Oxidizing and Reducing Agents

Oxidation states of nitrogen Identifying oxidizing and reducing agents 

In general, a substance with an element in one of its highest possible oxidation states is an oxidizing agent. If the element is in one of its lowest possible oxidation states, the substance is a reducing agent. 

In this reaction, N2O4 is the oxidizing agent and N2H4 is the reducing agent. This reaction releases so much energy that it is used in some rocket propulsion systems. 

A red cloth becomes white when immersed in NaOCI(aq), which oxidizes the red pigment to colorless products. 

Thiosulfafe ion, 8203 , is an important reducing agent. One of its industrial uses is as an anticMor to destroy residual chlorine from the bleaching of fibers. 

Look back at the redox ladder for sulfur In Exercise 7D  

An oxidizing agent is a substance that takes up electrons during a chemical reaction and, in doing so, becomes reduced. A reducing agent supplies the electrons in this process and so becomes oxidized. 

When iron is heated in chiorine gas, iron(lll) chloride is produced. The ordinary equation is  

iron is acting as a reducing agent because it supplies electrons to chlorine 

Chiorine is acting as an oxidizing agent because it accepts electrons from iron and 

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Both oxidizing and reducing agents can interfere with this analysis. Explain what effect each of these interferents will have on the result of an analysis. 

Quantitative Calculations The stoichiometry of a redox reaction is given by the conservation of electrons between the oxidizing and reducing agents (see Section 2C) thus... 

Method for the external generation of oxidizing and reducing agents in coulometric titrations. 

Dinitrophenylhydrazones are cleaved by various oxidizing and reducing agents, and by exchange reactions. 

Tliis categor> includes chemicals reacting vitli otlier chemicals or materials and tlie decomposition of unstable chemicals (e.g tlie reaction of some substances witli water or moist air or witli strong oxidizing and reducing agents). 

Figure 11.9 Plot of volt equivalent against oxidation state for various compounds or ions containing N in acidic aqueous solution. Note that values of - AC refer lo N2 as standard (zero) but are quoted per mol of N aloms and per mol of. Nj they refer to reactions in the direction (ox) ne —> (red). Slopes corresponding to some common oxidizing and reducing agents are included for comparison.

Silicon, Phosphorus, and Sulfur Oxidizing and Reducing Agents of Intermediate Strengths... 

Self-Test K.3B When sulfuric acid reacts with sodium iodide, sodium iodate and sulfur dioxide are produced. Identify the oxidizing and reducing agents in this reaction. 

Identify the oxidizing and reducing agents in a reaction (Example K.2). 

Self-Test 14.7B Is the reaction between CaO and SiO, a redox reaction or a Lewis acid-base reaction If redox, identify the oxidizing and reducing agents. If Lewis acid-base, identify the acid and the base. 

Describe the acidic and basic character of water and hydrogen peroxide and compare their functions as oxidizing and reducing agents. 

For a table of oxidation and reduction reactions, and the oxidizing and reducing agents for each, see Hudlicky, M. J. Chem. Educ., 1977, 54, 100. 

Reactions or compounds of exceptional hazard are those involving combinations of powerful oxidants and reducing agents, in the so-called redox reactions or redox compounds. Such systems are capable of very large energy release rates, the best known examples being the propellant pairs used in rocket technology. 

The oxidizing and reducing agents are often inorganic compounds. 

The formula you need for this problem is AG° = -ncSSE°. The Faraday constant, <3, is equal to 9.65 x 104 joules volt-1 mole n is the number of electrons transferred between oxidizing and reducing agents in a balanced redox equation. 

Common dust collection system used for solid oxidizer and reducing agent/combustible material. 

A chemical reaction in which a single compound serves as both oxidizing and reducing agent and is thereby converted into a more oxidized and a more reduced derivative e.g., a hypochlorite upon appropriate heating yields a chlorate and a chloride. 

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