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Nomenclature

Nomenclature. Honors Coordinated Science II Wheatley-Heckman. Ionic Compounds. Held together by ionic bonds. What are ionic bonds? Between metals and non-metals Transfer of electrons between atoms. Attraction between oppositely charged ions. Ionic Compounds. Some examples are: NaCl

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Nomenclature

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  1. Nomenclature Honors Coordinated Science II Wheatley-Heckman

  2. Ionic Compounds • Held together by ionic bonds. • What are ionic bonds? • Between metals and non-metals • Transfer of electrons between atoms. • Attraction between oppositely charged ions.

  3. Ionic Compounds • Some examples are: • NaCl • MgCl2 • KBr • LiO2 • These are all bonds between cations (positive ions) and anions (negative ions).

  4. Naming Ionic Compounds • Binary Ionic Compounds • The metal will be your cation. Its name comes first. • The non-metal will be your anion. Its name comes second, but undergoes a slight change. • Change the ending to –ide. • Example: Chlorine  Chloride, Nitrogen  Nitride • LiO2 Lithium + Oxygen = Lithium Oxide

  5. Practice • Name the following ionic compounds: • NaCl • Rb2S • BeF2 • Cs3N • KI • In ionic compounds, the subscripts do NOT affect the name of the compound.

  6. Naming Ionic Compounds • Polyatomic Ions • Ions made of multiple atoms. • Name using an ion chart, but otherwise name the same as binary compounds. • Examples: • MgCO3 = Magnesium Carbonate • (NH4)SO4 = Ammonium Sulfate

  7. Writing Formulas from Names • The key to writing correct ionic formulas is to balance your positive and negative charges. We want a neutral molecule. • The charge of the cation becomes the subscript of the anion . • The charge of the anion becomes the subscript of the cation.

  8. Writing Formulas From Names • Sodium Chloride • Sodium = Na+, Chlorine = Cl- Na1Cl1 NaCl

  9. Writing Formulas from Names • Magnesium Fluoride • Magnesium = Mg2+, Fluorine = Fl- Mg1Fl2 MgFl2 **Do not include the charge in your formula.

  10. Why does this work? • Magnesium Fluoride Magnesium Fluorine -1 2+ -1 2 + -2 = 0

  11. Ionic Naming using Transition Metals • The charges of transition metals can vary. • A metal can have different charges depending on the situation. • You can use the formula to determine its charge in a specific molecule.

  12. Example #1 • CuI2 • We know Iodine has a charge of -1, but we have to determine the charge of copper. Copper Iodine +? -1 So… the charge of Copper in this molecule must be +2. The name is written: Copper (II) Chloride -1 ____ + -2 = 0

  13. Example #2 Chlorine Manganese • Mn2Cl4 +? -1 +? -1 We are trying to find the charge of one Manganese atom. The charge of one Manganese atom is +2, so the formula for Mn2Cl4 is: Manganese (II) Chloride -1 -1 2 x ? + -4 = 0

  14. Writing Names from Formulas • You can write the name for ionic compounds using transition metals the same as ionic compounds using alkali or alkaline earth metals. Mercury (I) Sulfide Mercury = Hg+, Sulfur = S2- Hg2S

  15. Molecular Compounds • Held together by Covalent bonds. • Between non-metals. • Sharing of electrons • Examples: • H2O • C2H4 • SO

  16. Naming Molecular Compounds • Begin by writing the name as you would a binary ionic compound. • Add prefixes to each name which tell you how many of that atom are in the molecule. • If there is only one atom of the first element in the molecule you can leave out the “mono” prefix. Prefix Definitions Mono = 1 Di = 2 Tri = 3 Tetra = 4 Penta = 5 Hexa = 6 Hepta = 7 Octa = 8 Nona = 9 Deca = 10

  17. Practice • P2S3 • H2O • CO • N2O4

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