Redox reactions
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contains explanation of redox reaction, differences between oxidation and reduction, related pictures and solved examples along with test your understanding section.
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Redox reaction ( GROUP E )
The oxidation state of nitrogen in (NH4)2SO4 is -3.
The oxidation state of sulfur in (NH4)2SO4 is +6.
The oxidation state of oxygen in (NH4)2SO4 is -2.
Oxidation reduction lesson grade 9
This presentation is designed for teaching the concepts oxidation reduction to students using the 5E strategy.
Redox Reaction
Redox reactions involve the transfer of electrons between substances, causing some substances to be oxidized (lose electrons) and others to be reduced (gain electrons). In the examples given, sodium metal is oxidized when it reacts with bromine gas, losing electrons to become sodium ions. Bromine gas is reduced, gaining electrons to become bromide ions. Zinc metal also undergoes oxidation when reacting with hydrochloric acid, losing electrons to form zinc ions, while hydrogen ions are reduced, gaining electrons to form hydrogen gas. Oxidation numbers are used to indicate the charge of atoms in their elemental or ionic states and can help identify whether a substance is being oxidized or reduced in a redox reaction.
Oxidation reduction reaction
This the reaction that explains the loose or gain oxygen, hydrogen, electron transfer and the increase or decrease of oxidation number.
In this slide, we also talk about the oxidation number: how it is being calculated, examples of element in a compound with their oxidation number
Redox Reactions
The document defines oxidation and reduction (redox) reactions in terms of oxygen/hydrogen gain or loss, electron transfer, and changes in oxidation state. It provides examples of redox reactions like combustion and corrosion. Redox involves both oxidation, defined as gaining oxygen, losing hydrogen, losing electrons, or increasing oxidation state, and reduction, defined as the opposite of these processes. Common oxidizing and reducing agents can be identified through color changes using potassium iodide and dichromate solutions.
3 a redox reaction
The document discusses oxidation, reduction, and redox reactions. It defines oxidation as gain of oxygen, loss of hydrogen, or loss of electrons, and reduction as the opposite. Redox reactions involve both oxidation and reduction occurring simultaneously through the transfer of electrons between reactants.
Topic 7 oxidation and reduction
SUBJECT: CHEMISTRY
TOPIC : Oxidation and Reduction
for grade 10 and 11.IGCSE,MYP,CBSE,SSC and other boards
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The document discusses redox (reduction-oxidation) reactions. It defines oxidation and reduction in terms of electron transfer and changes in oxidation number. Key points include:
1) Redox reactions involve the transfer of electrons from a reducing agent to an oxidizing agent.
2) Oxidation is the loss of electrons or an increase in oxidation number, while reduction is the gain of electrons or a decrease in oxidation number.
3) Oxidizing agents undergo reduction by gaining electrons, while reducing agents undergo oxidation by losing electrons.
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Redox reaction ( GROUP E )
The oxidation state of nitrogen in (NH4)2SO4 is -3.
The oxidation state of sulfur in (NH4)2SO4 is +6.
The oxidation state of oxygen in (NH4)2SO4 is -2.
Oxidation reduction lesson grade 9
This presentation is designed for teaching the concepts oxidation reduction to students using the 5E strategy.
Redox Reaction
Redox reactions involve the transfer of electrons between substances, causing some substances to be oxidized (lose electrons) and others to be reduced (gain electrons). In the examples given, sodium metal is oxidized when it reacts with bromine gas, losing electrons to become sodium ions. Bromine gas is reduced, gaining electrons to become bromide ions. Zinc metal also undergoes oxidation when reacting with hydrochloric acid, losing electrons to form zinc ions, while hydrogen ions are reduced, gaining electrons to form hydrogen gas. Oxidation numbers are used to indicate the charge of atoms in their elemental or ionic states and can help identify whether a substance is being oxidized or reduced in a redox reaction.
Oxidation reduction reaction
This the reaction that explains the loose or gain oxygen, hydrogen, electron transfer and the increase or decrease of oxidation number.
In this slide, we also talk about the oxidation number: how it is being calculated, examples of element in a compound with their oxidation number
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3 a redox reaction
The document discusses oxidation, reduction, and redox reactions. It defines oxidation as gain of oxygen, loss of hydrogen, or loss of electrons, and reduction as the opposite. Redox reactions involve both oxidation and reduction occurring simultaneously through the transfer of electrons between reactants.
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The document discusses redox (reduction-oxidation) reactions. It defines oxidation and reduction in terms of electron transfer and changes in oxidation number. Key points include:
1) Redox reactions involve the transfer of electrons from a reducing agent to an oxidizing agent.
2) Oxidation is the loss of electrons or an increase in oxidation number, while reduction is the gain of electrons or a decrease in oxidation number.
3) Oxidizing agents undergo reduction by gaining electrons, while reducing agents undergo oxidation by losing electrons.
REDOX reactions Balancing by the Ion-electron method (acid medium)
This document provides an overview of how to balance redox reactions using the ion-electron method in an acid medium. It explains the steps as follows:
1) Calculate the oxidation numbers of each atom in the reaction.
2) Identify which elements are being reduced and oxidized.
3) Write the half-reactions in ionic form.
4) Balance each half-reaction, balancing elements other than H/O first, then O, then H.
5) Balance charges by adding electrons.
6) Multiply half-reactions to equalize electrons.
7) Add the half-reactions together to give the complete ionic and molecular equations.
The
C11 redox reactions
The document defines oxidation and reduction as well as oxidizing and reducing agents. It explains that oxidation is the loss of electrons or gain of oxygen, while reduction is the gain of electrons or loss of oxygen. Oxidizing agents cause oxidation by accepting electrons, while reducing agents cause reduction by donating electrons. Redox reactions involve both oxidation and reduction halves that always occur together. Tests are described to identify oxidizing agents using potassium iodide solution, which will turn reddish brown if iodine is liberated, indicating an oxidizing agent is present.
Redox
This document discusses oxidation-reduction (redox) reactions through examples of writing complete and net ionic equations, identifying oxidizing and reducing agents, writing half-reactions, and balancing redox reactions. Key points covered include:
1. Redox reactions involve the transfer of electrons between atoms.
2. Net ionic equations show the ionic form of the reactants and products.
3. The atom that loses electrons is oxidized and acts as the reducing agent. The atom that gains electrons is reduced and acts as the oxidizing agent.
4. Half-reactions allow identifying how many electrons are lost or gained in the oxidation and reduction steps.
5. Balancing redox reactions
C11 redox reactions
The document defines oxidation and reduction as well as oxidizing and reducing agents. It explains that oxidation is the loss of electrons or gain of oxygen, while reduction is the gain of electrons or loss of oxygen. Oxidizing agents cause oxidation by accepting electrons, while reducing agents cause reduction by donating electrons. Redox reactions involve both oxidation and reduction halves that always occur together. Tests are described to identify oxidizing agents using potassium iodide solution, which will turn reddish brown if iodine is liberated, indicating an oxidizing agent is present.
Redox reactions
1. Redox reactions involve the transfer of electrons from one reactant to another. The substance that loses electrons is oxidized and is the reducing agent, while the substance that gains electrons is reduced and is the oxidizing agent.
2. To determine if a substance is reduced or oxidized, ask if it gains or loses electrons. Gaining electrons means it is reduced, while losing electrons means it is oxidized.
3. An example reaction of ethane burning in oxygen is worked through to assign oxidation numbers, determine which substances gain or lose electrons, and identify the reducing and oxidizing agents.
Chemistry - Chp 20 - Oxidation Reduction Reactions - PowerPoint
The document discusses oxidation-reduction (redox) reactions. It defines oxidation as loss of electrons and reduction as gain of electrons. Redox reactions involve the transfer of electrons between reactants. Oxidation numbers are used to identify oxidized and reduced species in redox reactions. Redox equations can be balanced using two methods - comparing oxidation number changes or using half-reactions. Electrochemical cells use spontaneous redox reactions to generate electricity, with oxidation occurring at the anode and reduction at the cathode.
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This document discusses oxidation and reduction reactions. It defines oxidation as a reaction where oxygen combines with an element/compound or where an element loses hydrogen or electrons. Reduction is defined as a reaction where an element gains oxygen, hydrogen, or electrons. Common reducing agents are listed such as lithium aluminium hydride and sodium borohydride. The concept of oxidation state is introduced, which is the charge an atom would have if it existed as an ion in a compound. Rules for determining oxidation states are provided. An example of finding the oxidation states of elements in ammonium sulfate is worked out.
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Oxidation reduction reactions honors
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This document discusses oxidation-reduction (redox) reactions. It defines redox reactions as those involving the loss or gain of electrons. The reactant that loses electrons (gets oxidized) is the reducing agent, while the reactant that gains electrons (gets reduced) is the oxidizing agent. Oxidation is defined as the loss of electrons, while reduction is the gain of electrons. The document also provides examples of variable valence elements that can exist in different oxidation states and outlines the steps for balancing redox equations under acidic and basic conditions.
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The document discusses oxidation and reduction reactions. It defines oxidation as the loss of electrons or an increase in oxidation state, and reduction as the gain of electrons or a decrease in oxidation state. Redox reactions involve both oxidation and reduction occurring simultaneously. Oxidation states can be used to identify what is oxidized and reduced in a reaction. The document provides examples of calculating oxidation states in various compounds and ions using rules like the sum of oxidation states equaling the overall charge.
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An electrochemical cell converts chemical energy into electrical energy through spontaneous redox reactions. It consists of two half-cells separated by a salt bridge. In the cathode half-cell, reduction occurs as oxidized species gain electrons. In the anode half-cell, oxidation occurs as reduced species lose electrons. Electrons flow through an external circuit from the anode to the cathode. The standard electrode potential of each half-reaction predicts the cell's voltage under standard conditions.
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Redox Reactions
Redox reactions involve the transfer of electrons between reactants. They consist of two half-reactions, one of reduction where a species gains electrons and one of oxidation where a species loses electrons. An example is the breathalyzer test where alcohol in the blood is oxidized to acids and water, producing an electric current which is measured to determine blood alcohol level.
Oxidation reduction reactions
The document discusses oxidation-reduction (redox) reactions. It defines oxidation as the loss of electrons and reduction as the gain of electrons. Redox reactions always involve both an oxidation and a reduction process. The substance undergoing oxidation is the reducing agent as it loses electrons, while the substance undergoing reduction is the oxidizing agent as it gains electrons. Assigning oxidation numbers to atoms allows identification of which substances are oxidized and reduced in a reaction.
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This document provides an overview of redox (reduction-oxidation) reactions, including definitions of key terms like oxidation, reduction, oxidizing agents, reducing agents, and disproportionation reactions. It discusses identifying oxidation and reduction based on changes in oxygen, hydrogen, or electron content. Methods for determining oxidation states and balancing redox reactions using the half-reaction method are also described. Real-world examples of redox processes like corrosion and the blue bottle experiment are mentioned.
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This document discusses redox reactions and oxidation states. It defines oxidizing and reducing agents as chemical species that cause the other reactant to be oxidized or reduced, respectively. Redox reactions involve the oxidation of one substance and the reduction of another through electron transfer. Tests are described to identify reducing and oxidizing agents based on their ability to reduce dichromate, manganate, or oxidize iodide ions. The document also explains how to determine the oxidation state of atoms in compounds and polyatomic ions using the fact that the sum of oxidation states equals the overall charge.
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This document defines and provides examples of different types of chemical reactions including synthesis, decomposition, single displacement, double displacement, neutralization, and combustion reactions. It explains the key characteristics of each type of reaction and how to predict the products based on the reactants. Examples are given for each type of reaction to illustrate the concepts.
C6b Redox Reactions
Rusting is an example of a redox reaction where:
1. Iron loses electrons and is oxidized.
2. Oxygen gains electrons and is reduced.
3. For rusting to occur, iron needs to be in contact with both oxygen and water, and acids or salts can catalyze the reaction.
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The document discusses oxidation-reduction (redox) reactions, including definitions and examples. It covers topics like rusting, fire, combustion, fuels, ignition sources, and both everyday and hazardous chemical reactions involving oxidation. Color changes and the role of elements like oxygen, chlorine, and metals are also examined in the context of redox processes.
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3) Write the half-reactions in ionic form.
4) Balance each half-reaction, balancing elements other than H/O first, then O, then H.
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This document discusses oxidation-reduction (redox) reactions through examples of writing complete and net ionic equations, identifying oxidizing and reducing agents, writing half-reactions, and balancing redox reactions. Key points covered include:
1. Redox reactions involve the transfer of electrons between atoms.
2. Net ionic equations show the ionic form of the reactants and products.
3. The atom that loses electrons is oxidized and acts as the reducing agent. The atom that gains electrons is reduced and acts as the oxidizing agent.
4. Half-reactions allow identifying how many electrons are lost or gained in the oxidation and reduction steps.
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The document defines oxidation and reduction as well as oxidizing and reducing agents. It explains that oxidation is the loss of electrons or gain of oxygen, while reduction is the gain of electrons or loss of oxygen. Oxidizing agents cause oxidation by accepting electrons, while reducing agents cause reduction by donating electrons. Redox reactions involve both oxidation and reduction halves that always occur together. Tests are described to identify oxidizing agents using potassium iodide solution, which will turn reddish brown if iodine is liberated, indicating an oxidizing agent is present.
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1. Redox reactions involve the transfer of electrons from one reactant to another. The substance that loses electrons is oxidized and is the reducing agent, while the substance that gains electrons is reduced and is the oxidizing agent.
2. To determine if a substance is reduced or oxidized, ask if it gains or loses electrons. Gaining electrons means it is reduced, while losing electrons means it is oxidized.
3. An example reaction of ethane burning in oxygen is worked through to assign oxidation numbers, determine which substances gain or lose electrons, and identify the reducing and oxidizing agents.
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The document discusses oxidation-reduction (redox) reactions. It defines oxidation as loss of electrons and reduction as gain of electrons. Redox reactions involve the transfer of electrons between reactants. Oxidation numbers are used to identify oxidized and reduced species in redox reactions. Redox equations can be balanced using two methods - comparing oxidation number changes or using half-reactions. Electrochemical cells use spontaneous redox reactions to generate electricity, with oxidation occurring at the anode and reduction at the cathode.
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This document discusses oxidation and reduction reactions. It defines oxidation as a reaction where oxygen combines with an element/compound or where an element loses hydrogen or electrons. Reduction is defined as a reaction where an element gains oxygen, hydrogen, or electrons. Common reducing agents are listed such as lithium aluminium hydride and sodium borohydride. The concept of oxidation state is introduced, which is the charge an atom would have if it existed as an ion in a compound. Rules for determining oxidation states are provided. An example of finding the oxidation states of elements in ammonium sulfate is worked out.
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The document discusses balancing redox reactions using the half-reaction method. It provides several examples of writing and balancing half-reactions and using them to derive the overall balanced redox equation. Key steps include separating the reaction into oxidation and reduction half-reactions, balancing all elements except H and O, adding H2O to balance O, adding H+ or OH- to balance H, and adding electrons to balance charge.
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This document discusses redox reactions and oxidation numbers. It defines oxidation as the gain of oxygen or loss of electrons, and reduction as the loss of oxygen or gain of electrons. Examples are given of redox reactions like burning magnesium and copper in silver nitrate solution. Oxidation numbers are introduced as a way to determine if an element is oxidized or reduced in a reaction by calculating the change in electrons. Practice problems are included to help understand how to identify oxidation states and oxidation numbers.
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The document discusses oxidation-reduction (redox) reactions, where there is a transfer of electrons between reactants. It defines oxidation as the loss of electrons and reduction as the gain of electrons. An example redox reaction and its net ionic form are provided. The document explains how to determine the oxidation states of elements and identifies common oxidation states of nonmetals. It describes how to write half-reactions by separating a redox reaction into its oxidation and reduction components.
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This document discusses oxidation-reduction (redox) reactions. It defines redox reactions as those involving the loss or gain of electrons. The reactant that loses electrons (gets oxidized) is the reducing agent, while the reactant that gains electrons (gets reduced) is the oxidizing agent. Oxidation is defined as the loss of electrons, while reduction is the gain of electrons. The document also provides examples of variable valence elements that can exist in different oxidation states and outlines the steps for balancing redox equations under acidic and basic conditions.
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The document discusses oxidation and reduction reactions. It defines oxidation as the loss of electrons or an increase in oxidation state, and reduction as the gain of electrons or a decrease in oxidation state. Redox reactions involve both oxidation and reduction occurring simultaneously. Oxidation states can be used to identify what is oxidized and reduced in a reaction. The document provides examples of calculating oxidation states in various compounds and ions using rules like the sum of oxidation states equaling the overall charge.
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Redox reactions involve the transfer of electrons between reactants. They consist of two half-reactions, one of reduction where a species gains electrons and one of oxidation where a species loses electrons. An example is the breathalyzer test where alcohol in the blood is oxidized to acids and water, producing an electric current which is measured to determine blood alcohol level.
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The document discusses oxidation-reduction (redox) reactions. It defines oxidation as the loss of electrons and reduction as the gain of electrons. Redox reactions always involve both an oxidation and a reduction process. The substance undergoing oxidation is the reducing agent as it loses electrons, while the substance undergoing reduction is the oxidizing agent as it gains electrons. Assigning oxidation numbers to atoms allows identification of which substances are oxidized and reduced in a reaction.
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This document provides an overview of redox (reduction-oxidation) reactions, including definitions of key terms like oxidation, reduction, oxidizing agents, reducing agents, and disproportionation reactions. It discusses identifying oxidation and reduction based on changes in oxygen, hydrogen, or electron content. Methods for determining oxidation states and balancing redox reactions using the half-reaction method are also described. Real-world examples of redox processes like corrosion and the blue bottle experiment are mentioned.
Redox reactions
This document discusses redox reactions and oxidation states. It defines oxidizing and reducing agents as chemical species that cause the other reactant to be oxidized or reduced, respectively. Redox reactions involve the oxidation of one substance and the reduction of another through electron transfer. Tests are described to identify reducing and oxidizing agents based on their ability to reduce dichromate, manganate, or oxidize iodide ions. The document also explains how to determine the oxidation state of atoms in compounds and polyatomic ions using the fact that the sum of oxidation states equals the overall charge.
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Redox reactions
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This document discusses oxidation-reduction (redox) reactions and concepts related to them. It defines oxidation as the loss of electrons or an increase in oxidation number, and reduction as the gain of electrons or a decrease in oxidation number. Redox reactions involve both an oxidation and a reduction occurring simultaneously. Oxidizing agents undergo reduction, reducing electrons and undergoing oxidation. Methods for determining oxidation numbers and balancing redox equations are also outlined.
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This document provides information on chemical equations and oxidation-reduction reactions. It defines key concepts like oxidation, reduction, oxidizing agents, reducing agents and oxidation numbers. Examples of different types of chemical reactions like combination, decomposition, displacement and combustion are outlined. Steps for writing and balancing chemical equations are described. Oxidation-reduction reactions are explained along with biological examples of electron transfer processes. Specific equations are given and identified as oxidation or reduction reactions.
5.1 electrochemistry
This document discusses electrochemistry and redox reactions. It defines oxidation and reduction, and explains that they occur together in redox reactions. Redox reactions involve the transfer of electrons from one species to another, changing their oxidation states. Oxidizing agents accept electrons from reducing agents. Common oxidizing agents are hydrogen peroxide and chlorine, while common reducing agents are carbon and hydrogen. Redox reactions can be identified by changes in oxidation states and through color changes using indicators like potassium manganate or iodide.
Roca,gabriel geif
This document discusses redox reactions and provides examples. It first defines redox reactions as transfers of electrons between species that change oxidation states. It gives the example of iron being oxidized by hydrogen peroxide in an acid solution.
It then asks to find 5 examples of real-world redox reactions with balanced equations and identification of oxidizing and reducing agents. Examples given include photosynthesis, alkaline batteries, metal tarnish, corrosion, and bleaching, each with balanced equations and identification of oxidizing and reducing agents.
Oxidation- reduction reactions
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References
Tindale, Ritchie et al, 2014, Chemistry for CSEC 2nd Edition, Nelson Thornes. p156-159
Electron Transfer in Redox Reactions Todayhttps://www.sewanhakaschools.org
Chem 101 week 6 pt2
This document contains lecture notes on quantitative analysis in chemistry. It discusses gravimetric analysis, which determines the amount of a substance by converting it into a product that can be isolated and weighed. An example is given of determining the amount of lead in water by precipitating lead sulfate, filtering and weighing the precipitate. A practice problem demonstrates calculating the mass of lead from the mass of lead sulfate precipitate obtained.
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This document discusses various topics related to aqueous solutions and reactions. It begins by defining key terms like solute, solvent, electrolyte and providing examples. It then covers properties of aqueous solutions such as conductivity. Various acid-base reactions and concepts are explained like Brønsted-Lowry acids and bases, neutralization reactions. Oxidation-reduction reactions and oxidation numbers are also discussed. Finally, the document covers concentration of solutions and calculations involving molarity, dilution and preparation of solutions.
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This chapter tell you about the reduction in the Oxidation reaction there he is revolutions their transfer of ions and also about the oxidizing agent in the reducing agent
Ch 22sec1
This document discusses oxidation-reduction (redox) reactions. It defines oxidation as losing electrons and reduction as gaining electrons. Oxidation and reduction always occur together, with one substance being oxidized as it loses electrons and the other being reduced as it gains electrons. The substance being oxidized is the reducing agent and the substance being reduced is the oxidizing agent. Corrosion occurs through redox reactions as metals like iron are oxidized, forming metal oxide compounds.
Chemistry zimsec chapter 6 electrochemistry
1. Electrochemistry involves redox reactions where one element is oxidized and another is reduced. Oxidation is the loss of electrons and an increase in oxidation number, while reduction is the gain of electrons and a decrease in oxidation number.
2. Electrolysis is the passage of an electric current through an ionic substance to cause a non-spontaneous redox reaction. Oxidation occurs at the anode and reduction at the cathode.
3. Aluminum is extracted from bauxite via electrolysis. Bauxite is dissolved in molten cryolite to lower its melting point, then electrolysis separates aluminum ions at the cathode.
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Redox reactions
- 1. aNUSHIKA bANSAL lAKSHMI sURESH VAIBHAVI pATEL sHREYA sHARMA VANSHIKA sHARMA Redox reactions
- 2. REDOXREACTIONS Oxidation reactions are common events in everyday life : Example- combustion of fossil fuel, Corrosion of metals, Dry cells and accumulators, Metabolism of nutrients in human bodies, Photosynthesis in green plants
- 4. Oxidation-ReductionReactions Redox reactions are electron transfer reactions. The process may involve the complete transfer of electrons to form ionic bonds or only a partial transfer or shift of electrons to form covalent bonds. In terms of electronic concept, oxidation is the process which involves loss of electrons whereas reduction is the process which involves gain of electrons.
- 5. OXIDATION REDUCTION Oxidation is the loss of electrons by a particle in a reaction, resulting in an increase in the oxidation number. Ex., Ared – n e- -> Aox Reduction is the gain of electrons by a particle in a reaction that results in a decrease in the oxidation number. Ex., BOX + n e- -> Bred
- 6. Balancing redox reactions Describing the overall electrochemical reaction for a redox process requires a balancing of the component half-reactions for oxidation and reduction. In general, for reactions in aqueous solution, this involves adding H+, OH−, H2O, and electrons to compensate for the oxidation changes.
- 9. Example 2Al + 6HCl → 2AlCl3 + 3H2 2Al → 2Al3+ + 6e- (oxidation) 6e- + 6H+ → 3H2 (reduction) Al is getting oxidized to 2Al3+. As all metals are reducing agents & 6H+ gets reduced to 3H2. Therefore HCl is the oxidizing agent.
- 10. TESTYOURUNDERSTANDING Name the substance oxidized, reduced, oxidizing agent and reducing agent in the following reactions: i. 3MnO2 + 4Al → 3Mn + 2Al2O3 a) MnO2 has lost oxygen to form Mn. Hence MnO2 has been reduced. b) Al has gained oxygen to form 2Al2O3. Hence, Al has been oxidized. c) MnO2 is the oxidizing agent. d) Al is the reducing agent.
- 11. ii. 2Na +Cl2 → 2NaCl a) Sodium loses electron to form Na+. Hence, sodium has been oxidized. b) Chlorine gains electrons to form Cl-. Hence, chlorine has been reduced. c) Sodium is the reducing agent.. d) Chlorine is the oxidizing agent.. iii. Cu + 2AgNO3 → Cu(NO3)2 + 2Ag a) Copper has lost electrons to form Cu2+. Hence, copper has been oxidized &, therefore, is a reducing agent.. b) AgNO3 (Ag+ ion) gains electron to form Ag. Hence, AgNO3 has been reduced &, therefore, is an oxidizing agent..