1 / 19

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.

acton
Télécharger la présentation

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. 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

More Related