Redox (continued)
Visão Geral
When iron rusts, when a fuel burns, when a battery drives your phone, the same hidden bargain is taking place: one substance loses something and another gains it. That bargain is a redox reaction, the simultaneous oxidation and reduction that powers an enormous slice of chemistry, biology and industry.
In this lesson you will learn redox three ways: as the gain and loss of oxygen, as the transfer of electrons, and as a change in oxidation number. You will assign oxidation numbers with Roman numerals, spot oxidising and reducing agents, and read the tell-tale colour changes that prove a redox reaction has happened.
Objetivos
- Use a Roman numeral to indicate the oxidation number of an element in a compound.
- Define redox reactions as involving simultaneous oxidation and reduction.
- Define oxidation as gain of oxygen and reduction as loss of oxygen.
- Identify redox reactions as reactions involving gain and loss of oxygen.
- Identify oxidation and reduction in redox reactions.
- [Supplement] Define oxidation in terms of: (a) loss of electrons (b) an increase in oxidation number.
- [Supplement] Define reduction in terms of: (a) gain of electrons (b) a decrease in oxidation number.
- [Supplement] Identify redox reactions as reactions involving gain and loss of electrons.
- [Supplement] Identify redox reactions by changes in oxidation number using: (a) the oxidation number of elements in their uncombined state is zero (b) the oxidation number of a monatomic ion is the same as the charge on the ion (c) the sum of the oxidation numbers in a compound is zero (d) the sum of the oxidation numbers in an ion is equal to the charge on the ion.
- [Supplement] Identify redox reactions by the colour changes involved when using acidified aqueous potassium manganate(VII) or aqueous potassium iodide.
- [Supplement] Define an oxidising agent as a substance that oxidises another substance and is itself reduced.
- [Supplement] Define a reducing agent as a substance that reduces another substance and is itself oxidised.
- [Supplement] Identify oxidising agents and reducing agents in redox reactions.
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Avaliação da Lição
Parabéns por concluir a lição em Redox (continued). Agora que você explorou o conceitos e ideias-chave, é hora de colocar seu conhecimento à prova. Esta seção oferece uma variedade de práticas perguntas destinadas a reforçar sua compreensão e ajudá-lo a avaliar sua compreensão do material.
Irá encontrar uma mistura de tipos de perguntas, incluindo perguntas de escolha múltipla, perguntas de resposta curta e perguntas de redação. Cada pergunta é cuidadosamente elaborada para avaliar diferentes aspetos do seu conhecimento e competências de pensamento crítico.
Use esta secção de avaliação como uma oportunidade para reforçar a tua compreensão do tema e identificar quaisquer áreas onde possas precisar de estudo adicional. Não te deixes desencorajar pelos desafios que encontrares; em vez disso, vê-os como oportunidades de crescimento e melhoria.
- Which statement defines oxidation in terms of electrons? A. Gain of electrons B. Loss of electrons C. Gain of protons D. Loss of neutrons Answer: B
- What is the oxidation number of an element in its uncombined state? A. +1 B. -1 C. 0 D. equal to its group number Answer: C
- In the reaction CuO + H2 -> Cu + H2O, the reducing agent is: A. CuO B. H2 C. Cu D. H2O Answer: B
- An oxidising agent is a substance that: A. is itself oxidised B. oxidises another substance and is itself reduced C. loses oxygen only D. gains electrons from no other species Answer: B
- When iodide ions turn acidified potassium iodide from colourless to yellow-brown, the iodide ions are: A. reduced B. oxidised C. unchanged D. acting as an oxidising agent Answer: B
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Secção do manual
Classifying Chemical Reactions
Define three common types of chemical reactions (precipitation, acid-base, and oxidation-reduction)
"Chemistry: Classifying Chemical Reactions" by OpenStax, OpenStax, Rice University, licensed under CC BY 4.0 (https://creativecommons.org/licenses/by/4.0/). Source: https://openstax.org/books/chemistry/pages/4-2-classifying-chemical-reactions. Access for free at https://openstax.org/books/chemistry/pages/1-introduction
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