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Nomenclature Notes

Nomenclature Notes. Introduction. Nomenclature: System for naming compounds Avoids “ common name ” confusion System – Name tells something about the composition of the compound. Introduction. Binary Compounds : Compounds composed of 2 elements. Categories of Binary Compounds.

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Nomenclature Notes

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  1. Nomenclature Notes

  2. Introduction • Nomenclature: System for naming compounds • Avoids “common name” confusion • System – Name tells something about the composition of the compound

  3. Introduction • Binary Compounds: Compounds composed of 2 elements

  4. Categories of Binary Compounds • Compounds that contain a metal and a nonmetal. • Called binary ionic compounds • Involves a positive cation (metal) and a negative anion (nonmetal) • NAME them by simply naming the ions! • There are 2 types of the metal / nonmetal compounds

  5. Type I Binary Compounds • Contain metal atoms that only form cation that has 1 possible charge

  6. Type I Binary Compounds • Contain metal atoms that only form cation that has 1 possible charge

  7. Type I Binary Compounds • Contain metal atoms that only form cation that has 1 possible charge

  8. Type I Binary Compounds • Contain metal atoms that only form cation that has 1 possible charge

  9. Type I Binary Compounds • Naming Rules • Name cation (metal) first and then the anion (non-metal) second. • Simply use the atom’s name for the name of the cation. • For the anion, take the root from the atom’s name and change the ending to –ide. NOTE: Sometimes the root gets more modification.

  10. Type I Binary Compounds

  11. Type I Binary Compounds

  12. Type I Binary Compounds

  13. Type I Binary Compounds

  14. Type I Binary Compounds

  15. Type I Binary Compounds • Remember symbols for ions show the charge but ionic compound formulas don’t.

  16. Type I Binary Compounds • For each of the following identify the ions and name the compounds.

  17. Type I Binary Compounds • For each of the following identify the ions and name the compounds.

  18. Type I Binary Compounds • For each of the following identify the ions and name the compounds.

  19. Type I Binary Compounds • For each of the following identify the ions and name the compounds.

  20. Type I Binary Compounds • For each of the following identify the ions and name the compounds.

  21. Type II Binary Ionic Compounds • Contain metal atoms that can form 2 or more cations.

  22. Type II Binary Ionic Compounds • Contain metal atoms that can form 2 or more cations.

  23. Type II Binary Ionic Compounds • Contain metal atoms that can form 2 or more cations.

  24. Type II Binary Ionic Compounds • Contain metal atoms that can form 2 or more cations.

  25. Type II Binary Ionic Compounds • Contain metal atoms that can form 2 or more cations.

  26. Type II Binary Ionic Compounds • Contain metal atoms that can form 2 or more cations.

  27. Type II Binary Ionic Compounds • Contain metal atoms that can form 2 or more cations.

  28. Type II Binary Ionic Compounds • Naming Rules • Name cation (metal) first and then the anion (non-metal) second. • Use Roman numeral after the cation’s name to indicate the charge. • Ni+2 Nickel (II) Ion • Ni+3 Nickel (III) Ion

  29. Type II Binary Ionic Compounds • Naming Rules • Name the anion as in Type I ions. • Take the root of the atom and change the ending to –ide. As before sometimes the root gets more modification. • P-3  Phosphide Ion • Br -1 Bromide Ion

  30. Type II Binary Ionic Compounds • How do know to use the Roman Numerals? • Look on you Periodic Table (from the bookstore). • If the METAL atom shows more than one possible cation charge you must use a Roman Numeral in the NAME.

  31. Type II Binary Ionic Compounds • How do we know which charge it is? • Know that the cation (positive) charge must balance the total anion (negative) charge. • Examples: • FeCl2 • PbO2

  32. Type II Binary Ionic Compounds • Another system (not used much anymore) for naming Type II Binary Ionic Compounds exists. • Ion form with the higher charge has the name ending in –ic. • Ion form with the lower charge has the name ending in –ous. • We will use the Roman Numeral System but you may at times see the other system.

  33. Binary Compounds – Categories • Compounds that contain a metal and a non-metal • Type I – Cation formed has only 1 possible charge. • Type II – Cation formed has 2 or more possible charges. • Compounds that contain only non-metals – • Type III Binary Compounds

  34. Type III Binary Compounds • Contain ONLY NON-METALS • Rules for naming! • 1st element in the formula is named first and full element name is used. • 2nd element is named as if it were an anion (-ide ending) • Prefixes are used to describe the number of atoms present.

  35. 1 = mono- 2 = di- 3 = tri- 4 = tetra- 5 = penta- 6 = hexa- 7 = hepta- 8 = octa- 9 = nona- 10= deca- Type III Binary Compounds Prefixes

  36. Type III Binary Compounds • Rules for naming! (Continued) • Never use the prefix mono- in naming the first element. • Drop the ending o or a ending on a prefix before an element that starts with the vowel – O or A • Examples: • N3S5 • P7O9 • S2O • CO6

  37. Type III Binary Compounds • Rules for naming! (Continued) • Never use the prefix mono- in naming the first element. • Drop the ending o or a ending on a prefix before an element that starts with the vowel – O or A • Examples: • N3S5 Trinitrogenpentasulfide • P7O9 • S2O • CO6

  38. Type III Binary Compounds • Rules for naming! (Continued) • Never use the prefix mono- in naming the first element. • Drop the ending o or a ending on a prefix before an element that starts with the vowel – O or A • Examples: • N3S5 Trinitrogenpentasulfide • P7O9 Heptaphosphorusnonoxide • S2O • CO6

  39. Type III Binary Compounds • Rules for naming! (Continued) • Never use the prefix mono- in naming the first element. • Drop the ending o or a ending on a prefix before an element that starts with the vowel – O or A • Examples: • N3S5 Trinitrogenpentasulfide • P7O9 Heptaphosphorusnonoxide • S2O Disulfur monoxide • CO6

  40. Type III Binary Compounds • Rules for naming! (Continued) • Never use the prefix mono- in naming the first element. • Drop the ending o or a ending on a prefix before an element that starts with the vowel – O or A • Examples: • N3S5 Trinitrogenpentasulfide • P7O9 Heptaphosphorusnonoxide • S2O Disulfur monoxide • CO6 Carbon hexoxide

  41. Writing Formulas • For Type I and Type II Compounds • Determine the charge on the ions present. • For type II compounds the roman numeral gives you the charge of the cation. • For Type I compounds the position on the periodic table helps you determine the charge. • Use subscripts for each atom so that the total charge on the compound is zero.

  42. Writing Formulas • For Type III – (identified because they are both non-metals) • Use the prefixes to determine the subscripts. • Remember that the subscript for the first element is 1 if there isn’t any prefix

  43. Writing Formulas • Practice Problems- Identify the type and then write the formula. • Sodium phosphide • Tricarbontetroxide. • Lithium selenide

  44. Writing Formulas • Practice Problems- Identify the type and then write the formula. • Iron (III) sulfide • Aluminum iodide • Boron octafluoride

  45. Writing Formulas • Practice Problems- Identify the type and then write the formula. • Manganese (VII) phosphide • Diphosphorous monoxide • Chromium (III) nitride

  46. Type IV - Compounds • Identified because • They contain more than two elements. • A POLYATOMIC ion (ion made of 2 or more different atoms) is present

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