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Nomenclature

Nomenclature. Naming Compounds. Ionic Compounds. Metal bonding with non-metal One atom gains electrons, one atom loses electrons Exist as ions with full highest energy levels. Are held together in a giant crystal by the electrostatic attraction of the opposite charges.

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Nomenclature

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  1. Nomenclature Naming Compounds

  2. Ionic Compounds • Metal bonding with non-metal • One atom gains electrons, one atom loses electrons • Exist as ions with full highest energy levels. • Are held together in a giant crystal by the electrostatic attraction of the opposite charges. • The metal is named first; the nonmetal gets “ide” at the end of it’s name. • Ex. CaCl2 Calcium chloride

  3. There is no real bond between the ions. There is just strong attraction between the opposite charges. - - + + - + + - - + - - + + -

  4. Metals Non-Metals Rule #1

  5. Writing Ionic Formulas • Determine the charge on each ion. • Find the lowest common multiple that will balance the charge. ex. Calcium Chloride Ca+2 Cl- +2 x2=-2 (to balance the charge) CaCl2

  6. Try theseMetal & Non-metal Sodium phosphide Magnesium telluride Lithium chloride Barium carbide Strontium arsenide

  7. Ionic Compounds part II • The transition metal is named first with a Roman numeral to indicate the charge on the ion; the nonmetal gets “ide” at the end of its name.

  8. Transition Metals

  9. Non- metals Rule #2 Transition Metals

  10. Non- metals Rule #2 Transition Metals

  11. What is the name of CuO ? We know that oxygen has a charge of –2. Therefore, copper must have a charge of +2. We must indicate the charge of the transition metal. Copper (II) oxide

  12. Try these:Transition Metal & Non-metal Fe3N2 NiBr3 CoCl2 HgI SnS2

  13. Try these:Transition Metal & Non-metal Fe3N2 Iron was multiplied by 3 and nitrogen (-3) was multiplied by 2 (-6) so that the charges would balance. The charge on Iron must have been +2. Iron (II) nitride

  14. Try these:Transition Metal & Non-metal NiBr3 The charge (from the periodic table) on Br is –1. Br was multiplied by 3 (hence the subscript), so the charge on Nickel MUST be +3. Nickel (III) Bromide

  15. Try these:Transition Metal & Non-metal CoCl2 The charge (from the periodic table) on Cl is –1. Chlorine was multiplied by 2 (hence the subscript), so the charge on Cobalt MUST be +2. Cobalt (II) Chloride

  16. Try these:Transition Metal & Non-metal HgI The charge (from the periodic table) on I is –1. Iodine was not multiplied by anything (no subscript), so the charge on Mercury MUST be +1. Mercury (I) Iodide

  17. Try these:Transition Metal & Non-metal MnO2 The charge (from the periodic table) on O is –2. Oxygen was multiplied by 2 (hence the subscript), so the charge on Manganese MUST be +4. Manganese (IV) Oxide

  18. Formula writing with transition metals Simple! ex. Nickel (II) Iodide The charge on the nickel ion is obviously +2. The charge on iodide is always -1. Therefore, the formula is: NiI2

  19. Ionic Compounds part III • Bonding with a Polyatomic ion • The metal is named first; the polyatomic anion is named second (a polyatomic cation is named first). Ex. Li3PO4 Lithium phosphate

  20. Polyatomic Ions thatwe use in science 10: hydroxide sulfate nitrate carbonate phosphate ammonium chlorate OH-1 SO4-2 NO3-1 CO3-2 PO4-3 NH4+1 ClO3-1

  21. Try these:Polyatomic Ion NaOH K2SO4 Ba(NO3)2 CuCO3 Li3PO4 NH4Cl

  22. Try these: Sodium Hydroxide Potassium Sulfate Barium Nitrate Copper(II) Carbonate Lithium Phosphate Ammonium Chlorate NaOH K2SO4 Ba(NO3)2 CuCO3 Li3PO4 NH4ClO3

  23. Writing Formulas Calcium sulfate Potassium carbonate Ammonium hydroxide Iron (III) chlorate Copper (I) phosphate Zinc sulfate

  24. Ionic BondingvsMolecular Bonding Makes "Compounds”vsMakes "Molecules" Transfers electronsvsShares electrons Metals & NonmetalsvsMade of Nonmetals Positive & NegativevsNeutral Weak BondvsStrong bond NaCl KOH CaCl2vs H2O CO2 NH3CH4

  25. Prefixes • Mono • Di • Tri • Tetra • Penta • Hexa • Hepta • Octa • Nona • Deca Molecular Compounds • Non-metals bond with non-metals. • Atoms share electrons. • The number of each atom present is indicated by a prefix. • Add “ide” to the end of the second atom’s name.

  26. Non- metals Rule #3

  27. ex. N2Odinitrogen monoxide NO nitrogen monoxide N2O3dinitrogen trioxide NO2nitrogen dioxide * N2O4dinitrogentetroxide N2O5dinitrogenpentoxide

  28. ex. N2Odinitrogenmonoxide NO nitrogenmonoxide N2O3dinitrogentrioxide NO2nitrogen dioxide* N2O4dinitrogentetroxide N2O5dinitrogenpentoxide * When the first atom is singular, the prefix “mono” is not used.

  29. Try These:Non-metal & Non-metal sulfur trioxide xenon hexafluoride krypton difluoride bromine pentachloride sulfur tetrachloride phosphorus trifluoride tetrarsenicdecoxide dinitrogen trioxide SO3 XeF6 KrF2 BrCl5 SCl4 PF3 As4O10 N2O3

  30. Writing Formulas • Write each atom’s symbol with a subscript equal to the prefix. Ex. Hexaphosphorus tribromide P6Br3 Pentatellurium mononitride Te5N

  31. Try these dinitrogen pentasulfide carbon monoxide heptasulfur trioxide xenon hexafluoride trisulfur hexafluoride phosphorus pentachloride nitrogen monoxide dibismuth trichloride

  32. Try these dinitrogen pentasulfideN2S5 carbon monoxideC0 heptasulfur trioxideS7O3 xenon hexafluorideXeF6 trisulfur hexafluorideS3F6 phosphorus pentachloridePCl5 nitrogen monoxide NO dibismuth trichlorideBi2Cl3

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