1. Net Ionic in SR Review Check NI I Notes on Net Ionic in SR
Guided Practice
Homework

2. Write, predict, balance, give NI
Barium hydroxide reacts with ammonium chloride.
Tell me where you are confused.
NH4+(aq) + OH-(aq) g NH3(g) + H2O(l)

3. Checking your homework
Be ready to make corrections!

4. Aqueous lead (II) acetate reacts with sulfuric acid
M: Pb(C2H3O2)2(aq) + H2SO4(aq)  PbSO4(s) + 2HC2H3O2(aq)
CI: Pb+2(aq) + 2C2H3O2­-(aq) + 2H+(aq) + SO4-2(aq)  PbSO4(s) + 2H+(aq) + 2C2H3O2-(aq)
NI: Pb+2(aq) + SO4-2(aq)  PbSO4(s)

5. Aqueous barium hydroxide reacts with aqueous lithium sulfate
M: Ba(OH)2(aq) +Li2SO4(aq)  BaSO4(s) + 2 LiOH(aq)
CI: Ba+2(aq) + 2OH-(aq) + 2Li+(aq) + SO4-2(aq)  BaSO4(s) + 2Li+(aq) + 2OH-(aq)
NI: Ba+2(aq) + SO4-2(aq)  BaSO4(s)

6. Aqueous magnesium nitrate reacts with aqueous potassium phosphate
M: 3 Mg(NO3)2(aq) + 2 K3PO4(aq)  Mg3(PO4)2(s) + 6 KNO3(aq)
CI: 3Mg+2(aq) + 6NO3‑(aq) + 6K+(aq) + 2PO4-3(aq)  Mg3(PO4)2(s) + 6K+(aq) + 6NO3-(aq)
NI: 3 Mg+2(aq) + 2 PO4-3(aq)  Mg3(PO4)2(s)

7. Aqueous lead (II) chlorate reacts with aqueous rubidium carbonate
M: Pb(ClO3)2(aq) + Rb2CO3(aq)  PbCO3(s) + 2 RbClO3(aq)
CI: Pb+2(aq) + 2ClO3‑(aq) + 2Rb+(aq) + CO3-2(aq)  PbCO3(s) + 2Rb+(aq) + 2ClO3-(aq)
NI: Pb+2(aq) + CO3-2(aq)  PbCO3(s)

8. Aqueous strontium nitrate reacts with aqueous nickel (II) sulfate
M: Sr(NO3)2(aq) + NiSO4(aq)  SrSO4(s) + Ni(NO3)2(aq)
CI: Sr+2(aq) + 2NO3-(aq) + Ni+2(aq) + SO4-2(aq)  SrSO4(s) + Ni+2(aq) + 2NO3-(aq)
NI: Sr+2(aq) + SO4-2(aq)  SrSO4(s)

9. Aqueous iron (II) chloride reacts with aqueous lithium phosphate
M: 3 FeCl2(aq) + 2 Li3PO4(aq)  Fe3(PO4)2(s) + 6 LiCl(aq)
CI: 3Fe+2(aq) + 6Cl-(aq) + 6Li+(aq) + 2PO4-3(aq) Fe3(PO4)2(s) + 6Li+(aq) + 6Cl-(aq)
NI: 3 Fe+2(aq) + 2 PO4-3(aq) Fe3(PO4)2(s)

10. Aqueous copper (II) iodide reacts with aqueous potassium hydroxide
M: CuI2(aq) + 2 KOH(aq)  Cu(OH)2(s) + 2 KI(aq)
CI: Cu+2(aq) + 2I-(aq) + 2K+(aq) + 2OH-(aq)  Cu(OH)2(s) + 2K+(aq) + 2I-(aq)
NI: Cu+2(aq) + 2 OH-(aq)  Cu(OH)2(s)

11. Aqueous magnesium sulfide reacts with aqueous carbonic acid
M: MgS(aq) + H2CO3(aq)  MgCO3(s) + H2S(g)
CI: Mg+2(aq) + S-2(aq) + 2H+(aq) + CO3-2(aq)  MgCO3(s) + H2S(g)
NI: Mg+2(aq) + S-2(aq) + 2H+(aq) + CO3-2(aq)  MgCO3(s) + H2S(g)

12. Aqueous barium sulfide reacts with aqueous chromium (I) perchlorate
M: BaS(aq) + 2 CrClO4(aq)  Ba(ClO4)2(aq) + Cr2S(s)
CI: Ba+2(aq) + S-2(aq) + 2 Cr+1(aq) + 2ClO4-(aq)  Cr2S(s) + Ba+2(aq) + 2ClO4-(aq)
NI: S-2(aq) + 2 Cr+1(aq)  Cr2S(s)

13. Aqueous zinc chloride reacts with aqueous magnesium sulfide
M: ZnCl2(aq) + MgS(aq)  ZnS(s) + MgCl2(aq)
CI: Zn+2(aq) + 2Cl-(aq) + Mg+2(aq) + S-2(aq)  ZnS(s) + Mg+2(aq) + 2Cl-(aq)
NI: Zn+2(aq) + S-2(aq)  ZnS(s)

14. Net Ionic Equations Single Replacement
Date:

15. General Guidelines
Net ionic equations for SR rxn follow the same procedures as NI DR, but only ONE ion gets canceled.

16. Example 2 NaI + Br2  2 NaBr + I2
Fill in state of matter using solubility chart and PT.
This is the MOLECULAR EQUATION
Rewrite aqueous compounds as ions

17. 2Na+(aq) + 2I-(aq) + Br2(l)  2Na+(aq) + 2Br-(aq) + I2(s)
This is the COMPLETE IONIC EQUATION
Cancel the matching ion from both sides.

18. 2I-(aq) + Br2(l)  2Br-(aq) + I2(s)
This is the net ionic equation.

19. Aqueous lithium chloride reacts with fluorine gas.
2Cl-(aq) + F2(g) g Cl2(g) + 2F-(aq)

20. Aqueous magnesium bromide reacts with lithium.
Mg+2(aq) + 2Li(s) g Mg(s) + 2Li+(aq)

21. Hints There MUST be one ion on each side of the equation.
The charges on both sides of the equation must be equal.
Diatomics are ONLY diatomic when they were alone in the original equation – if they come out of a compound they are ions, not diatomic.

22. Oxidation Reduction When something is oxidized, its charge goes up.
When something is reduced, its charge goes down.
NI equations make it easy to determine what was oxidized and what was reduced.

23. Determine Oxidized and Reduced
2I-(aq) + Br2(l)  2Br-(aq) + I2(s)
2Cl-(aq) + F2(g) g Cl2(g) + 2F-(aq)
Mg+2(aq) + 2Li(s) g Mg(s) + 2Li+(aq)