1 / 43

Chapter 8 Review: Topics

Balancing Equations Types of Reactions Solubility Rules Net Ionic Equations . Oxidation Numbers REDOX Predicting Products Activity Series. Chapter 8 Review: Topics. A piece of aluminum is placed in a solution of zinc chloride. Type of Reaction:_______________ Reactants Products

barny
Download Presentation

Chapter 8 Review: Topics

An Image/Link below is provided (as is) to download presentation Download Policy: Content on the Website is provided to you AS IS for your information and personal use and may not be sold / licensed / shared on other websites without getting consent from its author. Content is provided to you AS IS for your information and personal use only. Download presentation by click this link. While downloading, if for some reason you are not able to download a presentation, the publisher may have deleted the file from their server. During download, if you can't get a presentation, the file might be deleted by the publisher.

E N D

Presentation Transcript

  1. Balancing Equations Types of Reactions Solubility Rules Net Ionic Equations Oxidation Numbers REDOX Predicting Products Activity Series Chapter 8 Review: Topics

  2. A piece of aluminum is placed in a solution of zinc chloride. • Type of Reaction:_______________ • Reactants • Products • Equation with states of matter • ______________________________

  3. A piece of aluminum is placed in a solution of zinc chloride. Single Displacement. Balance the equation: __Al(s) + __ZnCl2(aq) __ AlCl3(aq) + __Zn(s)

  4. A piece of aluminum is placed in a solution of zinc chloride. Oxidation Numbers: 2 Al (s) + 3 ZnCl2(aq) 2 AlCl3(aq) + 3 Zn(s) Al =___________  Al = ____________ Zn= __________  Zn= ____________ Cl= ___________  Cl = ____________ • REDOX? ______________

  5. A piece of aluminum is placed in a solution of zinc chloride. Oxidation Numbers: 2 Al (s) + 3 ZnCl2(aq) 2 AlCl3(aq) + 3 Zn(s) Al = 0  Al = +3 Zn= +2  Zn= 0 Cl= -1  Cl = -1 REDOX? Yes

  6. A piece of aluminum is placed in a solution of zinc chloride. Oxidation Numbers: 2 Al (s) + 3 ZnCl2(aq) 2 AlCl3(aq) + 3 Zn(s) Al = 0  Al = +3 Zn= +2  Zn= 0 Cl= -1  Cl = -1 Oxidized: ___ Reduced: _____

  7. A piece of aluminum is placed in a solution of zinc chloride. Oxidation Numbers: 2 Al (s) + 3 ZnCl2(aq) 2 AlCl3(aq) + 3 Zn(s) Al = 0  Al = +3 Zn= +2  Zn= 0 Cl= -1  Cl = -1 Oxidized: Al Reduced: Zn

  8. A piece of aluminum is placed in a solution of zinc chloride. Net Ionic Equation: 2Al (s) + 3ZnCl2(aq) 2 AlCl3(aq) + 3Zn(s) _______________________________ _______________________________ Spectator Ion(s): ______________

  9. A piece of aluminum is placed in a solution of zinc chloride. Net Ionic Equation: 2 Al (s) + 3 ZnCl2(aq) 2 AlCl3(aq) + 3 Zn(s) _______________________________ 2 Al + 3 Zn+2  2 Al 3+ + 3 Zn Spectator Ion(s): Cl-

  10. Solid potassium carbonate is heated. • Type of Reaction:_______________ • Reactants • Products • Equation with states of matter • ______________________________

  11. Solid potassium carbonate is heated. Decomposition. Balance the equation: __ K2CO3(s) __ K2O (s) + __CO2(g)

  12. Solid potassium carbonate is heated. Oxidation Numbers: 1 K2CO3(s) 1 K2O (s) + 1 CO2(g) K =___________  K = ____________ C= ___________  C = ____________ O= ___________  O = ____________ • REDOX? ______________

  13. Solid potassium carbonate is heated. Oxidation Numbers: 1 K2CO3(s) 1 K2O (s) + 1 CO2(g) K = +1  K = +1 C = +4  C = +4 O = -2  O = -2 REDOX? No

  14. Solid potassium carbonate is heated. Net Ionic Equation: 1 K2CO3(s) 1 K2O (s) + 1CO2(g) ____________________________ ____________________________ Spectator Ion(s): ______________

  15. Solid potassium carbonate is heated. Net Ionic Equation: 1 K2CO3(s) 1 K2O (s) + 1CO2(g) NONE – no species are aqueous.

  16. Heptene(C7H14) is burned in air. • Type of Reaction:_______________ • Reactants • Products • Equation with states of matter • ______________________________

  17. Heptene(C7H14) is burned in air. Combustion Balance the equation: __C7H14(l) + __O2(g) __CO2(g) + __H2O (l)

  18. Heptene(C7H14) is burned in air. Oxidation Numbers: 2 C7H14(l) + 21 O2(g) 14 CO2(g) + 14 H2O (l) C =___________  C = ____________ H = __________  H = ____________ O = ___________  O = ____________ • REDOX? ______________

  19. Heptene(C7H14) is burned in air. Oxidation Numbers: 2 C7H14(l) + 21 O2(g) 14 CO2(g) + 14 H2O (l) C = -2  C = +4 H = +1  H = +1 O = 0  O = -2 REDOX? Yes

  20. Heptene(C7H14) is burned in air. Oxidation Numbers: 2 C7H14(l) + 21 O2(g) 14 CO2(g) + 14 H2O (l) C = -2  C = +4 H = +1  H = +1 O = 0  O = -2 Oxidized: ___ Reduced: _____

  21. Heptene(C7H14) is burned in air. Oxidation Numbers: 2 C7H14(l) + 21 O2(g) 14 CO2(g) + 14 H2O (l) C = -2  C = +4 H = +1  H = +1 O = 0  O = -2 Oxidized: C Reduced: O

  22. Heptene(C7H14) is burned in air. Net Ionic Equation: 2 C7H14(l) + 21 O2(g) 14 CO2(g) + 14 H2O (l) _____________________________ _______________________________ Spectator Ion(s): ______________

  23. Heptene(C7H14) is burned in air. Net Ionic Equation: 2 C7H14(l) + 21 O2(g) 14 CO2(g) + 14 H2O (l) _______________________________ NONE – no aqueous species.

  24. Magnesium metal is combined with oxygen gas. • Type of Reaction:_______________ • Reactants • Products • Equation with states of matter • ______________________________

  25. Magnesium metal is combined with oxygen gas. Synthesis Balance the equation: __Mg (s) + __O2(g) __MgO (s)

  26. Magnesium metal is combined with oxygen gas. Oxidation Numbers: 2 Mg (s) + 1 O2(g) 2 MgO (s) Mg =___________  Mg = ____________ O = ___________  O = ____________ • REDOX? ______________

  27. Magnesium metal is combined with oxygen gas. Oxidation Numbers: 2 Mg (s) + 1 O2(g) 2 MgO (s) Mg = 0  Mg = +2 O = 0  O = -2 REDOX? Yes

  28. Magnesium metal is combined with oxygen gas. Oxidation Numbers: 2 Mg (s) + 1 O2(g) 2 MgO (s) Mg = 0  Mg = +2 O = 0  O = -2 Oxidized: ___ Reduced: _____

  29. Magnesium metal is combined with oxygen gas. Oxidation Numbers: 2 Mg (s) + 1 O2(g) 2 MgO (s) Mg = 0  Mg = +2 O = 0  O = -2 Oxidized: Mg Reduced: O

  30. Magnesium metal is combined with oxygen gas. Net Ionic Equation: 2 Mg (s) + 1 O2(g) 2 MgO (s) _____________________________ _______________________________ Spectator Ion(s): ______________

  31. Magnesium metal is combined with oxygen gas. Net Ionic Equation: 2 Mg (s) + 1 O2(g) 2 MgO (s) _______________________________ NONE – no aqueous species.

  32. Solid iron(II) sulfide is reacted with aqueous hydrochloric acid. • Type of Reaction:_______________ • Reactants • Products • Equation with states of matter • ______________________________

  33. Solid iron(II) sulfide is reacted with aqueous hydrochloric acid. Double Displacement Balance the equation: __ FeS (s) + __ HCl (aq) __FeCl2(aq) + __H2S (g)

  34. Solid iron(II) sulfide is reacted with aqueous hydrochloric acid. Oxidation Numbers: 1 FeS (s) + 2 HCl (aq) 1 FeCl2(aq) + 1 H2S (g) Fe =___________  Fe = ____________ S = ___________  S = _____________ H =___________  H = _____________ Cl = __________  Cl = _____________ • REDOX? ______________

  35. Solid iron(II) sulfide is reacted with aqueous hydrochloric acid. Oxidation Numbers: 1 FeS (s) + 2 HCl (aq) 1 FeCl2(aq) + 1 H2S (g) Fe = +2  Fe = +2 S = -2  S = -2 H = +1  H = +1 Cl = -1  Cl = -1 • REDOX? No

  36. Solid iron(II) sulfide is reacted with aqueous hydrochloric acid. Net Ionic Equation: 1 FeS (s) + 2 HCl (aq) 1 FeCl2(aq) + 1 H2S (g) _____________________________ _______________________________ Spectator Ion(s): ______________

  37. Solid iron(II) sulfide is reacted with aqueous hydrochloric acid. Net Ionic Equation: 1 FeS (s) + 2 HCl (aq) 1 FeCl2(aq) + 1 H2S (g) __________________________________ 1 FeS (s) + 2 H+(aq)  1 Fe +2(aq) + 1 H2S (g) Spectator ion(s): Cl-

  38. Additional Practice • Chlorine gas is bubbled through a solution of hydrofluoric acid. • Fluorine gas is bubbled through a solution of sodium chloride. • Silver nitrate and potassium iodide solutions are mixed.

  39. Additional Practice • Solid potassium chlorate is heated in the presence of a catalyst. • Solid magnesium oxide is reacted with sulfur dioxide gas.

More Related