Oxidation and Reduction

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Information about Oxidation and Reduction
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Published on March 4, 2010

Author: grazianir

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Oxidation and Reduction : Oxidation and Reduction Oxidation : Oxidation Reaction with oxygen Loss of electrons Oxidation is Loss of e- OiL Reduction : Reduction Less metal than amount of ore Gain of electrons Reduction is Gain of e- RiG RedOx Reactions : RedOx Reactions Oxidation always occurs with Reduction If something loses electrons something else has to gain RedOx Reactions : RedOx Reactions Lose electrons oxidation. Gain electrons reduction. RedOx Reactions : RedOx Reactions Oxidation is loss. Reduction is gain. RedOx Reactions : RedOx Reactions Statues turning green Rusting of iron Combustion of fuel Effects of bleach Browning of fruit Oxidation Numbers : Oxidation Numbers Tells the number of electrons gained or lost Assigned to atoms, may not be actual charge Higher electronegativity get negative values Change during Redox reactions Rules for Oxidation Numbers : Rules for Oxidation Numbers Single, pure elements have an oxidation number of 0. All monatomic ions have an oxidation number equal to their ionic charge. In a compound, oxygen has an oxidation number of 2-. In a compound, hydrogen has an oxidation number of 1+ Rules for Oxidation Numbers : Rules for Oxidation Numbers In compounds, alkali metals have an oxidation number of 1+, alkaline earth metals have an oxidation number 2+, and fluorine has an oxidation number 1-. For a compound, the sum of the oxidation numbers of each atom must equal 0. For a polyatomic ion, the sum of the oxidation numbers of each atom must equal the charge of the ion Review : Review Oxidation and Reduction always occur together As one atoms loses electrons another atoms must gain them Oil Rig Leo goes Ger Examples : Examples Rusting Iron is oxidized Oxygen in air is reduced Nitroglycerine Glycerin is oxidized Nitro is reduced Agents : Agents “Agents” cause the reaction Oxidizing agents Cause oxidation Take the electrons Reduced in process Agents : Agents “Agents” cause the reaction Reducing agents Cause reduction Give the electrons Oxidized in process Examples : Examples Iron rusting Iron is oxidized It is the reducing agent Oxygen is reduced It is the oxidizing agent Show Redox : Show Redox Mg + HCl  MgCl2 + H2 First balance the equation Show Redox : Show Redox Mg + 2 HCl  MgCl2 + H2 First balance the equation Show Redox : Show Redox Mg + 2 HCl  MgCl2 + H2 Mark the oxidation numbers Show Redox : Show Redox 0 +1 -1 +2 -1 0 Mg + 2 HCl  MgCl2 + H2 Mark the oxidation numbers Show Redox : Show Redox 0 +1 -1 +2 -1 0 Mg + 2 HCl  MgCl2 + H2 Oxidation is loss of electrons Show Redox : Show Redox 0 +1 -1 +2 -1 0 Mg + 2 HCl  MgCl2 + H2 Oxidation is loss of electrons More positive numbers Show Redox : Show Redox 0 +1 -1 +2 -1 0 Mg + 2 HCl  MgCl2 + H2 Reduction is gain of electrons Show Redox : Show Redox 0 +1 -1 +2 -1 0 Mg + 2 HCl  MgCl2 + H2 Reduction is gain of electrons Charge gets lower Examples : Examples Magnesium reacting with acid Magnesium is oxidized It is the reducing agent Hydrogen is reduced It is the oxidizing agent

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