1 / 20

Oxidation-Reduction Reactions

LEO SAYS GER. Oxidation-Reduction Reactions. OIL RIG. Oxidation and Reduction ( Redox ). Electrons are transferred Spontaneous redox rxns can transfer energy Electrons (electricity) Heat Non-spontaneous redox rxns can be made to happen with electricity. LEO says GER :.

suchin
Télécharger la présentation

Oxidation-Reduction Reactions

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. LEO SAYS GER Oxidation-Reduction Reactions OIL RIG

  2. Oxidation and Reduction (Redox) • Electrons are transferred • Spontaneous redoxrxns can transfer energy • Electrons (electricity) • Heat • Non-spontaneous redoxrxns can be made to happen with electricity

  3. LEO says GER : Lose Electrons = Oxidation Sodium is oxidized Gain Electrons = Reduction Chlorine is reduced

  4. Rules for Assigning Oxidation NumbersRules 1 & 2 • The oxidation number of any uncombined • element is zero 2. The oxidation number of a monatomic ion equals its charge

  5. Rules for Assigning Oxidation NumbersRules 3 & 4 3.The oxidation number of oxygen in compounds is -2 4. The oxidation number of hydrogen in compounds is +1

  6. Rules for Assigning Oxidation Number Rule 5 5. The sum of the oxidation numbers in the formula of a compound is 0 2(+1) + (-2) = 0 H O (+2) + 2(-2) + 2(+1) = 0 Ca O H

  7. Rules for Assigning Oxidation NumbersRule 6 6. The sum of the oxidation numbers in the formula of a polyatomic ion is equal to its charge X + 4(-2) = -2 S O X + 3(-2) = -1 N O  X = +5  X = +6

  8. EXAMPLE: Each sodium atom loses one electron: Each chlorine atom gains one electron:

  9. Not All Reactions are Redox Reactions Reactions in which there has been no change in oxidation number are not redox rxns. Examples:

  10. Reducing Agents and Oxidizing Agents • The substance reduced is the oxidizingagent • The substance oxidized is the reducingagent Sodium is oxidized – it is the reducing agent Chlorine is reduced – it is the oxidizing agent

  11. Trends in Oxidation and Reduction Active metals: • Lose electrons easily • Are easily oxidized • Are strong reducingagents Active nonmetals: • Gain electrons easily • Are easily reduced • Are strong oxidizing agents

  12. Electrochemical Terminology Electrode: A conductor used to establish contact with a nonmetallic part of a circuit, such as an electrolyte Half-cell: a metal electrode in contact with a solution of its own ions Anode: The electrode where oxidation takes place Cathode: The electrode where reduction takes place

  13. Voltaic Cells Anode: negative Cathode: positive Voltaic cells: Electrochemical cells in which a spontaneous redox reaction can be harnessed to produce an electric current.

  14. Zinc – Copper Battery

  15. Zinc-Carbon Dry Cell Battery

  16. Electrolytic Cells Cathode: negative Anode: positive Electrolytic cells: Electrochemical cell in which an electric current is used to drive a non-spontaneous process

  17. Electrolysis of H2O Electrolyte is usually dilute sulfuric acid 2H2O  2H2 + O2

  18. Electroplating of Silver Cathode is the object to be plated Anode is a piece of the plating metal Solution contains ions of the plating metal

More Related