 – Hydronium

10. Hydrates Compounds with water molecules surrounding the formula unit of the compound. Compounds with water molecules surrounding the formula unit of the compound. Rule: Rule: Regular name + Prefix hydrate Regular name + Prefix hydrate Example: MgSO 4 7 H 2 O Example: MgSO 4 7 H 2 O Magnesium Heptahydrate Magnesium Heptahydrate

11. Some Have Traditional Names by Convention H 2 O – Water H 2 O – Water PH 3 – Phosphine PH 3 – Phosphine NH 3 – Ammonia NH 3 – Ammonia N 2 H 4 – Hydrazine N 2 H 4 – Hydrazine NO – Nitric Oxide NO – Nitric Oxide N 2 O – Nitrous Oxide N 2 O – Nitrous Oxide