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Chemical Names and Formulae

Chemical Names and Formulae. SNC1P Mr. M. Couturier. Chemical Names. IUPAC is the International Union of Pure and Applied Chemistry which sets the standards of chemistry, which includes naming chemicals. A few definitions.

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Chemical Names and Formulae

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  1. Chemical Names and Formulae SNC1P Mr. M. Couturier

  2. Chemical Names • IUPAC is the International Union of Pure and Applied Chemistry which sets the standards of chemistry, which includes naming chemicals.

  3. A few definitions • A binary compound is a compound that contains two different elements. • A polyatomic ion consists of two or more different non-metal atoms, which are joined by covalent bonds.

  4. Metal+Non-Metal Compounds • When naming a compound with a metal and a non-metal, you must: • Name the metal first • Name the non-metal next but add the suffix –ide.

  5. Metal+Non-Metal Compounds • Examples: Complete the chemical compound using electron diagrams and then name it. • Na and Cl: • K and S: • Mg and N: • Li and C: • Ca and Br: • Ba and F:

  6. Metal+Non-Metal Compounds • Examples: • Na and Cl: NaCl sodium chloride • K and S: K2S potassium sulfide • Mg and N: Mg3N2 magnesium nitride • Li and C: Li4C lithium carbide • Ca and Br: CaBr2 calcium bromide • Ba and F: BaF2 barium fluoride

  7. Metal+Non-Metal Compounds • Note that regardless of the number of atoms present, the name of the compound is simply named by the metal and the non-metal (with the –ide suffix). However, this is only true when dealing with metals that are only willing to give a specific number of electrons. For example, calcium always gives 2 electrons. However, this is not always the case with transition metals.

  8. Metal+Non-Metal Compounds • When looking at the periodic table you will note that there is an “ionic charge” listed. For example, Fe can sometimes give 2 electrons (forming the cation Fe2+) and sometimes it gives 3 electrons (forming the cation Fe3+).

  9. Metal+Non-Metal Compounds

  10. Metal+Non-Metal Compounds • Examples: Given the cation, determine the compound formed as well as it name. • Fe2+ and S: • Cu2+ and N: • Fe2+ and F: • Fe3+ and F: • Hg+ and Br: • Hg2+ and Br:

  11. Metal+Non-Metal Compounds • Examples: Given the cation, determine the compound formed as well as it name. • Fe2+ and S: FeS iron (II) sulfide or ferrous sulfide • Cu2+ and N: Cu3N2 copper (II) nitride or cupric nitride • Fe2+ and F: FeF2 iron (II) fluoride or ferrous fluoride • Fe3+ and F: FeF3 iron (III) fluoride or ferric fluoride • Hg+ and Br: Hg2Br2 mercury (I) bromide or mercurous bromide • Hg2+ and Br: HgBr2 mercury (II) bromide or mercuric bromide

  12. Metal+Non-Metal Compounds • TRICK: The suffix –ous is used for the lower charge whereas the suffix –ic is used for the higher charge.

  13. Metal+Non-Metal Compounds

  14. Non-Metal Compounds • When naming a compound with a non-metals you must: • Name the leftmost element first • Add the suffix –ide to the next element • Add Greek prefixes for the numbers of atoms (except if the first element only has one)

  15. Greek class

  16. Non-Metal Compounds • Examples: Given the following non-metals, determine the compound formed as well as it name. • NO • N2O • NO2 • N2O5 • N2O3

  17. Non-Metal Compounds • Examples: Given the following non-metals, determine the compound formed as well as it name. • NO nitrogen monoxide • N2O dinitrogen monoxide • NO2 nitrogen dioxide • N2O5 dinitrogen pentoxide • N2O3 dinitrogen trioxide

  18. Polyatomic Ions • When naming a compound with one or more polyatomic ions, you must: • Name the cation first • Name the anion second

  19. Polyatomic Ions

  20. Polyatomic Ions • Examples: • Ammonium cyanide: • [NH4+] + [CN-] • (NH4)CN • Ammonium hydroxide: • [NH4+] + [OH-] • (NH4)OH

  21. Polyatomic Ions • Examples: • Barium sulfate: • [Ba2+] + [SO42-] • BaSO4 • Iron (II) nitrate OR ferrous nitrate • [Fe2+] + [NO3-] • Fe(NO3)2

  22. Polyatomic Ions

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