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Nomenclature

Nomenclature. Naming Compounds: Covalent. Name in order, the second element gets the -ide ending Each element has “prefix”- refers to how many atoms of that element there are Note : drop mono for first element Ex: N 2 O 4 dinitrogen tetraoxide Ex: CO 2 carbon dioxide. Practice.

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Nomenclature

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  1. Nomenclature

  2. Naming Compounds: Covalent • Name in order, the second element gets the -ide ending • Each element has “prefix”- refers to how many atoms of that element there are Note: dropmonoforfirstelement Ex: N2O4 dinitrogen tetraoxide Ex: CO2 carbon dioxide

  3. Practice Give the corresponding name or formula • Carbon tetrafluoride • CF4 • P2O5 • Diphosphorous pentoxide • N2O • Dinitrogen monoxide • CO • Carbon monoxide

  4. Ionic Compounds: Formula • We can determine the formula of a compound by using the criss cross method using the ion charges • E.g. what compound would form from Ca + S? Step 1 - write ion charge: Ca2+S2- Step 2 - cross down ion charge: Ca2S2 Step 3 – reduce: CaS

  5. Practice! • Write the chemical formula for the following: • Al and Br • AlBr3 • K and S • K2S • Mg and N • Mg3N2 • Be and O • BeO • Cu and Cl • CuCl or CuCl2

  6. Ionic compounds: Naming • Metal (cation) first then non-metal • Non-metal ends in -ide. • Example: sodium chloride Give formulae & name: • Ca + I • CaI2 calcium iodide • O + Mg • MgO magnesium oxide • Na + S • Na2S = sodium sulfide

  7. Multivalent (more than one charge) Often transition metals These you will need to know: Iron Fe2+ Fe3+ Tin Sn2+ Sn4+ Lead Pb2+ Pb4+ Copper Cu1+ Cu2+ Multivalent Metals

  8. Multivalent Metals: Naming method 1 • Stock System – the charge of the multivalent ion is indicated as a Roman numeral after the name of the metal is written • Ex: Fe2O3 iron (III) oxide • Ex: CuCl2 copper (II) chloride Note: Metals in groups 1, 2, 3 or Ag+, Al3+, Zn2+, exist with only one charge, therefore Roman numerals are not used when naming them.

  9. Multivalent Metals: Naming method 2 • Classical System – using latin stems and one of two endings. • - ic  bigger charge • - ous  smaller charge • Ex: Fe3+ = ferric Fe2+ = ferrous Sn2+ = stannic Sn4+ = stannous Pb2+ = plumbic Pb4+= plumbous Cu1+ = cupric Cu2+ = cuprous • Ex: Fe2O3 is ferric oxide

  10. Polyatomic Ions • Polyatomic ions are a series, most often two or more elements that are combined together with just one over all charge. • They interact as a single unit • To recognize if a compound has a polyatomic ion: if there are at least three (3) elements in the compound. • The positive ion is named first (check to see if it is a multivalent ion or is ammonium, NH41+). This followed by the named of the negative polyatomic ion

  11. Polyatomic Ions to Know • NO2- nitrite • NO3- nitrate • SO32- sulphite • SO42- sulphate • CO32- carbonate • PO43- phosphate • HCO3- hydrogen carbonate • OH- hydroxide • NH4+ ammonium

  12. Tricks for Polyatomic Ions with Oxygen • You can substitute other elements in for Cl

  13. Practice! Write the corresponding name or formula: • Ca(OH)2 • Calcium hydroxide • Magnesium sulphite • MgSO3 • Ammonium hydroxide • NH4OH • Fe(NO3)2 • Iron (II) Nitrate

  14. Acids • A compound that contains hydrogen and has special properties • Must be in an aqueous state (aq) – dissolved in water • 2 types of acids • Binary acids • oxyacids

  15. Naming Acids: Binary Acids • Binary: H + non-metal • Ex: HCl Binary acids: naming depends on state of acid • If it’s not aqueous: hydrogen + non-metal HCl(g) = hydrogen chloride • If it is aqueous: hydro + non-metal + ic acid HCl(aq) = hydrochloric acid Ex: HBr(aq) is hydrobromic acid

  16. Naming Acids: Oxyacids • Oxyacids: H + polyatomic ion • Ex: H2SO4 • name the polyatomic ion • Replace: ate  ic, ite  ous • add “acid” to the name E.g. H2NO3 • Nitrate  Nitric • Nitric acid

  17. Practice • H3PO4(aq) • Phosphoric acid • Hypochlorous acid • HClO(aq) • H2SO3(aq) • Sulphurous acid • Carbonic Acid • H2CO3(aq)

  18. Hydrates • Some compounds contain H2O in their crystal lattice structure. These compounds are called hydrates. • The H2O can usually be removed if heated. • A dot () separates water • Ex: CuSO4•5H2O • Name as usual, then a prefix + “hydrate” indicates the # of H2O groups. • Ex: CuSO4•5H2O is copper(II) sulfate pentahydrate sodium sulfate decahydrate nickel(II) sulfate hexahydrate Na2CO3•H2O BaCl2•2H2O Na2SO4•10H2O NiSO4•6H2O sodium carbonate monohydrate barium chloride dihydrate

  19. Practice! Homework!! • Nomenclature Worksheets

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