1 / 11

Oxidizing & Reducing Agents

Oxidizing & Reducing Agents. Oxidizing Agents  An oxidizing agent , or oxidant , gains electrons and is reduced in a chemical reaction. Reducing Agents  A reducing agent, or reductant , loses electrons and is oxidized in a chemical reaction. Mg (s) + S (s)  Mg S (s). oxidized.

onawa
Download Presentation

Oxidizing & Reducing Agents

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. Oxidizing & Reducing Agents

  2. Oxidizing Agents An oxidizing agent, or oxidant, gains electrons and is reduced in a chemical reaction. Reducing Agents  A reducing agent, or reductant, loses electrons and is oxidized in a chemical reaction. Mg(s) + S(s)  Mg S(s) oxidized reduced 0 0 +2 -2 Reducing Agent Oxidizing Agent

  3. Reference Table J Strongest reducing agent – Oxidize the most Strongest oxidizing agent – Reduce the most

  4. How to Identify Reducing and Oxidizing Agents Cl2 (aq) + 2 Br- (aq)  2 Cl- (aq) + Br2 (aq) Oxidation: 2 Br- (aq)  Br2 (aq) Oxidation States:-1                   0 Reduction: Cl2 (aq)  2 Cl- (aq) Oxidation States:  0                  -1 * Br- loses an electron; it is oxidized from Br- to Br2.Br- is the reducing agent. * Cl2gains one electron; it is reduced from Cl2 to 2 Cl-.  Cl2 is the oxidizing agent.

  5. Learning Check: Which are the oxidizing and reducing agents? Pb + NaNO3 PbO + NaNO2 Pb loses 2e- to become Pb+2, so it is oxidized. N+5 gains 2e- to become N+3, so it is reduced. 0 +1 +5 -2 +2 -2 +1 +3 -2

  6. Calculating Potentials Chart on p. 469 shows reduction potentials *For oxidation: reverse rxn, change the sign What is the maximum voltage that can be obtained from an electrochemical cell with Zn/Zn2+ and Cu/Cu2+? Use Table J to see which oxidizes or reduces. Zn oxidizes, Cu reduces Reduces: Cu2+ + 2e-  Cu 0.34 V Oxidizes: Zn  Zn2+ + 2e- 0.76 V 1.10 V ** Positive voltage = spontaneous

  7. Learning Check: Using the table of standard potentials (p. 469), calculate the theoretical voltage. Cu/Cu2+ and Mg/Mg2+ Oxidation: Mg  Mg2+ + 2e- 2.37 V Reduction: Cu2+ + 2e-  Cu 0.34 V 2.7 V Mg/Mg2+ and Zn/Zn2+ Oxidation: Mg  Mg2+ + 2e- 2.37 V Reduction: Zn2+ + 2e-  Zn - 0.76 V 1.6 V

More Related