11B_Reactivity Series.pptx

REACTIVITY OF METALS REDOX REACTIONS & EQUATIONS REACTIVITY SERIES OF METALS Metals can be ranked by their tendency to give away their electrons (undergo oxidation) or accept electrons (undergo reduction). The more readily a metal gives away its electrons, the less likely it is willing to acc...

REACTIVITY OF METALS REDOX REACTIONS & EQUATIONS REACTIVITY SERIES OF METALS Metals can be ranked by their tendency to give away their electrons (undergo oxidation) or accept electrons (undergo reduction). The more readily a metal gives away its electrons, the less likely it is willing to accept electrons from other metals. l l. c a Oxidants undergo Re reduction (equation listed left to right) l l. c a Reductants undergo Re oxidation (reverse direction of equation) COMPARING REACTIVITIES When metals interact with or , they undergo oxidation. The metals listed to the right lead to the most vigorous reactions. METAL DISPLACEMENT REACTIONS Metal Displacement: The ions from one metal are replaced by the ions of another metal. Metal displacement reactions may occur spontaneously (reactions that do not require catalysts) between the strongest oxidising agent and the strongest reducing agent in a solution. METAL DISPLACEMENT REACTIONS Example. An iron nail () is suspended in a solution of cations. The solution is connected via salt bridge to a solution of ions, with a copper rod () placed inside it. METAL DISPLACEMENT REACTIONS Example. An iron nail () is suspended in a solution of cations. The solution is connected via salt bridge to a solution of ions, with a copper rod () placed inside it. We can determine the direction of a spontaneous redox reaction between two metals by looking at their positions on the reactivity series. Recall is the strongest oxidising agent and so undergoes. displacement Metal reduction: reactions occur (s) between the strongest oxidising is the strongest reducing and reducing agent and so undergoes agents in a solution. oxidation: (aq)  METAL DISPLACEMENT REACTIONS Example. An iron nail () is suspended in a solution of cations. The solution is connected via salt bridge to a solution of ions, with a copper rod () placed inside it. l l ca Combining the oxidation and reduction half-equations forms the Re. overall equation. Oxidation: (aq) Reduction:(s) Overall: (s) (s) WRITING REDOX FULL- EQUATIONS Worked Example 6. Write the balanced overall redox equation, if any, that would occur in the following scenario. Do not include spectator ions in the overall redox equation. A strip of zinc metal, (s) is added to a solution of silver nitrate, (aq). WRITING REDOX FULL- EQUATIONS Worked Example 6. Write the balanced overall redox equation, if any, that would occur in the following scenario. Do not include spectator ions in the overall redox equation. A strip of zinc metal, (s) is added to a solution of silver nitrate, (aq). Metals Involved: (aq) Reduction: ((s) ) Spontaneous reactions create a Oxidation: reverse Z (aq) on the reactivity series. Overall: (s) (s) WRITING REDOX FULL- EQUATIONS Worked Example 7. Write the balanced overall redox equation, if any, that would occur in the following scenario. Do not include spectator ions in the overall redox equation. A strip of zinc metal, (s) is added to a solution of aluminium sulfate, (aq). WRITING REDOX FULL- EQUATIONS Worked Example 7. Write the balanced overall redox equation, if any, that would occur in the following scenario. Do not include spectator ions in the overall redox equation. A strip of zinc metal, (s) is added to a solution of aluminium sulfate, (aq). Metals Involved: (aq) Model Written Recall Response:. Spontaneous Since is a less reactive reactions create a metal than it will not be reverse Z able to displace the ions on the reactivity from the ions. Therefore, series. there will be no observed reaction. Since this reaction does not is a spectator ion and will have a reverse Z, not take part in any this reaction cannot be COMPARING METAL REACTIVITIES We can compare the reactivity of two metals experimentally. Setup: Beaker 1: Metal A (s) + Metal B (aq) () Beaker 2: Metal A (aq) () + Metal B (s) Observation: One beaker will record a reaction, one Exam will not. ple. The beaker that records the reaction has the more reactive metal in solid form as a reactant. Recall. Higher metal reactivity = stronger reducing agent