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Net Ionic Equations

Net Ionic Equations. Net Ionic Equations. Equations attempt to show only the exact particles involved in the reaction. Net Ionic Equations. You must first decide - are substances written as molecules or ions?. (NH 4 ) 2 S + Fe(NO 3 ) 2 2NH 4 NO 3 + FeS

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Net Ionic Equations

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  1. Net Ionic Equations

  2. Net Ionic Equations Equations attempt to show only the exact particles involved in the reaction.

  3. Net Ionic Equations You must first decide - are substances written as molecules or ions?

  4. (NH4)2S + Fe(NO3)2 2NH4NO3 + FeS This is a molecular equation.

  5. (NH4)2S + Fe(NO3)2 2NH4NO3 + FeS S-2 + Fe+2 FeS This is the same equation written in net ionic form.

  6. Write this in net ionic form: H2SO4(aq) H2O(l) + SO3(aq) Which are molecules? Which are ions?

  7. Seven rules to help you decide ions or molecules.

  8. Rule #1 - Binary acids Strong Acids are written in ionic form. Examples: HCl, HBr, HI Weak Acids are written in molecular form. Examples: All Others

  9. Rule #2 - Ternary acids Strong Ternary Acids: the number of oxygen atoms exceeds the number of hydrogen atoms by two or more, are written in ionic form. Examples: H2SO4, HNO3

  10. Rule #2 - Ternary acids Weak ternary acids are written in molecular form. Examples: H3PO4

  11. Rule #3 - Polyprotic acids Those acids have more than one ionizable hydrogen atom. The first hydrogen is ionized. The second and all other ionizations are always weak.

  12. Rule #4 - Bases Hydroxides of Groups (IA) and (IIA), except Be, are strong bases and written in ionic form. All others are weak bases and written in molecular form.

  13. Rule #5 - Salts Salts are written in molecular form if they are insoluble. Salts are written in ionic form if they are soluble.

  14. Salt Solubility Rules Salts of Group (IA) and ammonia are soluble. Acetates and nitrates are soluble. Binary compounds of Group (VIIA), except F, with metals, except Ag, Hg+1, and Pb, are soluble.

  15. Salt Solubility Rules All sulfates are soluble, except those of Ba, Sr, Pb, Ca, Ag, and Hg+1. Except for those in Rule 1, carbonates, hydroxides, oxides, sulfides, and phosphates are insoluble.

  16. Rule #6 - oxides Oxides are always written in molecular form.

  17. Rule #7 - gases Gases are always written in molecular form.

  18. Write this in net ionic form: H2SO4(aq) H2O(l) + SO3(aq)

  19. Write this in net ionic form: H2SO4(aq) H2O(l) + SO3(aq) molecule or ion? Which Rule?

  20. Write this in net ionic form: H2SO4(aq) H2O(l) + SO3(aq) H+(aq) + HSO4-(aq)

  21. Write this in net ionic form: H2SO4(aq) H2O(l) + SO3(aq) H+(aq) + HSO4-(aq) molecule or ion? Which Rule?

  22. Write this in net ionic form: H2SO4(aq) H2O(l) + SO3(aq) H+(aq) + HSO4-(aq) H2O(l)

  23. Write this in net ionic form: H2SO4(aq) H2O(l) + SO3(aq) H+(aq) + HSO4-(aq) H2O(l) molecule or ion? Which Rule?

  24. Write this in net ionic form: H2SO4(aq) H2O(l) + SO3(aq) H+(aq) + HSO4-(aq) H2O(l) + SO3(aq)

  25. Write this in net ionic form: H2SO4(aq) H2O(l) + SO3(aq) H+(aq) + HSO4-(aq) H2O(l) + SO3(aq) To check the answer, ask these two questions:

  26. Write this in net ionic form: H2SO4(aq) H2O(l) + SO3(aq) H+(aq) + HSO4-(aq) H2O(l) + SO3(aq) Do both sides of the arrow have the same number of elements?

  27. Write this in net ionic form: H2SO4(aq) H2O(l) + SO3(aq) H+(aq) + HSO4-(aq) H2O(l) + SO3(aq) Do both sides of the arrow have the same total charge?

  28. Spectator ions Ions appearing on BOTH sides of the equation.

  29. Spectator ions They are assumed to take no part in the reaction and are canceled.

  30. Spectator ions They are NOT part of a net ionic equation.

  31. Write in net ionic form 2AgNO3(aq) + H2SO4(aq)   Ag2SO4(cr) + 2HNO3(aq) molecule or ion?

  32. Write in net ionic form 2AgNO3(aq) + H2SO4(aq)   Ag2SO4(cr) + 2HNO3(aq) 2Ag+(aq) + 2NO3-(aq)

  33. Write in net ionic form 2AgNO3(aq) + H2SO4(aq)   Ag2SO4(cr) + 2HNO3(aq) 2Ag+(aq) + 2NO3-(aq) molecule or ion?

  34. Write in net ionic form 2AgNO3(aq) + H2SO4(aq)   Ag2SO4(cr) + 2HNO3(aq) 2Ag+(aq) + 2NO3-(aq) + H+(aq) + HSO4-(aq)

  35. Write in net ionic form 2AgNO3(aq) + H2SO4(aq)   Ag2SO4(cr) + 2HNO3(aq) 2Ag+(aq) + 2NO3-(aq) + H+(aq) + HSO4-(aq) molecule or ion?

  36. Write in net ionic form 2AgNO3(aq) + H2SO4(aq)   Ag2SO4(cr) + 2HNO3(aq) 2Ag+(aq) + 2NO3-(aq) + H+(aq) + HSO4-(aq) Ag2SO4(cr)

  37. Write in net ionic form 2AgNO3(aq) + H2SO4(aq)   Ag2SO4(cr) + 2HNO3(aq) 2Ag+(aq) + 2NO3-(aq) + H+(aq) + HSO4-(aq) Ag2SO4(cr) molecule or ion?

  38. Write in net ionic form 2AgNO3(aq) + H2SO4(aq)   Ag2SO4(cr) + 2HNO3(aq) 2Ag+(aq) + 2NO3-(aq) + H+(aq) + HSO4-(aq) Ag2SO4(cr) + 2H+(aq) + 2NO3-(aq)

  39. Write in net ionic form 2AgNO3(aq) + H2SO4(aq)   Ag2SO4(cr) + 2HNO3(aq) 2Ag+(aq) + 2NO3-(aq) + H+(aq) + HSO4-(aq) Ag2SO4(cr) + 2H+(aq) + 2NO3-(aq) Spectator ions?

  40. Write in net ionic form 2AgNO3(aq) + H2SO4(aq)   Ag2SO4(cr) + 2HNO3(aq) 2Ag+(aq) + 2NO3-(aq) + H+(aq) + HSO4-(aq) Ag2SO4(cr) + 2H+(aq) + 2NO3-(aq) Spectator ions?

  41. Write in net ionic form 2AgNO3(aq) + H2SO4(aq)   Ag2SO4(cr) + 2HNO3(aq) 2Ag+(aq) + 2NO3-(aq) + H+(aq) + HSO4-(aq) Ag2SO4(cr) + 2H+(aq) + 2NO3-(aq) Spectator ions?

  42. Write in net ionic form 2AgNO3(aq) + H2SO4(aq)   Ag2SO4(cr) + 2HNO3(aq) 2Ag+(aq) + HSO4-(aq) Ag2SO4(cr) + H+(aq)

  43. Write in net ionic form 2AgNO3(aq) + H2SO4(aq)   Ag2SO4(cr) + 2HNO3(aq) 2Ag+(aq) + HSO4-(aq) Ag2SO4(cr) + H+(aq) Are elements balanced?

  44. Write in net ionic form 2AgNO3(aq) + H2SO4(aq)   Ag2SO4(cr) + 2HNO3(aq) 2Ag+(aq) + HSO4-(aq) Ag2SO4(cr) + H+(aq) Is the charge the same on both sides of the arrow?

  45. Write in net ionic form 2AgNO3(aq) + H2SO4(aq)   Ag2SO4(cr) + 2HNO3(aq) 2Ag+(aq) + HSO4-(aq) Ag2SO4(cr) + H+(aq) This IS the net ionic equation!

  46. Net Ionic Equations END

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