Summary By looking at each element's oxidation state on the reactant side of a chemical equation compared with the same element's oxidation state on the product side, one can determine if the element is reduced or oxidized, and can therefore identify the oxidizing and reducing agents of a chemical reaction.
Reduced Oxidized. Is B the oxidizing or reducing agent? Which one is reduced and which one is oxidized? In a redox reaction, there must be an oxidizing agent and no reducing agent a reducing agent and no oxidizing agent a reducing agent and an oxidizing agent no reducing or oxidizing agent Which of the following is a strong reducing agent?
Which of the following is a strong oxidizing agent? Remember that gaining electrons means it is "reduced". Keep in mind that losing electrons means it is "oxidized". In this reaction, hydrogen loses one electron. Hydrogen is oxidized, thus making it the reducing agent. An element that is oxidized is a reducing agent, because the element loses electrons, and an element that is reduced is an oxidizing agent, because the element gains electrons.
Because this oxidation state lies between the extremes of the more common 0 and -2 oxidation states of oxygen, H 2 O 2 can act as either an oxidizing agent or a reducing agent. Spontaneous oxidation-reduction reactions convert the stronger of a pair of oxidizing agents and the stronger of a pair of reducing agents into a weaker oxidizing agent and a weaker reducing agent. On the basis of many such experiments, the common oxidation-reduction half-reactions have been organized into a table in which the strongest reducing agents are at one end and the strongest oxidizing agents are at the other, as shown in the table below.
By convention, all of the half-reactions are written in the direction of reduction. Furthermore, by convention, the strongest reducing agents are usually found at the top of the table. Fortunately, you don't have to memorize these conventions. Featured Video. Cite this Article Format. Helmenstine, Anne Marie, Ph. What Is an Oxidizing Agent? Oxidation Reduction Reactions—Redox Reactions.
Metals Versus Nonmetals - Comparing Properties. Oxidation and Reduction Reaction Example Problem. Oxidation Definition and Example in Chemistry. What Does Reactivity Mean in Chemistry? Find the Anode and Cathode of a Galvanic Cell.
Your Privacy Rights. However, oxidizing materials can supply combustible substances with oxygen and support a fire even when air is not present.
Although most oxidizing materials do not burn themselves, they can produce very flammable or explosive mixtures when combined with combustible materials like:. Some oxidizing materials are also incompatible with non-combustible materials. These oxidizers can undergo dangerous reactions with water, inorganic acids or even other oxidizing materials.
The MSDS for a particular oxidizing material should explain what other substances the oxidizer is incompatible with reacts in a dangerous fashion and any other conditions, such as heat, shock or friction, that could result in dangerous chemical reactions.
Oxidizing materials may be toxic or corrosive. Depending on the material, route of exposure inhalation, eye or skin contact, or swallowing and dose, they could harm the body. Corrosive oxidizers can also attack and destroy metal. The MSDSs and the container labels should explain all of the hazards of the oxidizing materials that you use in the workplace. An example is ammonium perchlorate. This material is a white or colourless, odourless crystals. It is used in explosives and fireworks; as an oxidizing agent in solid rocket and missile propellants; as an adhesive; as an engraving agent; laboratory analytical reagent; chemical intermediate for alkali and alkaline metal perchlorates; animal feed supplement; and in oxygen-generating devices for life-support systems in submarines, spacecraft, bomb shelters and breathing apparatus.
Ammonium perchlorate can decompose at high temperatures forming toxic gases, such as chlorine, hydrogen chloride and nitrogen oxides. Closed containers or tanks may rupture and explode if heated.
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