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You rank oxidizing agents according to their standard reduction potentials. > Here's a typical table of standard reduction potentials. (From wps.prenhall.com) The species at the top left have the greatest "potential" to be reduced, so they are the strongest oxidizing agents. The strongest oxidizing agent in the list is "F"_2, followed by "H"_2"O"_2, and so on down to the weakest oxidizing ...
Thus, hydrogen peroxide is the stronger oxidizing agent. Look at the electronegativity values. Oxidation is the removal of electrons from an atom or polyatomic ion. The higher the electronegativity the greater the pull an oxidizing agent has for electrons. The higher the pull for electrons the stronger the oxidizing agent.
A reduction reaction is one in which a reactant in a chemical reaction gains one or more electrons. Reduction reactions always occur in conjunction with oxidation reactions, in which a reactant loses one or more electrons. Reduction-oxidation reactions are often called redox equations. A reduction reaction is only one half of a redox reaction.
The oxidizing agent is "I"_2. A quick technique to use here would be to look at the fact that you're going from iodine, "I"_2, on the reactants' side to the iodide anion, "I"^(-), on the products' side. In this case, you're going from a neutral molecule to a negatively charged ion, so right from the start, you know that iodine is being reduced, i.e. it is taking in electrons. This can only ...
An oxidizing agent is reduced by the oxidized ion. For instance, Pb(s)+H_2O(l)+O_2(g) to Pb(OH)_2(s) + H_2(g) I know, it's not balanced! Pb has an oxidation state of 0, H has one of +2 in water. After the reaction, lead is oxidized to a state of +2, losing electrons, while hydrogen turns into gas, gaining electrons and having a state of 0. So, since Pb is oxidized, H is the oxidizing agent ...
Dichromate is the oxidizing agent.... And ferrous ion is the species that is oxidized.... And we use the method of half-equations..
Reducing agents are the element(s) that are oxidized (oxidation state increases) and oxidizing agents are the element(s) that are reduced oxidation state decreases). You MUST have BOTH for a redox reaction to occur! So, look for the two (or more) elements in an equation whose reaction change requires a CHANGE in their oxidation state. If no change is found, the reaction is not a redox reaction ...
The oxidizing agent is FORMALLY the species that is reduced..... See this old answer for the formal rules of oxidation numbers. We conceive that a species, an atom LOSES electron upon oxidation. And thus for the oxidation of methane..... CH_4(g)+O_2(g) rarr CO_2(g) + 2H_2O(l) We can put in oxidation numbers if we like.....
If we look at, say, the combustion of coal: C(g) + O2(g) → CO2(g) Zerovalent oxygen gas oxidizes zerovalent carbon to give +IV CO−II 2, in which the oxygen has been formally reduced, and the carbon formally oxidized. And of course we can artificially split these reactions up to give separate oxidation/reduction reactions, for instance,
1 Answer. Hydrogen is formally reduced, and is thus the oxidizing agent.. And so .... H 2O(l) + e− → 1 2H 2(g) ↑ ⏐ ⏐⏐ +H O− reduction half equation. And natrium metal is oxidized....i.e. the metal is the REDUCING agent... N a(s) → N a+ + e− oxidation half equation. And we simply add one t'other to remove the electrons....