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AP Net Ionic Equations

AP Net Ionic Equations. AP equations are found in the free response section of the AP test. You will have 3 equations following by a question about the reaction. The equations are of mixed types.

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AP Net Ionic Equations

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  1. AP Net Ionic Equations

  2. AP equations are found in the free response section of the AP test. You will have 3 equations following by a question about the reaction. The equations are of mixed types.

  3. The sections is worth 15 points and is 10% of the free response grade. Free response is 50% of the total AP test grade.

  4. All AP equations “work.” In each case, a reaction will occur. These equations need to be written in net ionic form. All spectator ions must be left out and all ions must be written in ionic form.

  5. Answer 3 equations that must be balanced. • Each equation is followed by a question. • 1 pt for reactants, 2 points for products, and 1 pt for each question.

  6. Strong Acids are: Exception: concentrated sulfuric acid-keep together because it really is 97% H2SO4 and 3% water in the jug. • Strong Bases are:

  7. Weak acids and bases keep together

  8. All molecular substances and nonsoluble compounds must be written together (not ionized!).

  9. Know your solubility rules!!! • Ca(OH)2 and Sr(OH) 2 are moderately soluble and can be written together or as ions. • Ba(OH)2 is soluble and Mg(OH)2 is insoluble. • CaSO4 and SrSO4 are moderately soluble and can be written together or as ions. • Weak electrolytes, such as acetic acid, are not ionized. • Solids and pure liquids are written together, also. • A saturated solution is written in ionic form while a suspension is written together.

  10. Double Replacement Two compounds react to form two new compounds. No changes in oxidation numbers occur. All double replacement reactions must have a “driving force” that removes a pair of ions from solution.

  11. Manganese(II) nitrate solution is mixed with a sodium hydroxide solution

  12. Excess hydrochloric acid is added to an aqueous solution of potassium sulfite

  13. Hydrogen sulfide gas is bubbled through a solution of lead(II) nitrate

  14. A solution of ammonium sulfate is added to a potassium hydroxide solution

  15. Solutions of tripotassium phosphate and zinc nitrate are mixed

  16. Gaseous hydrofluoric acid reacts with solid silicon dioxide.

  17. Single Replacement Rxns Treat like redox reactions. Reaction where one element displaces another in a compound. One element is oxidized and another is reduced. A + BC  B + AC + charges replace + and – charges replace -

  18. Active metals replace less active metals or hydrogen from their compounds in aqueous solution.

  19. Active nonmetals replace less active nonmetals from their compounds in aqueous solution. Each halogen will displace less electronegative (heavier) halogens from their binary salts.

  20. Examples • A piece of aluminum metal is added to a solution of silver nitrate

  21. Small chunks of solid sodium are added to water

  22. Chlorine gas is bubbled into a solution of sodium bromide

  23. Magnesium turnings are added to a solution of iron(III) chloride

  24. Anhydrides Anhydride means “without water.” Water is a reactant in each of these equations.

  25. Memorize the Rules Look for: 1. Oxides + H2O a. metallic oxide + H2O  base b. nonmetallic oxide + H2O  acid

  26. 2. Metal hydride + H2O metal hydroxide + H2

  27. 3. Group 1 and 2 nitride + H2O metal hydroxide + NH3

  28. 4. Phosphorus halide + H2O  H3PO4 or H3PO3 + H(halide) acid

  29. Examples • Excess water is added to solid calcium hydride

  30. Solid lithium hydride is added to water

  31. Solid dinitrogen pentoxide is added to water

  32. Solid potassium oxide is added to water

  33. Phosphorus pentachloride solid is added to water

  34. Methylamine gas is bubbled into distilled water

  35. Oxidation-Reduction Reactions • Redox reactions involve the transfer of electrons. The oxidation numbers of at least two elements must change. • Single replacement, some combination and some decomposition reactions are redox reactions.

  36. To predict the products of a redox reaction, look at the reagents given to see if there is both an oxidizing agent and a reducing agent. • When a problem mentions an acidic or basic solution, it is probably redox.

  37. Examples • A solution of tin(II) chloride is added to an acidified solution of potassium permanganate.

  38. Hydrogen peroxide solution is added to a solution of iron(II) sulfate

  39. Potassium permanganate solution is added to a solution of oxalic acid acidified with a few drops of sulfuric acid.

  40. A piece of iron is added to a solution of iron(III) sulfate.

  41. Solid sodium dichromate is added to an acidified solution of sodium iodide

  42. Potassium permanganate is mixed with an alkaline solution of sodium sulfite

  43. Copper (II) sulfide is oxidized by dilute nitric acid.

  44. A solution of potassium iodide is added to an acidified solution of potassium dichromate.

  45. Acid-Base Neutralization Rxns Acids react with bases to produce water and salts.

  46. Examples Hydrogen sulfide gas is bubbled through a solution of potassium hydroxide

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