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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. REMEMBER !. Metals tend to Lose electrons and become positive ions ( cations ) .

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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. REMEMBER ! • Metals tend to Lose electrons and become positive ions (cations). • Non-metals tend to gain electrons and become negative ions (anions).

  4. Example 1: Sodium and Fluorine.Draw Bohr-Rutherford diagrams of both atoms.

  5. + - Na F Electro-magnetic Force is created by the TRANSFERof electrons forming a BOND !

  6. Crystal Lattice Structure • Each electron which Sodium atom lost, is grabbed by Fluorine atom. • There same number of Na+ and F- ions, their ratio is 1:1, but • ions do not form molecules. Instead, they are tightly packed in crystals with alternative + and – ions.

  7. Example 2 : Aluminum and Chlorine. Draw Lewis diagrams of both atoms Al Cl Cl Cl

  8. Chemical Formula • Ex 1: One Sodium for One Fluorine • NaF • Ex2 : One Aluminum for Three Chlorine • NaCl3 • Subscript 3 in the formula indicates that it takes 3 Cl atoms to 1 Al atom. • With the right subscript, the overall charge of the compound is zero.

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

  10. 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

  11. Writing Chemical Formulas for Ionic Compounds. • Points to note: • The metal ion/cation is always first • The nonmetal ion/anion is always written second • Steps: • Write the chemical symbols for each element (metal first) • Write the ionic charge above each element • Criss-cross the NUMBERS (not the signs) and write them as subscripts

  12. 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)

  13. 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

  14. 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)

  15. Ex. 1 Magnesium and Chlorine Total Charge Check: Ex.2 Calcium and Oxygen Total Charge Check:

  16. HINTS: • Criss-cross rule will help you to figure out the right subscript in the compound formula • Ignore subscript if it is 1 • Subscripts do not have signs: it’s a number of ions! • Final formula shall not indicate charge on top • Reduce subscripts, go by lower terms

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

  18. 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 parentheses to indicate • the oxidation number of the metal • 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

  19. 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

  20. 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

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