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Redox

A-Level AQA Chemistry

This pack of flashcards covers fundamental concepts of redox chemistry, including definitions of oxidation and reduction, assigning oxidation numbers, identifying oxidizing and reducing agents, and the composition of half equations. It also explains the balancing of redox equations and the role of electrons in these processes.

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"Describe oxidation."	"Oxidation is the process of electron loss."
"Describe reduction."	"Reduction is the process of electron gain."
"What are the rules for assigning oxidation numbers?"	"1. All uncombined elements have an oxidation number of zero. 2. The oxidation numbers of the elements in a compound add up to zero. 3. The oxidation number of a monoatomic ion is equal to the ionic charge. 4. In a polyatomic ion, the sum of the individual oxidation numbers of the elements adds up to the charge on the ion. 5. Several elements have invariable oxidation numbers in their common compounds."
"Define oxidizing agent."	"An oxidizing agent (or oxidant) is the species that causes another element to oxidize. It is itself reduced in the reaction."
"Define reducing agent."	"A reducing agent (or reductant) is the species that causes another element to reduce. It is itself oxidized in the reaction."
"Describe a reduction half equation."	"A reduction half equation only shows the parts of a chemical equation involved in reduction. The electrons are on the left."
"Describe an oxidation half equation."	"An oxidation half equation only shows the parts of a chemical equation involved in oxidation. The electrons are on the right."
"Describe the process of balancing redox equations."	"The process of balancing redox equations involves determining the oxidation numbers of the elements being oxidized and reduced, adding electrons to the appropriate side of the equation to balance the change in oxidation number, and ensuring that the sum of charges on the reactant side equals the sum of charges on the product side."
"What is the purpose of adding electrons to half equations?"	"The purpose of adding electrons to half equations is to balance the change in oxidation number."
"How do you balance half equations that involve substances with varying amounts of oxygen?"	"Half equations involving substances with varying amounts of oxygen are balanced by adding H+, OH- ions, and H2O."
"Define oxidation number."	"Oxidation number is the charge that an atom would have if the compound or ion were purely ionic."

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Describe oxidation.

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Oxidation is the process of electron loss.

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[{"id":979801,"front":"Describe oxidation.","back":"Oxidation is the process of electron loss.","front_language":"English","back_language":"English","front_image":"","back_image":"","order":0,"explanation":"Oxidation involves the loss of electrons, leading to an increase in the oxidation state of a substance. This process is fundamental in various chemical reactions, such as combustion and rusting. It is a key concept in understanding redox reactions in chemistry.","deleted_at":null,"flashcard_deck_id":"ly8EZ","original_id":null,"examMode":{"text":"","correct":"","incorrect":"","info":""}},{"id":979802,"front":"Describe reduction.","back":"Reduction is the process of electron gain.","front_language":"English","back_language":"English","front_image":"","back_image":"","order":0,"explanation":"Reduction is a chemical process that involves the gain of electrons. It occurs when a species accepts electrons from another species, resulting in a decrease in its oxidation state. This transfer of electrons allows for the formation of new chemical bonds and the conversion of one substance into another. Reduction is an essential part of many biological and chemical reactions, including photosynthesis, respiration, and the production of metals from their ores. It is often accompanied by oxidation, forming a redox reaction.","deleted_at":null,"flashcard_deck_id":"ly8EZ","original_id":null,"examMode":{"text":"","correct":"","incorrect":"","info":""}},{"id":979803,"front":"What are the rules for assigning oxidation numbers?","back":"1. All uncombined elements have an oxidation number of zero. 2. The oxidation numbers of the elements in a compound add up to zero. 3. The oxidation number of a monoatomic ion is equal to the ionic charge. 4. In a polyatomic ion, the sum of the individual oxidation numbers of the elements adds up to the charge on the ion. 5. Several elements have invariable oxidation numbers in their common compounds.","front_language":"English","back_language":"English","front_image":"","back_image":"","order":0,"explanation":"The rules for assigning oxidation numbers are based on the concept of electron transfer in chemical reactions. Each element in a compound is assigned an oxidation number based on certain rules. These rules include: uncombined elements have an oxidation number of zero, the sum of oxidation numbers in a compound is zero, the oxidation number of a monoatomic ion is equal to its ionic charge, the sum of oxidation numbers in a polyatomic ion is equal to its charge, and certain elements have fixed oxidation numbers in their common compounds. These rules help determine the distribution of electrons in a compound and provide a way to track the transfer of electrons during chemical reactions.","deleted_at":null,"flashcard_deck_id":"ly8EZ","original_id":null,"examMode":{"text":"","correct":"","incorrect":"","info":""}},{"id":979804,"front":"Define oxidizing agent.","back":"An oxidizing agent (or oxidant) is the species that causes another element to oxidize. It is itself reduced in the reaction.","front_language":"English","back_language":"English","front_image":"","back_image":"","order":0,"explanation":"Oxidizing agents are substances that facilitate the oxidation of other substances by accepting electrons. This process causes the oxidizing agent to be reduced while the other substance is oxidized. This definition aligns with the fundamental principles of redox reactions in chemistry.","deleted_at":null,"flashcard_deck_id":"ly8EZ","original_id":null,"examMode":{"text":"","correct":"","incorrect":"","info":""}},{"id":979805,"front":"Define reducing agent.","back":"A reducing agent (or reductant) is the species that causes another element to reduce. It is itself oxidized in the reaction.","front_language":"English","back_language":"English","front_image":"","back_image":"","order":0,"explanation":"A reducing agent is a substance that donates electrons to another chemical species, causing it to undergo reduction. This results in the reducing agent itself being oxidized. This process is fundamental in various chemical reactions, such as in redox reactions and industrial processes.","deleted_at":null,"flashcard_deck_id":"ly8EZ","original_id":null,"examMode":{"text":"","correct":"","incorrect":"","info":""}},{"id":979806,"front":"Describe a reduction half equation.","back":"A reduction half equation only shows the parts of a chemical equation involved in reduction. The electrons are on the left.","front_language":"English","back_language":"English","front_image":"","back_image":"","order":0,"explanation":"A reduction half equation focuses solely on the reduction process in a chemical reaction, omitting the oxidation components. Electrons are depicted on the left side to illustrate their involvement in the reduction reaction. This simplifies the representation of the reduction process.","deleted_at":null,"flashcard_deck_id":"ly8EZ","original_id":null,"examMode":{"text":"","correct":"","incorrect":"","info":""}},{"id":979807,"front":"Describe an oxidation half equation.","back":"An oxidation half equation only shows the parts of a chemical equation involved in oxidation. The electrons are on the right.","front_language":"English","back_language":"English","front_image":"","back_image":"","order":0,"explanation":"An oxidation half equation is a representation of the oxidation process in a chemical reaction. It focuses on the species that are being oxidized and shows the transfer of electrons. In an oxidation half equation, the electrons are always shown on the right side, indicating their loss by the oxidized species. This representation allows for a clear understanding of the oxidation process and the flow of electrons.","deleted_at":null,"flashcard_deck_id":"ly8EZ","original_id":null,"examMode":{"text":"","correct":"","incorrect":"","info":""}},{"id":979809,"front":"Describe the process of balancing redox equations.","back":"The process of balancing redox equations involves determining the oxidation numbers of the elements being oxidized and reduced, adding electrons to the appropriate side of the equation to balance the change in oxidation number, and ensuring that the sum of charges on the reactant side equals the sum of charges on the product side.","front_language":"English","back_language":"English","front_image":"","back_image":"","order":0,"explanation":"Balancing redox equations is necessary to ensure that the number of atoms and charges are conserved. This is achieved by assigning oxidation numbers to the elements involved, adding electrons to balance the change in oxidation number, and adjusting coefficients to balance the number of atoms. The goal is to have the total charge and number of atoms equal on both sides of the equation.","deleted_at":null,"flashcard_deck_id":"ly8EZ","original_id":null,"examMode":{"text":"","correct":"","incorrect":"","info":""}},{"id":979810,"front":"What is the purpose of adding electrons to half equations?","back":"The purpose of adding electrons to half equations is to balance the change in oxidation number.","front_language":"English","back_language":"English","front_image":"","back_image":"","order":0,"explanation":"Adding electrons to half equations is necessary to balance the change in oxidation number. This is because electrons are involved in the transfer of charge during a redox reaction. By adding the appropriate number of electrons to the half equation, the overall charge is balanced, ensuring that the reaction obeys the law of conservation of charge. This allows for a complete and accurate representation of the redox reaction.","deleted_at":null,"flashcard_deck_id":"ly8EZ","original_id":null,"examMode":{"text":"","correct":"","incorrect":"","info":""}},{"id":979811,"front":"How do you balance half equations that involve substances with varying amounts of oxygen?","back":"Half equations involving substances with varying amounts of oxygen are balanced by adding H+, OH- ions, and H2O.","front_language":"English","back_language":"English","front_image":"","back_image":"","order":0,"explanation":"Half equations involving substances with varying amounts of oxygen are balanced by adding H+, OH- ions, and H2O. This is because the addition of H+ ions helps balance the hydrogen atoms, OH- ions balance the oxygen atoms, and H2O molecules balance both hydrogen and oxygen atoms. This ensures that the number of atoms on both sides of the equation is equal, maintaining the law of conservation of mass.","deleted_at":null,"flashcard_deck_id":"ly8EZ","original_id":null,"examMode":{"text":"","correct":"","incorrect":"","info":""}},{"id":979812,"front":"Define oxidation number.","back":"Oxidation number is the charge that an atom would have if the compound or ion were purely ionic.","front_language":"English","back_language":"English","front_image":"","back_image":"","order":0,"explanation":"Oxidation number is a measure of the charge that an atom carries in a compound or ion. It is based on the assumption that the compound or ion is purely ionic, meaning that electrons are completely transferred from one atom to another. Oxidation number helps in determining the electron distribution and the degree of oxidation or reduction in a chemical reaction.","deleted_at":null,"flashcard_deck_id":"ly8EZ","original_id":null,"examMode":{"text":"","correct":"","incorrect":"","info":""}}]

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