Respectively which is the strongest reducing agent

These data allow us to compare the oxidative and reductive strengths of a variety of substances. The strongest oxidant in the table is F 2 , with a standard electrode potential of 2. This high value is consistent with the high electronegativity of fluorine and tells us that fluorine has a stronger tendency to accept electrons it is a stronger oxidant than any other element.

Not all oxidizers and reducers are created equal. Examples of strong oxidizers include hydrogen peroxide, permanganate, and osmium tetroxide. Reducing agents are typically electropositive elements such as hydrogen, lithium, sodium, iron, and aluminum, which lose electrons in redox reactions. Hydrides compounds that contain hydrogen in the formal -1 oxidation state , such as sodium hydride, sodium borohydride and lithium aluminum hydride, are often used as reducing agents in organic and organometallic reactions.

This fact might be surprising because cesium, not lithium, is the least electronegative element. The apparent anomaly can be explained by the fact that electrode potentials are measured in aqueous solution, where intermolecular interactions are important, whereas ionization potentials and electron affinities are measured in the gas phase. Lithium metal is therefore the strongest reductant most easily oxidized of the alkali metals in aqueous solution.

Elemental fluorine, for example, is the strongest common oxidizing agent. F 2 is such a good oxidizing agent that metals, quartz, asbestos, and even water burst into flame in its presence. Other good oxidizing agents include O 2 , O 3 , and Cl 2 , which are the elemental forms of the second and third most electronegative elements, respectively.

Another place to look for good oxidizing agents is among compounds with unusually large oxidation states, such as the permanganate MnO 4 - , chromate CrO 4 2- , and dichromate Cr 2 O 7 2- ions, as well as nitric acid HNO 3 , perchloric acid HClO 4 , and sulfuric acid H 2 SO 4.

These compounds are strong oxidizing agents because elements become more electronegative as the oxidation states of their atoms increase.

Good reducing agents include the active metals, such as sodium, magnesium, aluminum, and zinc, which have relatively small ionization energies and low electro-negativities.

Some compounds can act as either oxidizing agents or reducing agents. One example is hydrogen gas, which acts as an oxidizing agent when it combines with metals and as a reducing agent when it reacts with nonmetals. Another example is hydrogen peroxide, in which the oxygen atom is in the -1 oxidation state.

To help eliminate confusion, there is a mnemonic device to help determine oxidizing and reducing agents. Identify the oxidizing agent and the reducing agent in the following redox reaction:. Note that while a specific atom typically has an odization state changes, the agents are the actual species, not the atoms.

Oxidizing and reducing agents are important in industrial applications. They are used in processes such as purifying water, bleaching fabrics, and storing energy such as in batteries and gasoline.

Oxidizing and reducing agents are especially crucial in biological processes such as metabolism and photosynthesis.

All combustion reactions are also examples of redox reactions. A combustion reaction occurs when a substance reacts with oxygen to create heat. One example is the combustion of octane, the principle component of gasoline:. 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.

Oxidizing and Reducing Agents An oxidizing agent , or oxidant , gains electrons and is reduced in a chemical reaction.

An oxidizing agent oxidizes other substances and gains electrons; therefore, its oxidation state decreases. Applications Oxidizing and reducing agents are important in industrial applications. 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.