OIL RIG so the larger (more positive) the E0, the more likely the compound in the half reaction is to gain resultats concours dgac electrons (be reduced).
Cl2 2e- - 2Cl-.36, cr2O72- 14H 6e- - 2Cr3 7H2O.33, o2 4H 4e- - 2H2O.23, br2 2e- - 2Br-.07, nO3- 4H 3e- - NO 2H2O.96, hg2 2e- -.85, ag e- -.80.
Fe3 e- - Fe2.77, i2 2e- - 2I-.54, cu e- -.52, fe(CN)63- e- - Fe(CN)64-.36, cu2 2e- -.34, cu2 e- -.15, sn4 2e- - Sn2.15 2H 2e- -.00.
In the same way, the compound with the larger reduction potential pulls the electrons over to its side.The reduction potential is the tendency of a compound to be reduced.The E0 values can be looked up in tables, and are always given for reduction halfreactions (reactions gaining electrons).Reaction, eo, f2 2e- - 2F-.87, co3 e- - Co2.80, pbO2 4H SO42- 2e- - PbSO4(s) 2H2O.69, mnO4- 8H 5e- - Mn2 4H2O.49, pbO2 4H 2e- - Pb2 2H2O.46.It makes sense that they occur together if we think about how oxidations lose electrons while reductions gain electrons (remember OIL RIG).Similarly, a compound with a large (positive) reduction potential attracts electrons more strongly than a small (or even a negative) reduction potential.The redox pie: two half reactions make a whole, we just discussed in the last section how a redox reaction is really two reactions that happen together, an oxidation and a reduction.Fe2(aq) 2e- - Fe(s) -0.41, cd2(aq) 2e- - Cd(s) -0.40, ni2(aq) oral concours as ap 2e- - Ni(s) -0.23, sn2(aq) 2e- - Sn(s) -0.14, pb2(aq) 2e- - Pb(s) -0.13, fe3(aq) 3e- - Fe(s) -0.04 2H(aq) 2e- - H2(g).00, sn4(aq) 2e- - Sn2(aq).15.Acidic Solution, eo (V f2(g) 2 e 2 F(aq).87, co3(aq) e, co2(aq).82.But which atoms gain electrons, and which ones lose them?Pb4(aq) 2 e, pb2(aq).8, h2O2(aq) 2 H(aq) 2 e 2 H2O.77, niO2(s) 4 H(aq) 2 e, ni2 (aq) 2 H2O.7.
concours jean louis />
K(aq) e- - K(s) -2.92, ca2(aq) 2e- - Ca(s) -2.76, na(aq) e- - Na(s) -2.71, mg2(aq) 2e- - Mg(s) -2.38, al3(aq) 3e- - Al(s) -1.66 2H2O(l) 2e- - H2(g) 2OH-(aq) -0.83, zn2(aq) 2e- - Zn(s) -0.76, cr3(aq) 3e- - Cr(s) -0.74.Other atoms hold onto their electrons very tightly, and are in fact able to attract nearby electrons into their orbitals.Shouldnt there be such a thing as an "oxidation potential too?Cl2(g) 2 e 2 Cl(aq).358, cr2O72 14 H(aq) 6 e 2 Cr3(aq) 7 H2O.33, n2H5(aq) 3 H(aq) 2 e 2 NH4(aq).24 MnO2(s) 4 H(aq) 2 e Mn2(aq) 2 H2O.23 O2(g) 4 H(aq) 4 e 2 H2O.229 Pt2(aq) 2 e Pt(s).It can tell us which compounds are oxidized or reduced, depending on whether electrons are gained or lost.The reduction potential is experimentally determined for the oxidation and reduction half reactions, and is called.As it turns out, you can tell how likely a compound is to be oxidized from the reduction potential.Thus, in a redox reaction, when two half-reactions are coupled together, the half-reaction (with the higher E0) will be the reduction reaction, while the half-reaction with a smaller (or more negative) E0 will then be forced backwards and act as the oxidation reaction.PbO2(s) SO42(aq) 4 H(aq).A knowledge of the half-reaction reduction potentials can therefore tell you whether compounds are more likely to be oxidized or reduced.
If a compound is less likely to be reduced, it is more likely to be oxidized.
To remember the relationship of E0 and oxidation and reduction, consider the reduction potential as how much a compound wants to get reduced (it has a lot of potential for reduction).
Lets return to the, oIL RIG definition of redox reactions for a moment.