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Ch. 4 - Structure of Matter

Ch. 4 - Structure of Matter. IV. Naming Ionic Compounds & Writing Formulas for Ionic Compounds Oxidation Number Ionic Names Ionic Formulas. Bonding Review. Ionic Bond Transfer of eletcrons from a metal to a non-metal (unless we have a polyatomic ion Covalent Bond

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Ch. 4 - Structure of Matter

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  1. Ch. 4- Structure of Matter IV. Naming Ionic Compounds & Writing Formulas for Ionic Compounds Oxidation Number Ionic Names Ionic Formulas

  2. Bonding Review Ionic Bond Transfer of eletcrons from a metal to a non-metal (unless we have a polyatomic ion Covalent Bond Sharing of electrons between two or more non-metals

  3. A. Oxidation Number • The charge on an ion. • Indicates the # of e- gained/lost to become stable. 1+ 0 2+ 3+ 4+ 3- 2- 1-

  4. B. Ionic Names • Write the names of both elements, cation first. • Change the anion’s ending to -ide. • Write the names of polyatomic ions. • For ions with variable oxidation #’s, write the ox. # in parentheses using Roman numerals. Overall charge = 0.

  5. Polyatomic Ion List • +1 • ammonium, NH4+ • -1 • acetate, C2H3O2-, or CH3COO - • bromate, BrO3- • chlorate, ClO3- • chlorite, ClO2- • cyanide, CN- • hydrogen carbonate, HCO3- (also called bicarbonate) • hydroxide, OH- • hypochlorite, ClO- • iodate, IO3- • nitrate, NO3- • nitrite, NO2- • permanganate, MnO4- • perchlorate, ClO4- • thiocyanate, SCN– • -2 • carbonate, CO3 -2 • chromate, CrO4 -2 • dichromate, Cr2O7 -2 • oxalate, C2O4 -2 • peroxide, O2 -2 • sulfate, SO4 -2 • sulfite, SO3 -2 • -3 • phosphate, PO4 -3 • phosphite, PO3-3 • arsenate, AsO4-3 • -iteis one less oxygen than the ite ion • Hypo- is one less oxygen than the ite ion • Per- is one more oxygen than the ate • Hydrogen can be added to -2 or -3 ions to make a “new ion” i.e. H2PO4–1 is dihydrogen phosphate (note the – charge went up 1 for each H+ added)

  6. B. Ionic Names • NaBr • Na2CO3 • FeCl3 • (NH4)3PO4

  7. C. Ionic Formulas • Write each ion. Put the cation first. • Overall charge must equal zero. • If charges cancel, just write the symbols. • If not, crisscross the charges to find subscripts. Called charge crossing • Use parentheses when more than one polyatomic ion is needed. • Roman numerals indicate the oxidation #.

  8. C. Ionic Formulas • potassium chloride • magnesium nitrate • copper(II) chloride • Ammonium hydroxide • Lead (IV) phosphate

  9. C. Ionic Formulas • calcium oxide • aluminum chlorate • iron(III) oxide • Ca2+ O2- CaO • Al3+ ClO3-  Al(ClO3)3 • Fe3+ O2- Fe2O3

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