Topic: Names, Formulas, Equations, & Reactions Aim: How do we name & write formulas for ionic compounds? Do now: Name these: P4O10, NH3, NO2, AlBr3 HW:

Naming Ionic Compounds with Polyatomic Ions See Table E!! Three options Metal name + name of polyatomic ion OR Polyatomic ion + nonmetal (w/ “-ide”) OR Polyatomic ion + polyatomic ion Same deal as binary ionic – NO PREFIXES. Never change name or ending of a poly. ion.

Naming Ionic Compounds with Polyatomic Ions KNO3 NH4Cl KOH MgCO3 Al2(SO4)3 Na3PO4 Potassium nitrate Ammonium chloride Potassium hydroxide Magnesium carbonate Aluminum sulfate Sodium phosphate

Naming Ionic Compounds with Polyatomic Ions NH4NO3 Ca(NO3)2 LiNO3 K2Cr2O7 Mg(C2H3O2)2 (NH4)2SO3 Ammonium nitrate Calcium nitrate Lithium nitrate Potassium dichromate Magnesium acetate Ammonium sulfite

Formulas – Ionic Compounds with Polyatomic Ions No prefixes, so…CRISS-CROSS METHOD AGAIN Take oxidation state of the element & of the ENTIRE polyatomic ion & criss-cross them to get your formula **If you end up with more than one polyatomic ion, enclose it in parentheses!! & put the subscript outside Do not include charge in the final formula Al +3 SO4 -2 Al (SO4) 2 3

Formulas of Ionic Compounds with Polyatomic Ions Sodium hydroxide Potassium nitrate Potassium phosphate Magnesium sulfate Magnesium hydroxide NaOH KNO3 K3PO4 MgSO4 Mg(OH)2

Formulas of Ionic Compounds with Polyatomic Ions Aluminum phosphate Aluminum nitrate Ammonium nitrate Ammonium sulfite Sodium carbonate AlPO4 Al(NO3)3 NH4NO3 (NH4)2SO3 Na2CO3

Topic: Names, Formulas, Balancing Aim: How do you name and write formulas for ionic compounds using the stock system? Do Now: Name the following: P2O5, Mg(NO3)2 Write formulas for: lithium oxide, disulfur tetroxide HW:

Ionic Compounds – Stock System Some metals have >1 oxidation state Which ones? Transition metals

Ionic Compounds – Stock System A ROMAN NUMERAL tells the ox. state to use for the metal. Example: Iron (Fe) can be +2 or +3 So: Iron (II) chloride tells the reader that Fe has a +2 charge Formula is Fe+2Cl- (criss-cross)  FeCl2 So: Iron (III) chloride tells the reader that Fe has a +3 charge Formula is Fe+3Cl- (criss-cross)  FeCl3

Formulas – Ionic Compounds – Stock System Iron II oxide Tin II sulfide Lead II nitrate Iron III oxide Tin IV oxide FeO SnS Pb(NO3)2 Fe2O3 SnO2

Formulas – Ionic Compounds – Stock System Copper I chloride Mercury II iodide Copper II nitrite Lead IV oxide Gold I oxide CuCl HgI2 Cu(NO2)2 PbO2 Au2O

Naming Ionic Compounds – Stock System When writing the name from the formula, use the NONMETAL (with known oxidation #) to figure out the METAL (b/c there is more than 1 option for the oxidation #) You have to do a little bit of math.

Naming Ionic Compounds – Stock System Ex: FeO Fe can be +2 (Iron II) or +3 (Iron III) Oxygen is -2 1 oxygen x -2 charge = -2 total charge 1 iron x _?_ charge = +2 total charge (to cancel out the -2) ? = +2 So it is Iron II Oxide

Naming Ionic Compounds – Stock System Ex: Fe2O3 Fe can be +2 (Iron II) or +3 (Iron III) Oxygen is -2 3 oxygens x -2 charge = -6 total charge 2 iron x _?_ charge = +6 total charge (to cancel out the -6) ? = +3 So it is Iron III Oxide

Naming Ionic Compounds – Stock System CuCl FeS HgI2 Pb(NO3)2 Sn(OH)2 Copper I chloride Iron II sulfide Mercury II iodide Lead II nitrate Tin II hydroxide

Naming Ionic Compounds – Stock System Cu(NO3)2 Fe2O3 PbI4 SnO2 FeCO3 Copper II nitrate Iron III oxide Lead IV iodide Tin IV oxide Iron II carbonate