Use electron or electron shift to identify what element is oxidized and what ele
ID: 820522 • Letter: U
Question
Use electron or electron shift to identify what element is oxidized and what element is reduced in each reaction. NOTE: "Element" does NOT mean molecule, just the atom, please! For the same reactions, what are the oxidizing agent and what are the reducing agents? (NOTE: Molecules) a. 2 Na(s) + Br2(l) ---> 2 NaBr(s) b. H2(g) + Cl2(g) ---> 2 HCl(g) c. 2 Li(s) + F2(g) ---> 2 NiF(s) d. S(s) + Cl2(g) ---> SCl2(g) e. N2(g) + 2 O2(g) ---> 2 NO2(g) f. Mg(s) + Cu(NO3)2(aq) ---> Mg(NO3)2(aq) + Cu(s)Explanation / Answer
we know that gain of electro is reduction and loss of electron is oxidation. Based on electron effinity of atom the electron of molecule are shifted accordingly.
In Na + Br = NaBr for making bond between Na and Br , Na looses electron thus Na is oxidised while Br is gaining electro so it is reduced. Now Br is responsible for oxidizing Na, so Br is the oxidising agent similarly Na is reducing agent for Br. In case of covalent bonding the atom towards which the electro pair is shifted may be treated as the atom gaining electron and the other atom as atom loosing electro. So in Similar way given above
H+Cl= HCl H oxidised, Cl reduced, Cl oxidising agent, H reducing agent.
Li+F=LiF Li oxidised, F reduced, F oxidising agent, Li reducing agent.
S+Cl2= SCl2 S oxidised, Cl reduced, Cl oxidising agent, S reducing agent.
N2+2O2=2NO2 N oxidised, O reduced, O oxidising agent, N reducing agent.
Mg+Cu(NO3)2=Mg(NO3)2+Cu ====> Consider Cu(NO3)2 in this Cu is +ve while NO3 is -ve , during reaction Mg looses electrons and become +ve charged. These electrons of Mg are gained by Cu to become neutral and +ve charged Mg combines with NO3. Thus in this reaction Cu is reduced and Mg is oxidised. Cu is oxidizing and Mg is reducing agent.
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