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Net Ionic in SR

Net Ionic in SR. Review Check NI I Notes on Net Ionic in SR Guided Practice Homework. Write, predict, balance, give NI. Barium hydroxide reacts with ammonium chloride. Tell me where you are confused. NH 4 + (aq) + OH - (aq) g NH 3(g) + H 2 O (l). Checking your homework.

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Net Ionic in SR

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  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)

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