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Chemistry Nomenclature

Chemistry Nomenclature. Binary Ionic Compounds. What are they made of?. Binary  Ionic  Example . 2 elements. metal ion + non-metal ion. sodium, Na +  metal chlorine, Cl -  non-metal. Naming from Formula. Write name of metal Write name of non-metal

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Chemistry Nomenclature

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  1. Chemistry Nomenclature Binary Ionic Compounds

  2. What are they made of? Binary  Ionic  Example  2 elements metal ion + non-metal ion sodium, Na+  metal chlorine, Cl-  non-metal

  3. Naming from Formula • Write name of metal • Write name of non-metal • Non-metal suffix = IDE NaCl sodium sodium chlorine sodium chloride

  4. Binary Compounds Binary compounds that contain a metal of fixed oxidation number (group 1, group 2, Al, Zn, Ag, etc.), and a non-metal. To name these compounds, give the name of metal followed by the name of the non-metal, with the ending replaced by the suffix –ide. Examples: LiF lithium fluoride (Li1+ F1-) CaS calcium sulfide (Ca2+ S2-) AlI3 aluminum iodide (Al3+ I1-)

  5. Cations and Anions Common Simple Cations and Anions Cation Name Anion Name* H 1+ hydrogen H 1-hydride Li 1+ lithium F 1-fluoride Na 1+ sodium Cl 1-chloride K 1+ potassium Br 1-bromide Cs 1+ cesium I 1-iodide Be 2+ beryllium O 2-oxide Mg 2+ magnesium S 2-sulfide Al 3+ aluminum Ag 1+ silver *The root is given in color. Zumdahl, Zumdahl, DeCoste, World of Chemistry2002, page 86

  6. Step 4: AlCl 3 Formula from Name: Criss-Cross Rule Example: Aluminum Chloride Step 1: Aluminum Chloride write out name with space 3+ Al Cl 1- Step 2: write symbols & charge of elements Al Cl Step 3: 1 3 criss-cross charges as subsrcipts combine as formula unit (“1” is never shown)

  7. Look at the Nelson textbook • Page 195 • Complete Questions 1 - 6

  8. Step 4: AlO 3 Criss-Cross Rule Example: Aluminum Oxide Step 1: Aluminum Oxide write out name with space 3+ Al O 2- Step 2: write symbols & charge of elements Al O Step 3: 2 3 criss-cross charges as subsrcipts 2 combine as formula unit

  9. Step 4: Mg2O2 Criss-Cross Rule Example: Magnesium Oxide Step 1: Magnesium Oxide 2+ Mg O 2- Step 2: Mg O Step 3: 2 2 Step 5:MgO (reduce subscripts to lowest ratio)

  10. Naming Binary Compounds Formula Name barium oxide • BaO ____________________ • ________________ sodium bromide • MgI2 ____________________ • KCl ____________________ • ________________ strontium fluoride • ________________ cesium fluoride NaBr magnesium iodide potassium chloride SrF2 CsF

  11. CHEMISTRY :LESSON 5 Multivalent Ionic Compounds Multivalent = Atoms with more than 1 charge

  12. Multivalent Binary CompoundsContaining a Metal (Variable Oxidation Number) and Non Metal • To name these compounds (stock system): • Write the name of the metal • Followed by Roman numerals in brackets to indicate • the charge of the metal ion • Write the name of the nonmetal, with its ending replaced by • the suffix –ide. Examples IUPAC System FeCl2 iron (II) chloride FeCl3 iron (III) chloride SnO tin (II) oxide SnO2 tin (IV) oxide

  13. ROMAN NUMERALS 1 6 2 7 3 8 4 9 5 10

  14. Common Multivalent Cations Ion IUPAC System Fe 3+ iron (III) Fe 2+ iron (II) Cu 2+ copper (II) Cu 1+ copper (I) Au 3+ gold (III) Au 1+ gold (I) Sn 4+ tin (IV) Sn 2+ tin (II) Pb 4+ lead (IV) Pb 2+ lead (II) Cr 3+ chromium (III) Cr 2+ chromium (II) Ni 3+ nickel (III) Ni 2+ nickel (II) Zumdahl, Zumdahl, DeCoste, World of Chemistry2002, page 90

  15. Naming Binary Compounds Formula Name tin (IV) fluoride • SnF4 ____________________ • HgO ____________________ • ________________ copper (II) fluoride • ________________ copper (I) sulfide • Cr2O3 ____________________ • ________________ lead (IV) oxide mercury (II) oxide CuF2 Cu2S chromium (III) oxide PbO2

  16. Assignment • McGraw Hill Ryerson Textbook • Page 146 • Questions 5-6 • Course Package Page A19 • Page 150 question 9

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