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The term oxidation is named after oxygen, which is the most common oxidizing agent. Oxygen has a strong attraction for electrons, and in most chemical reactions it will take two electrons away from another atom (or from two atoms, such as in the case of the famous water molecule which is composed of one oxygen atom and two hydrogen atoms). So when an atom loses one or more electrons, it is oxidized.
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Is iodide an oxidising agent?
No iodide is a reducing (the opposite of oxidizing) agent at least with potassium iodide.
How is it possible for hydrogen peroxide to be both an oxidizing agent and reducing agent?
Hydrogen peroxide can act as an oxidizing agent by accepting electrons from other substances, causing them to be oxidized. It can also act as a reducing agent by donating electrons to other substances, causing them to be reduced. The ability of hydrogen peroxide to both accept and donate electrons allows it to exhibit both oxidizing and reducing properties.
What does the reducing agent in a redox reaction do?
reduces another atom
Is germanium ii chloride an oxidizing or reducing agent?
As there is no oxygen in the compound (GeCl2), it would be a reducing agent (especially in HCl).
Is potassium dichromate a reducing agent?
No, potassium dichromate is an oxidizing agent. It can accept electrons from other substances, causing the other substances to be oxidized.
What is the relationship between oxidizing and oxidizing agent?
An oxidizing agent is a substance that causes another substance to be oxidized. Oxidation refers to the loss of electrons by a substance, while reduction refers to the gain of electrons. In a redox reaction, the oxidizing agent itself gets reduced as it accepts electrons from the substance being oxidized.
Is iodide an oxidising agent?
No iodide is a reducing (the opposite of oxidizing) agent at least with potassium iodide.
Is MNO2 a oxidising agent?
Yes, MnO2 is an oxidizing agent as it can accept electrons from other substances, causing them to be oxidized in a chemical reaction. It commonly acts as a strong oxidizing agent in various chemical reactions.
What are correct regarding the reaction between potassium ferrocyanide and KMnO4 in acidic solution Permanganate ion is the oxidizing agent or Oxidized?
permanganate ion is an oxidising agent and is reduced.
How is it possible for hydrogen peroxide to be both an oxidizing agent and reducing agent?
Hydrogen peroxide can act as an oxidizing agent by accepting electrons from other substances, causing them to be oxidized. It can also act as a reducing agent by donating electrons to other substances, causing them to be reduced. The ability of hydrogen peroxide to both accept and donate electrons allows it to exhibit both oxidizing and reducing properties.
What does the reducing agent in a redox reaction do?
reduces another atom
Is germanium ii chloride an oxidizing or reducing agent?
As there is no oxygen in the compound (GeCl2), it would be a reducing agent (especially in HCl).
Is potassium dichromate a reducing agent?
No, potassium dichromate is an oxidizing agent. It can accept electrons from other substances, causing the other substances to be oxidized.
What is the equation for the oxidation of ethanoic anhydride by potassium permanganate?
Ethanoic anhydride can no longer be oxidized by any oxidizing agent.
Sulphur dioxide can act as oxidising agent only?
Sulfur dioxide can act both as an oxidizing agent and a reducing agent. As an oxidizing agent, sulfur dioxide can be reduced to sulfur or sulfite ions. As a reducing agent, sulfur dioxide can be oxidized to sulfur trioxide or sulfuric acid.
How can cyclohexane be oxidized into cyclohexanone?
Cyclohexane can be oxidized into cyclohexanone by using an oxidizing agent such as potassium permanganate (KMnO4) or sodium dichromate (Na2Cr2O7) in the presence of a catalyst like sulfuric acid (H2SO4). The cyclohexane reacts with the oxidizing agent, resulting in the formation of cyclohexanol, which is further oxidized to cyclohexanone.
What are the reducing and oxidizing agents of the reaction FeCl plus SnCl?
In this reaction, FeCl2 is the oxidizing agent because it causes another species to be reduced (lose electrons), while SnCl2 is the reducing agent because it causes another species to be oxidized (gain electrons).
