1 / 11

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

ulric-boyd
Download Presentation

Chemical Nomenclature

An Image/Link below is provided (as is) to download presentation Download Policy: Content on the Website is provided to you AS IS for your information and personal use and may not be sold / licensed / shared on other websites without getting consent from its author. Content is provided to you AS IS for your information and personal use only. Download presentation by click this link. While downloading, if for some reason you are not able to download a presentation, the publisher may have deleted the file from their server. During download, if you can't get a presentation, the file might be deleted by the publisher.

E N D

Presentation Transcript

  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 and ferric) • Lead (plumbous and plumbic) • Mercury (Mercurous and Mercuric) • Nickel (Nickelous and Nickelic) • Chromium (Chromous and Chromic) • Manganese (Manganous and Manganic) • Cobalt (Cobaltous and Cobaltic) • Tin (Stannous and Stannic) • Antimony (Antimonious and Antimonic) • Copper (Cuprous and Cupric)

  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

More Related