What is the strongest and weakest oxidizing agent?
The strongest oxidizing agent in the list is F2, followed by H2O2, and so on down to the weakest oxidizing agent, Li+.
Strong oxidizing agents are typically compounds with elements in high oxidation states or with high electronegativity, which gain electrons in the redox reaction (Figure 1). Examples of strong oxidizers include hydrogen peroxide, permanganate, and osmium tetroxide.
<br> R: Fluorine is the strongest oxidising agent in the periodic table. A: Lithium is the strongest reducing agent in the periodic table.
Examples of oxidizing agents include halogens, potassium nitrate, and nitric acid. A reducing agent, or reductant, loses electrons and is oxidized in a chemical reaction.
The most common oxidizing agents are halogens—such as fluorine (F2), chlorine (Cl2), and bromine (Br2)—and certain oxy anions, such as the permanganate…
Fluorine, having the largest positive value of electrode potential, is the strongest oxidizing agent.
In order to find the oxidizing agent in a chemical reaction, we need to look at the compound's oxidation state at the beginning and end of the reaction. The compound that ends with a lower oxidation state than it had in the beginning is the oxidizing agent.
Lithium is the strongest reducing agent because of lower reduction potential (i.e it has lower tendency to acquire electrons.)
Li+ is the weakest oxidizing agent as it has most negative standard reduction potential.
Sodium, hydrogen, and lithium are examples of strong oxidizing agents. While weak reducing agents cannot lose electrons easily. Fluorine, chlorine, iron etc. are weak reducing agents.
Which substance is the weakest oxidizing agent?
The weakest oxidizing agent does not have an affinity towards the electron and therefore they do not oxidize the other molecules easily. The weakest oxidizing agent is as follows: Pyridinium chlorochromate ( PCC ) , ( COCl ) 2 , etc. The oxidizing agents are used for the purification of water, bleaching agent, etc.
Higher the electronegativity greater the pull of electrons and hence the stronger the oxidizing agent. Example: The strongest elemental oxidizing agent is fluorine.
The most common oxidizing agents are halogens—such as fluorine (F2), chlorine (Cl2), and bromine (Br2)—and certain oxy anions, such as the permanganate…
Fluorine is the most electronegative of all the elements of the periodic table, and hence it has the ultimate oxidation power.
So, as MnO4− has maximum oxidation state of Mn, it is the strongest oxidizing agent and the order of increasing strength as an oxidizing agent is as follows: Mn2+<MnO2<MnO4−