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MULTIVALENT IONIC COMPOUNDS

MULTIVALENT IONIC COMPOUNDS. Ions of some transition elements can have more than one possible charge. Such elements are called MULTIVALENT species. For example, what are the 2 possible charges for copper – Cu? _________________ _________________

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MULTIVALENT IONIC COMPOUNDS

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  1. MULTIVALENT IONIC COMPOUNDS • Ions of some transition elements can have more than one possible charge. • Such elements are called MULTIVALENT species. • For example, what are the 2 possible charges for copper – Cu? • _________________ • _________________ • WE use ROMAN NUMERALS to indicate the type of charge on these multivalent ions. • 1+  I • 2+  II • 3+  III • 4+  IV • 5+  V • 6+  VI • ONLY USE WITH MULTIVALENT IONS!

  2. GIVEN NAME, WRITE FORMULA RULES • Use ROMAN NUMERALS to determine the ION CHARGE of the MULTIVALENT ION. • If ROMAN NUMERAL are NOT given, use the charge found on the top in each box on the table. • EXAMPLE: • copper (II) oxide _________________________

  3. GIVEN NAME, WRITE FORMULA • lead (IV) sulfide _________________________ • tin sulfide _________________________

  4. GIVEN FORMULA, WRITE NAME • RULES • Write the names of the ions. • Write the ROMAN NUMERAL for the MULTIVALENT ION. There are 2 METHODS: • METHOD 1 Charges must add up to zero. • METHOD 2 Charge of Anion X Subscript of Anion Subscript of Cation

  5. GIVEN FORMULA, WRITE NAME • PbI2 _________________________ • Fe2O3 _________________________

  6. GIVEN FORMULA, WRITE NAME • CuCl _________________________ • MnO2 _________________________

  7. POLYATOMIC IONIC COMPOUNDS • DEFINITION: • Polyatomic ions are GROUPS OF ATOMS acting as 1 ION, carrying an OVERALL CHARGE. • On the back of your periodic table, there is a POLYATOMIC ION TABLE. • Endings of polyatomic ions are easily recognizable as they are often –ATE or –ITE, providing a good clue. • EXAMPLES: • nitrate ________ • nitrite ________ • cyanide ________ • hydroxide ________ • bicarbonate ________ • chlorate ________ • carbonate ________ • sulfate ________ • phosphate ________ • ammonium ________ • acetate ________

  8. GIVEN NAME, WRITE FORMULA • lithium sulfate _____________________ • ammonium carbonate _____________________

  9. GIVEN NAME, WRITE FORMULA • hydrogen dichromate _____________________ • sodium acetate _____________________

  10. GIVEN FORMULA, WRITE NAME • HNO3 _____________________ • NaOH _____________________

  11. GIVEN FORMULA, WRITE NAME • KMnO4 _____________________ • Cu2SO4 _____________________

  12. SOME OTHER NAMES . . . • hydrogen carbonate is AKA bicarbonate HCO3- • hydrogen sulfate is AKA bisulfate HSO4- • tetraborate B4O72- • silicate SiO32- • glutamate C5NH8O4-

  13. HYDRATED IONIC COMPOUNDS • Hydrated ionic compounds have WATER attached to their crystal lattice structure. • Solutions become hydrated when they are crystallized from a water solution. • They are often recognizable by eye because they are often SHINY and TRANSLUCENT. • Examples: • Bluestone, Epsom salts, Rock salts • BLUESTONE  CuSO4 ∙5H2O • 5 H2O molecules attached to each CuSO4 compound. • The “dot” represents a weak bond.

  14. HYDRATED IONIC COMPOUNDS • We indicate the presence of water with the word HYDRATE and we indicate the number of water molecules with our GREEK PREFIXES: • MONO 1, DI 2, TRI 3, TETRA 4, PENTA 5, HEXA 6, HEPTA 7, OCTA 8, NONA 9, DECA 10 • ANHYDROUS: NO water attached

  15. GIVEN NAME, WRITE FORMULA • barium chloride dihydrate • _____________________ • potassium hydroxide hexahydrate • _____________________

  16. GIVEN NAME, WRITE FORMULA • sodium carbonate octahydrate • _____________________ • cobalt (II) chloride decahydrate • _____________________

  17. GIVEN FORMULA, WRITE NAME • CaSO4 ∙2H2O _____________________ • Na3PO4 ∙4H2O ______________________

  18. GIVEN FORMULA, WRITE NAME • HCN ∙ 3H2O _____________________ • HOMEWORK: • DO THE SHEET ON HYDRATED IONIC COMPOUNDS ON THE NEXT PAGE OF YOUR HANDOUT.

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