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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!
MULTIVALENT IONIC COMPOUNDS
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RULES1. Use ROMAN NUMERALS to
determine the ION CHARGE of the MULTIVALENT ION.
2. If ROMAN NUMERAL are NOT given, use the charge found on the top in each box on the table.
EXAMPLE: copper (II) oxide
_________________________
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lead (IV) sulfide_________________________
tin sulfide_________________________
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RULES1. Write the names of the ions.
2. Write the ROMAN NUMERAL for the MULTIVALENT ION. There are 2 METHODS:
1. METHOD 1 Charges must add up to zero.
2. METHOD 2 Charge of Anion X Subscript of Anion
Subscript of Cation
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PbI2 _________________________
Fe2O3 _________________________
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CuCl _________________________
MnO2 _________________________
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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 ________
POLYATOMIC IONIC COMPOUNDS
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lithium sulfate _____________________
ammonium carbonate_____________________
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hydrogen dichromate_____________________
sodium acetate _____________________
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HNO3 _____________________
NaOH _____________________
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KMnO4
_____________________
Cu2SO4
_____________________
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hydrogen carbonate is AKA bicarbonate HCO3
-
hydrogen sulfate is AKA bisulfate HSO4-
tetraborate B4O72-
silicate SiO32-
glutamate C5NH8O4-
SOME OTHER NAMES . . .
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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.
HYDRATED IONIC COMPOUNDS
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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
HYDRATED IONIC COMPOUNDS
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barium chloride dihydrate _____________________
potassium hydroxide hexahydrate _____________________
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sodium carbonate octahydrate _____________________
cobalt (II) chloride decahydrate _____________________
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CaSO4 ∙2H2O _____________________
Na3PO4 ∙4H2O ______________________
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HCN ∙ 3H2O _____________________
HOMEWORK:◦ DO THE SHEET ON HYDRATED IONIC COMPOUNDS
ON THE NEXT PAGE OF YOUR HANDOUT.
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