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Naming Starts with Classifying Compounds (3 types)

Naming Starts with Classifying Compounds (3 types). • Binary Compounds = only 2 elements • Compounds containing polyatomic ions • Acids = formula often starts with H. Classifying Binary Compounds. Compounds containing a metal and a nonmetal are binary ionic

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Naming Starts with Classifying Compounds (3 types)

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  1. Naming Starts with Classifying Compounds (3 types) • Binary Compounds = only 2 elements • Compounds containing polyatomic ions • Acids = formula often starts with H

  2. Classifying Binary Compounds • Compounds containing a metal and a nonmetal are binary ionic • Compounds containing two nonmetals are molecular compounds • Compounds containing H and a nonmetal = Acids

  3. Binary Ionic Compounds (Fig. 5.1)

  4. Type IBinary Ionic Compounds • Contain Metal Cation + Nonmetal Anion • Metal listed first in formula & in compound name • Name metal cation first, name nonmetal anion second

  5. Type IBinary Ionic Compounds (cont.) • Metal cation name is the metal name • Nonmetal anion named by changing the ending on the nonmetal name to –ide • CaCl2 = calcium chloride

  6. Chemical Formulas • Identify the elements present • Element symbols • Identify the number of each atom • Subscripts • Aluminum sulfide Al2S3 • 2 Al atoms for every 3 S atoms

  7. Writing the Formulas from the Names • Determine the ions present • Determine the charges on the cation and anion • Balance the charges to get the subscripts

  8. Writing the Formulas from the Names (cont.) • Magnesium chloride • Mg2+ Cl- • Total positive charge must equal total negative charge • 1 Mg2+ will balance 2Cl- • MgCl2

  9. Compounds Containing Polyatomic Ions • Polyatomic ions are charged entities that contain more than one atom • Polyatomic compounds contain one or more polyatomic ions • Name polyatomic compounds by naming cation and anion • Al(C2H3O2)3 = aluminum acetate

  10. Patterns for Polyatomic Ions • Elements in the same column on the Periodic Table form similar polyatomic ions • same number of O’s and same charge ClO3- = chlorate  BrO3- = bromate

  11. Patterns for Polyatomic Ions (cont.) • If the polyatomic ion starts with H, add hydrogen- before the ions name and add 1 to the charge CO32- = carbonate  HCO3- = hydrogen carbonate

  12. Patterns for Polyatomic Ions (cont.) • -ate ion (chlorate = ClO3-) • -ate ion plus 1 O same charge, per- prefix (perchlorate = ClO4-) • -ate ion minus 1 O same charge, -ite suffix (chlorite = ClO2-) • -ate ion minus 2 O same charge, hypo- prefix, -ite suffix (hypochlorite = ClO-)

  13. Type IIBinary Ionic Compounds • Contain Metal Cation (metal with more than one possible charge) + Nonmetal Anion • Same format as for Type I • Use a roman numeral after the cation to indicate the charge

  14. Type IIBinary Ionic Compounds (cont.) • FeCl3 • Fe  iron • Cl  chloride • Total negative charge = Cl- x 3 = 3- • Need +3 to balance • Have only one Fe  Fe+3

  15. Type IIBinary Ionic Compounds (cont.) • FeCl3 = Iron (III) chloride

  16. Determining the Charge on a Cation – Au2S3 • Determine the charge on the anion • Sulfide = -2 • Determine the total negative charge • (-2) x 3 = -6 • Total positive charge = total negative charge • Divide total positive charge by the number of cations • +6/2 = +3

  17. Gold (III) sulfide

  18. Type IIBinary Ionic Compounds (cont.) • Old naming system • Uses root name or latin name for metal • Uses suffixes instead of roman numerals

  19. Type IIBinary Ionic Compounds (cont.) • Suffixes • _____ic for higher charge • _____ous for lower charge

  20. Type IIBinary Ionic Compounds (cont.) • Examples • Iron (III) chloride = ferric chloride • Iron (II) chloride = ferrous chloride

  21. Type IIBinary Ionic Compounds (cont.) • Common latin names • Cu – cupric, cuprous • Pb – plumbic, plumbous • Sn – stannic, stannous • Fe – ferric, ferrous

  22. Writing the Formulas from the Names (cont.) • For Type II Determine the charges on the cation and anion • Charge on cation = roman numeral • Balance the charges to get the subscripts

  23. Writing the Formulas from the Names (cont.) • Copper (I) oxide • Cu+1 O-2 • 2 Cu+1 will balance 1 O-2 • Cu2O

  24. Type III Binary Compounds(molecular compounds) • Name first element in formula first, use the full name of the element • Name the second element in the formula as if it were an anion (However, remember these compounds do not contain ions!)

  25. Type III Binary Compounds (cont.) • Use a prefix in front of each name to indicate the number of atoms • Never use the prefix mono- on the first element • CO2 = carbon dioxide • N2O5 = dinotrogen pentoxide

  26. Type III Prefixes

  27. Writing the Formulas from the Names • For Type III compounds, use the prefixes to determine the subscripts • Carbon tetrachloride • CCl4

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