1 / 27

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

flavian-myles
Download Presentation

Naming Starts with Classifying Compounds (3 types)

An Image/Link below is provided (as is) to download presentation Download Policy: Content on the Website is provided to you AS IS for your information and personal use and may not be sold / licensed / shared on other websites without getting consent from its author. Content is provided to you AS IS for your information and personal use only. Download presentation by click this link. While downloading, if for some reason you are not able to download a presentation, the publisher may have deleted the file from their server. During download, if you can't get a presentation, the file might be deleted by the publisher.

E N D

Presentation Transcript

  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

More Related