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Chapter 6

Chapter 6. Formulas and Names of Compounds. 6 .1 Molecular Compounds and Formulas. Molecular Compounds = 2 or more elements joined by covalent bonds Generally 2 nonmetals Binary compounds = End in – ide Carbon Diox ide. Table of Prefixes (memorize me!).

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Chapter 6

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  1. Chapter 6 Formulas and Names of Compounds

  2. 6.1 Molecular Compounds and Formulas • Molecular Compounds = 2 or more elements joined by covalent bonds • Generally 2 nonmetals • Binary compounds = • End in –ide • Carbon Dioxide

  3. Table of Prefixes (memorize me!)

  4. Prefixes tell how many of each atom there are • Mono not used if there is only one of the first atom • Ending of 1st atom not changed • Ending of 2nd atom changed to -ide • CO2

  5. CO • H2O • Si3O6 • P2Cl5

  6. Use the name to write the formula! • Carbon Tetrachloride • Sulfur Hexaflouride • TetraphosphorusDecoxide • Dinitrogen Monoxide

  7. 6.2 Ions and Ionic Compounds • Ionic Compound = Metal + nonmetal • Name metal1st! • Change ending of nonmetal to -ide • NaCl • KF

  8. Nothing fancy, just name it! • K2S • MgO • CaCl2 • Li3N

  9. Just naming it only works when combining a metal from the 1st two columns (s block)with a nonmetal. • Also Al3+Zn2+ Cd2+ Ni2+ Ag1+ • Most transition metals (d block) can have more than one charge

  10. 3.3 Ionic Compounds and Formula Units • All ionic compounds are neutral so total + must equal total – • Calcium Chloride • Ca = • Cl =

  11. Formula Unit • Chemical formula for an ionic compound • Always uses smallest whole – number ratio • Na2Cl2 • Na8Cl8

  12. Crisscross method • Write the cation and anion as symbols with their charges. • Sn4+ O2- • Cross the number so they become subscripts • Sn2O4 • Reduce if needed. • SnO2

  13. Aluminum Sulfide • Sodium Phosphide • Calcium Nitride • Barium Oxide

  14. Naming with transition metals • Transition metals can have more than one charge • Which charge the ion has is indicated by roman numerals • Iron (II) Oxide • Copper (I) Chloride

  15. Common Ions • Fe2+ , Fe3+ • Cr2+ , Cr3+ • Co2+ , Co3+ • Ni2+ , Ni3+ • Cu1+ , Cu2+ • Hg1+ , Hg2+ • Au1+ , Au3+

  16. Fe2O3 • CuCl2 • CoN • Hg3P2

  17. Iron (III) Iodide • Titanium (III) Oxide • Chromium (III) Sulfide • Copper (I) Chloride

  18. 6.4 Polyatomic Ions & Formula Units • Polyatomic ion = group of atoms that act as one ion and has one charge • Name it the way you do regular ions • NaNO3 • CuCO3

  19. NaCO3 • MgSO4 • Al(ClO3)3 • Fe3(PO4)2

  20. Lead (II) phosphate • Magnesium perchlorate • Ammonium nitrate • Ammonium sulfide

  21. Naming Acids • Acid = Produces H+ when dissolved in water • H + Halogen • Hydro __________ ic acid • H + Polyatomic Ion • Ion ending in –ite = _________ous acid • Ion ending in –ate = _________ic acid

  22. HCl • HBr • HNO2 • H3PO4

  23. Nitric Acid • Sulfuric Acid

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