Aim 4.7 Balancing Ionic Compounds with Polyatomic Ions

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  Aim 4.7 Balancing Ionic Compounds with Polyatomic Ions. Polyatomic Ion : an ion made of 2 or more non-metal atoms. Do Now: *HW out *Have Reference Tables ready *Do the Do Now on classwork *Copy Definition below onto CW. Do Now:.
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Aim 4.7 Balancing Ionic Compounds with Polyatomic Ions Polyatomic Ion: an ion made of 2 or more non-metal atoms. Do Now: *HW out *Have Reference Tables ready *Do the Do Now on classwork *Copy Definition below onto CW Do Now: Classwork: Practice with Table E, “Selected Polyatomic Ions” Part A: Name each polyatomic ion MnO4- _____________________________________________ 2. C2O42- _____________________________________________ ClO- _____________________________________________ 4. ClO3- _____________________________________________ NH4+_____________________________________________ 6. H3O+ _____________________________________________ Hg22+ _____________________________________________ 8. CO32- _____________________________________________ 9. NO2- _____________________________________________ 10. NO3- _____________________________________________ Part B: Write the chemical formula of each polyatomic ion from Table E Ex: hydroxide: OH- 1. thiosulfate: 2. hydrogen carbonate: 3. carbonate: 4. dichromate: 5. hydronium: 6. oxalate: Part C: Write the name of each ionic compound. from Table E(Each one contains at least one polyatomic ion, which is in bold)If it contains a transition metal that needs a roman numeral, it is bold and italicsEx: Li PO43-___lithium phosphate___________1. Li (OH)- _____________________________________________ 2. Mg1+2(CN)2-1___________________________________________3. K (SO4)2- _____________________________________________ 4. Fe32+ (PO4)23- _________________________________________ 5. Ca (O2)2-_____________________________________________ 6. Mg from Table EOH-_________________________________ 7. Be+2 (SO4)2- _________________________________ 8. Fe1+2 (NO2)2-_________________________________ 9. Hg22+ SO42- _________________________________ 10. (NH4)+ CN-_________________________________ Part D: Balance the ionic compounds using the from Table Ecriss-cross method. The charge of the ion is given for you. 1. Mg CN- 2. Li (SO4)2- 3. K (PO4)3- 4. Ca(NO2)2- (this has 2 ions, each with a -1 charge) 5. Na (CO3 )2- 6. Ba ( from Table EC2O4 )2- 7. Fe ClO- 8. Co (OH)- 9. Mn(PO4)3- 10. V (OH)- Part E: Reviewing Ionic Compounds with Transition Metals from Table EWrite a balanced ionic formula for each compound: 1. Iron (II) oxide: 2. Iron (III) oxide: 3. Vanadium (III) fluoride: 4. Titanium (II) sulfide: 5. Manganese (IV) oxide: 6. Vanadium (V) chloride:
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