good oxidizing agent
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Answers:An oxidizing agent causes other things to oxidize or lose electrons. Cl has the greatest electronegativity for electrons and would cause other elements to give them up.
Answers:Atoms, ions, and molecules that have an unusually large affinity for electrons tend to be good oxidizing agents. chemed.chem.purdue.edu/genchem//topicreview/bp/ch19/oxred_3.php - 25k
Answers:B. Cl2 Remember that an oxidizing agent is reduced, it GAINS electrons. Naturally, an element with a HIGH electronegativity, a high tendency for an atom to attract a bonding pair of electrons, would GAIN electrons. Looking at the periodic table, Cl is right next to F, the most electronegative element! Cl has a high electronegativity. Cesium, on the other hand is the most electropositive element, so it would be a reducing agent. Cesium is really v cool. :)
Answers:Standard reduction potential : MnO4 + 8 H+ + 5 e Mn2+ + 4 H2O E = +1.51 V As you can see it is low in the table RTlnKeq = nFE so a +ve E means the equilbrium is favored thermodynamically. If [MnO4]^- is reduced (gain of e-) it must be a strong oxidizing agent (removes e-s). Another way of looking at it: Mn in [MnO4]^- is formally Mn(VII) its maximum oxdn state with no d e-. Its preferred oxidation state in H2O is either Mn(II) d^5 or Mn(III) d^4. But that is thermodynamics and doesn't tell you about the rate of the redox rxn (kinetics). It is found that redox rxns are usually very fast (an e- is pretty small and doesn't let the odd atom get in the way of transfer.) Another factor that I haven't seen is that [MnO4]^- has tetrahedral coordination that probably allows direct contact of the metal center with the species being oxidized. Mn(II) in H2O is [Mn(H2O)6]^2+ that suggests [(Sub)MnO4]^- can readily form (Sub is substrate).