Weba) i) Hydration enthalpy of ion is more than ion because of smaller size of F – ion than Cl– ion. ii) is a reducing agent, whereas is an oxidising agent in group oxides because sulphur is more stable in +6 state and Tellurium is more stable in +4 state. b) 2F 2 + 2H 2 O -------> 4HF + O 2. I 2 doesnot react with water because I 2 is a weak ... Web30 Apr 2007 · Hydrogen peroxide is a powerful oxidising agent but is unusual in that it can act as reducing agent under certain conditions. The oxidation number of oxygen in hydrogen peroxide is -1, intermediate between 0 in oxygen and -2 in water, and this allows the oxygen to act as both a reductant and oxidant in either acid (H 2 O 2) or alkali (HO 2 ...
Why is SO2 a reducing agent and TeO2 an oxidising agent?
Web21 Sep 2024 · Oxidizing and Reducing Agents. A process in which one or more reactants combine together to form one or more different substances, called products. The forming substances are called chemical elements or compounds. A chemical reaction results in the rearrangement of the constituent atoms of the reactants to result in the formation of … WebIf sulfur goes from an oxidation state of +4 to +6 it is oxidizing and therefore can act as a reducing agent. Note that based on its placement in group 16 sulfur might prefer to be in a -2 oxidation state, which would suggest that sulfite can also act as an oxidizing agent in some circumstances. mexico in miss universe
Oxidizing agent - Wikipedia
WebReducing agents donate electrons while oxidising agents gain electrons. Both have various applications in chemistry. Redox reactions involve both reduction and oxidation taking … WebOxidizing and reducing agents. In a chemical reaction the substance to which oxygen is added or hydrogen is removed is said to be oxidized and the substance oxidized is the reducing agent and the substance which gets reduced is the oxidizing agent. Examples. The first example is as follows:-Reaction: 2 Na (s) + Cl 2 (g) → 2 Na + Cl-(s ... WebIn chemical compound: Classification of compounds. …and chlorine is called the oxidizing agent (it consumes electrons). The most common reducing agents are metals, for they tend to lose electrons in their reactions with nonmetals. The most common oxidizing agents are halogens—such as fluorine (F 2 ), chlorine (Cl 2 ), and bromine (Br 2 ... how to buy phone on emi online