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Chemical Nomenclature

Chemical Nomenclature. according to IUPAC the I nternational U nion of P ure and A pplied C hemistry. Made of 2 element Metal bonded to nonmetal Metallic cations have the same name as the metal

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Chemical Nomenclature

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

  2. Made of 2 element Metal bonded to nonmetal 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. Or the Latin System using a Latin root and suffix. Lower oxidation state – ous Higher oxidation state – ic Nonmetal anions: drop the ending and add –ide. The Rule: Unchanged cation name + anion name (drop ending) + ide Examples: NaCl: Sodium chloride CaBr2 : Calcium bromide Multiple oxidation states FeS: Iron (II) sulfide or Ferrous sulfide Fe2S3: Iron (III) sulfide Ferric sulfide Binary Ionic Compounds

  3. Other Elements that use the Latin System • Iron (ferrous, +2 and ferric, +3) • Lead (plumbous, +2 and plumbic, +4) • Mercury (Mercurous, +1 and Mercuric, +2) • Nickel (Nickelous, +2 and Nickelic, +3) • Chromium (Chromous, +2 and Chromic , +3) • Manganese (Manganous, +2 and Manganic, +4) • Cobalt (Cobaltous, +2 and Cobaltic, +3) • Tin (Stannous, +2 and Stannic, +4) • Antimony (Antimonious, +3 and Antimonic, +5) • Copper (Cuprous, +1 and Cupric, +2)

  4. Made of 2 elements 2 Nonmetals bonded 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. Rule of double vowel contraction: Drop the -a or -o before an -a or –o. Keep all other double vowels. Example: Pentoxide not pentaoxide Example: Diiodide not diodide Examples: CO2 : Carbon dioxide N205: Dinitrogenpentoxide Prefixes: Mono- Di- Tri- Tetra- Penta- Hexa- Hepta- Octa- Nona- Deca- Enna- Dodeca- Binary Covalent Compounds

  5. Ternary Compounds • Made of 3 or more elements • Ternary compounds – compounds of polyatomic ions • Polyatomic ions – ions made of more than one atom The Rule: • Cation name + anion name. • Examples: • KNO3 • Postassium nitrate • Rb2SO4 • Rubidium sulfate • Metals with multiple oxidation states • Pb3(PO3)2 • Lead (II) phosphite • Or Plumbousphosphite • Pb3(PO3)4 • Lead (IV) phosphite • Or Plumbic phosphite

  6. Binary Acids • Made of 2 elements (hydrogen and one other element) • Acid – hydrogen compounds of an monoatomic anion in water solution • Binary acids – acids made of two elements • Acids whose names end in –ide • Rule: • Add hydro to the beginning of the nonmetal’s name drop the ending and add –ic acid. • Hydro (nonmetal root) ic acid • Examples: • HCl • Hydrogen chloride (if pure substance) = hydrochloric acid (in water) • H2S • Hydrogen sulfide (if pure substance) = hydrosulfuric acid (in water)

  7. Ternary Acids • Ternary acid – hydrogen compounds of polyatomic anions in water solution • Acids whose names end in –ite or –ate • Rule: • If the ending is –ite, replace it with –ous acid • If the ending is –ate, replace it with –ic acid\ • Do not use hydro- at the beginning • Examples: • H2SO4 is sulfuric acid not hydrosulfuric acid • HNO2 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 • Example: • ClO-1 hypochlorite (assigned to lowest oxidation state of nonmetal) • ClO2-1 chlorite • ClO3-1 chlorate • ClO4-1 perchlorate (assigned to highest oxidation state of nonmetal) • Series oxoanions: (usually) • If 1 in the series use -ate • If 2 in the series use -ate and –ite • If 3 in the series use -ate, -ite, and per___ate • 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 • Examples • PO4-3 Phosphate ion • HPO4-2Monohydrogen phosphate ion or hydrogen phosphate ion • H2PO4-1 Dihydrogen phosphate ion or bihydrogen phosphate

  9. Other Polyatomic Ion Rules • Some polyatomic ions end in –ide by convention • OH-1 hydroxide • CN-1 cyanide • N3-1 azide • Polyatomic ions of the same element • Add per- • O-2 is oxide • O2-2 is peroxide • S-2 is sulfide • S2-2 is persulfide • Polyatomic cations formed from nonmetals end –ium • Examples • NH4+1 – Ammonium • H30+1 – Hydronium

  10. Hydrates • Compounds with water molecules surrounding the formula unit of the compound. • Rule: • Regular name + Prefix • hydrate • Example: MgSO4 • 7 H2O • Magnesium Heptahydrate

  11. Some Have Traditional Names by Convention • H2O – Water • PH3 – Phosphine • NH3 – Ammonia • N2H4 – Hydrazine • NO – Nitric Oxide • N2O – Nitrous Oxide

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