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Can someone give 5-10 illustrations of identifying oxidation and reduction species in redox reactions. Can someone give 5-10 illustrations of identifying oxidation and reduction species in redox reactions.
Oxidation - involves the loss of electrons or hydrogen OR gain of oxygen OR increase in oxidation stateReduction - involves the gain of electrons or hydrogen OR loss of oxygen OR decrease in oxidation state 1.H2 + F2 ? 2 HF The overall reaction may be written as two half-reactions: H2 ? 2 H+ + 2 e- (the oxidation reaction) F2 + 2 e- ? 2 F- (the reduction reaction) There is no net change in charge in a redox reaction so the excess electrons in the oxidation reaction must equal the number of electrons consumed by the reduction reaction. The ions combine to form hydrogen fluoride: H2 + F2 ? 2 H+ + 2 F- ? 2 HF 2. 2AgCl(s) + H2(g) ? 2 H+(aq) + 2 Ag(s) + 2 Cl AgCl Ag has a +1 oxidation state Cl has a -1 oxidation state H2 has an oxidation state of zeroH+ has a +1 oxidation state
Oxidation - involves the loss of electrons or hydrogen OR gain of oxygen OR increase in oxidation stateReduction - involves the gain of electrons or hydrogen OR loss of oxygen OR decrease in oxidation state 1.H2 + F2 ? 2 HF
The overall reaction may be written as two half-reactions:
H2 ? 2 H+ + 2 e- (the oxidation reaction)
F2 + 2 e- ? 2 F- (the reduction reaction)
There is no net change in charge in a redox reaction so the excess electrons in the oxidation reaction must equal the number of electrons consumed by the reduction reaction. The ions combine to form hydrogen fluoride:
H2 + F2 ? 2 H+ + 2 F- ? 2 HF
2. 2AgCl(s) + H2(g) ? 2 H+(aq) + 2 Ag(s) + 2 Cl
AgCl
Ag has a +1 oxidation state
Cl has a -1 oxidation state
H2 has an oxidation state of zeroH+ has a +1 oxidation state
3.2Na + Cl2 ------->2NaCl
Na –loss of 2 e-
Cl –gain of 2e-
4.2Na + O2-------->Na2O
Na-loss of 2 e-
O -gain 2 e-
5.2Na + S ------->Na2S
Na-loss of 2e-
S-gain of 2 e-
Thanks & Regard
Aarti Gupta
askiitians Faculty
Zn(s) + CuSO4(aq) ? ZnSO4(aq) + Cu(s)Copperbegins in the +2 oxidation state and is reduced to a neutral state over the course of the reaction. Zinc begins neutral and is oxidized to the +2 state.The oxidation half-reaction is:Zn(s) ? Zn2++ 2e-The reduction half-reaction is:Cu2++ 2e-? Cu(s)Sample 1. equation: 2 H2+ O2? 2 H2OThe sum of oxidation states in the reactants is equal to that in the products: 0 + 0 ? (2)(+1) + (-2)In this equation both H2and O2are free elements and their oxidation states are 0. Theproductis H2O, in which the oxidation state of oxygen is -2 and that of each hydrogen is +1.Sample 2. equation: 2 H2O ? 2 H2+ O2Calculation: (2)(+1) + (-2) = 0 ? 0 + 0In this equation the water is "decomposed" into hydrogen and oxygen, which are both neutral. Similar to the previous example, the H2O has a total oxidation state of 0, with each H taking on a +1 state and the O being -2. Thus, decomposition oxidizes oxygen from -2 to 0 and reduces hydrogen from +1 to 0.Sample 3. equation: Cl2+ 2 NaBr ? 2 NaCl + Br2Calculation: (0) + ((+1) + (-1) = 0) -> ((+1) + (-1) = (0) + 0In this equation Br is replaced with Cl and Cl is reduced, while Br is oxidized.Sample 4. equation: Fe2O3+ 6 HCl ? 2 FeCl3+ 3 H2OExplanation: In this equation Fe and H trade places and O and Cl trade places.Reaction: 2H2O2(aq) ? 2H2O(l) + O2(g)In the reactants H has an O has an O.S. of -1, which changes to -2 for the product, H2O (reduced) and 0 for the product, O2 (oxidized).Thanks & RegardsRinkoo GuptaAskIITians Faculty
Zn(s) + CuSO4(aq) ? ZnSO4(aq) + Cu(s)
Copperbegins in the +2 oxidation state and is reduced to a neutral state over the course of the reaction. Zinc begins neutral and is oxidized to the +2 state.
The oxidation half-reaction is:
Zn(s) ? Zn2++ 2e-
The reduction half-reaction is:
Cu2++ 2e-? Cu(s)
Sample 1. equation: 2 H2+ O2? 2 H2O
The sum of oxidation states in the reactants is equal to that in the products: 0 + 0 ? (2)(+1) + (-2)
In this equation both H2and O2are free elements and their oxidation states are 0. Theproductis H2O, in which the oxidation state of oxygen is -2 and that of each hydrogen is +1.
Sample 2. equation: 2 H2O ? 2 H2+ O2
Calculation: (2)(+1) + (-2) = 0 ? 0 + 0
In this equation the water is "decomposed" into hydrogen and oxygen, which are both neutral. Similar to the previous example, the H2O has a total oxidation state of 0, with each H taking on a +1 state and the O being -2. Thus, decomposition oxidizes oxygen from -2 to 0 and reduces hydrogen from +1 to 0.
Sample 3. equation: Cl2+ 2 NaBr ? 2 NaCl + Br2
Calculation: (0) + ((+1) + (-1) = 0) -> ((+1) + (-1) = (0) + 0
In this equation Br is replaced with Cl and Cl is reduced, while Br is oxidized.Sample 4. equation: Fe2O3+ 6 HCl ? 2 FeCl3+ 3 H2O
Explanation: In this equation Fe and H trade places and O and Cl trade places.
Reaction: 2H2O2(aq) ? 2H2O(l) + O2(g)
In the reactants H has an O has an O.S. of -1, which changes to -2 for the product, H2O (reduced) and 0 for the product, O2 (oxidized).
Thanks & Regards
Rinkoo Gupta
AskIITians Faculty
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