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Nomenclature

This guide covers the fundamental principles of naming binary and ternary compounds, including ionic and covalent compounds. It details the rules for naming binary compounds, where the positive element is named first followed by the negative element with an -ide suffix. It explains the use of geometric prefixes in molecular nomenclature, the identification of polyatomic ions, and the naming conventions for acids. Understanding these rules is essential for chemistry students to successfully derive formulas and determine the percent composition of compounds.

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Nomenclature

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  1. Nomenclature Naming Compounds

  2. Binary Compounds

  3. Compounds with only two elements in any ratio

  4. KCl NO2 CaCl2 P2O5 Al2O3 H2S Na2O etc

  5. Binary compounds can be either ionic or covalent

  6. Naming Binary Compounds

  7. Naming Ionic Compounds

  8. Name positive element first with its normal name • Name negative element last & change its ending to -ide

  9. KClCaCl2Al2O3Na2O

  10. Name Each: CaCl2 CaS K2O LiF

  11. Name Each: FeCl2 FeCl3

  12. If the Positive element is not from columns I or II • its ox # must be determined and written in roman numerals

  13. Determining the Charge • Add up the oxidation numbers of all the negative elements • The positive portion must balance out the negative portion • Divide the positive portion by the metal subscript

  14. Name Each: CuCl Fe2O3MnO2 CrO3

  15. Molecule

  16. A covalent compound that can exist as a separate unit • Non-metals bond to form molecules

  17. Naming Molecules or Covalent Compounds

  18. Same rules as ionic compounds except: • use geometric prefixes to determine the # of each atom

  19. Geometric Prefixes 1-mono 5-penta 2-di 6-hexa 3-tri 7-hepta 4-tetra etc

  20. Name Each: CO S2O3N2H4 SO3

  21. Nomenclature HW • Work problems: • 49 - 54 • on page 51

  22. Drill: Name Each: CaO P2O5Al2S3 SO2

  23. Deriving Formulas • Write the symbol for each element • Determine ox #s for each • Determine lowest common multiple to balance the charge • Apply subscripts

  24. Write formulas for: • Sodium sulfide • Lead (II) iodide • Diphosphorus pentoxide

  25. Write formulas for: • Chromium(III) oxide • Aluminum carbide

  26. Polyatomic Ion

  27. A group of atoms chemically combined that together have a charge

  28. Most are oxoanions • PO4-3 SO4-2 • A root element bound to oxygen

  29. Naming Polyatomic Ions

  30. Learn the polyatomic table on page 42 & 43 • Learn how to use the periodic table to determine polyatomic ions

  31. Name the root element • Change the ending to -ate • PO4-3 = phosphate • Some are unusual

  32. CN-1 OH-1 C2H3O2-1C2O4-2

  33. H2O H3O+1NH3 NH4+1

  34. Polyatomic Ion Endings • Maximum O = -ate • 1 less than max O = -ite • SO4-2 = sulfate • SO3-2 = sulfite

  35. Naming Ternary Compounds

  36. Ternary Compounds • Compounds containing more than two different elements • Most contain polyatomic ions

  37. Follow ionic rules for naming the compound • Name the polyatomic ion as the positive or negative portion

  38. Name Each: CaCO3K2SO4

  39. Name Each: Pb(NO3)2MgSO3

  40. Write Formulas For: • Lead (II) nitrate • Aluminum sulfate • Potassium chlorate • Ammonium phosphite

  41. Name the Following: BaSO4 CuNO3 SO2 (NH4)3PO4

  42. Naming Acids

  43. Binary acids become: • Hydro _____ ic acids • HCl - Hydrochloric acid

  44. Ternary acids become: • _____ ic acids or • _____ ous acids • H2SO4 - Sulfuric acid • H2SO3 - Sulfurous acid

  45. ____ ic acids form from polyatomic ions ending with ___ ate • ____ ous acids form from polyatomic ions ending with ___ ite

  46. ___ ide ions become: • hydro ___ ic acids • ___ ate ions become: • ___ ic acids • ___ ite ions become: • ___ ous acids

  47. Percent Compositionby Mass

  48. Determine the atomic mass of each element in the compound • Determine the molecular mass of the compound by adding • Divide each elemental mass by molecular mass • Multiply by 100 %

  49. MgCl2 • Mg = 24.3 g/mole • 2 Cl = 2 x 35.5 = 71.0 g/mole • MgCl2 = total = 95.3 g/mole • % Mg =24.3/95.3 x 100% • % Cl = 71.0/95.3 x 100 %

  50. Determine % Comp for Each: Fe2O3 C3H6O3 CuSO4*5H2O

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