LE>Oxidation-Reduction Reactions: Redox Redox ReactionsRedox reactions, or oxidation-reduction reactions, have a number of similarities khổng lồ acid-base reactions. Fundamentally, redox reactions are a family of reactions that are concerned with the transfer of electrons between species. Lượt thích acid-base reactions, redox reactions are a matched set -- you don"t have an oxidation reaction without a reduction reaction happening at the same time. Oxidation refers khổng lồ the loss of electrons, while reduction refers to lớn the gain of electrons. Each reaction by itself is called a "half-reaction", simply because we need two (2) half-reactions to form a whole reaction. In notating redox reactions, chemists typically write out the electrons explicitly:Cu (s) ----> Cu2+ + 2 e-This half-reaction says that we have solid copper (with no charge) being oxidized (losing electrons) to khung a copper ion with a plus 2 charge. Notice that, like the stoichiometry notation, we have a "balance" between both sides of the reaction. We have one (1) copper atom on both sides, & the charges balance as well. The symbol "e-" represents a miễn phí electron with a negative charge that can now go out và reduce some other species, such as in the half-reaction:2 Ag+ (aq) + 2 e- ------> 2 Ag (s)Here, two silver ions (silver with a positive charge) are being reduced through the addition of two (2) electrons to size solid silver. The abbreviations "aq" & "s" mean aqueous và solid, respectively. We can now combine the two (2) half-reactions to form a redox equation:We can also discuss the individual components of these reactions as follows. If a chemical causes another substance to be oxidized, we điện thoại tư vấn it the oxidizing agent. In the equation above, Ag+ is the oxidizing agent, because it causes Cu(s) to thảm bại electrons. Oxidants get reduced in the process by a reducing agent. Cu(s) is, naturally, the reducing agent in this case, as it causes Ag+ to gain electrons. As a summary, here are the steps to follow to balance a redox equation in acidic medium (add the starred step in a basic medium):Divide the equation into an oxidation half-reaction and a reduction half-reactionBalance theseBalance the elements other than H & OBalance the O by adding H2OBalance the H by adding H+Balance the charge by adding e-Multiply each half-reaction by an integer such that the number of e- lost in one equals the number gained in the otherCombine the half-reactions và cancel**Add OH- to lớn each side until all H+ is gone và then cancel again**In considering redox reactions, you must have some sense of the oxidation number (ON) of the compound. The oxidation number is defined as the effective charge on an atom in a compound, calculated according to lớn a prescribed phối of rules. An increase in oxidation number corresponds lớn oxidation, and a decrease khổng lồ reduction. The oxidation number of a compound has some analogy to lớn the pH & pK measurements found in acids và bases -- the oxidation number suggests the strength or tendency of the compound to be oxidized or reduced, to serve as an oxidizing agent or reducing agent. The rules are shown below. Go through them in the order given until you have an oxidation number assigned. For atoms in their elemental form, the oxidation number is 0 For ions, the oxidation number is equal to lớn their charge For single hydrogen, the number is usually +1 but in some cases it is -1 For oxygen, the number is usually -2The sum of the oxidation number (ONs) of all the atoms in the molecule or ion is equal khổng lồ its total charge.As a side note, the term "oxidation", with its obvious root from the word "oxygen", assumes that oxygen has an oxidation number of -2. Using this as a benchmark, oxidation numbers were assigned to lớn all other elements. For example, if we look at H2O, and assign the value of -2 to the oxygen atom, the hydrogens must each have an oxidation number of +1 by default, since water is a neutral molecule. As an example, what is the oxidation number of sulfur in sulfur dioxide (SO2)? Given that each oxygen atom has a -2 charge, và knowing that the molecule is neutral, the oxidation number for sulfur must be +4. What about for a sulfate ion (SO4 with a total charge of -2)? Again, the charge of all the oxygen atoms is 4 x -2 = -8. Sulfur must then have an oxidation number of +6, since +6 + (-8) = -2, the total charge on the ion. Since the sulfur in sulfate has a higher oxidation number than in sulfur dioxide, it is said khổng lồ be more highly oxidized. Working with redox reactions is fundamentally a bookkeeping issue. You need to be able to account for all of the electrons as they transfer from one species to lớn another. There are a number of rules and tricks for balancing redox reactions, but basically they all boil down to lớn dealing with each of the two half-reactions individually. Consider for example the reaction of aluminum metal to khung alumina (Al2O3). The unbalanced reaction is as follows:Looking at each half reaction separately:This reaction shows aluminum metal being oxidized to size an aluminum ion with a +3 charge. The half-reaction below shows oxygen being reduced to form two (2) oxygen ions, each with a charge of -2.If we combine those two (2) half-reactions, we must make the number of electrons equal on both sides. The number 12 is a common multiple of three (3) và four (4), so we multiply the aluminum reaction by four (4) & the oxygen reaction by three (3) to lớn get 12 electrons on both sides. Now, simply combine the reactions. Notice that we have 12 electrons on both sides, which cancel out. The final step is to combine the aluminum và oxygen ions on the right side using a cross multiply technique:Taking care of the number of atoms, you should over up with:One of the more useful calculations in redox reactions is the Nernst Equation. This equation allows us lớn calculate the electric potential of a redox reaction in "non-standard" situations. There exist tables of how much voltage, or potential, a reaction is capable of producing or consuming. These tables, known as standard potential tables, are created by measuring potential at "standard" conditions, with a pressure of 1 bar (≅1 atm), a temperature of 298° K (or 25° C, or room temperature) và with a concentration of 1.0 M for each of the products. This standard potential, or E°, can be corrected by a factor that includes the actual temperature of the reaction, the number of moles of electrons being transferred, and the concentrations of the redox reactants and products. The equation is:Perhaps the best way of understanding this equation is through an example. Suppose we have this reaction:Fe(s) + Cd2+(aq) ------> Fe2+(aq) + Cd(s)In this reaction iron (Fe) is being oxidized khổng lồ iron(II) ion, while the cadmium ion (Cd2+) in aqueous solution is being reduced to lớn cadmium solid. The question is: how does this reaction behave in "non-standard" conditions?The first thing lớn answer is how does it behave in standard conditions? We need khổng lồ look at the standard potential for each half-reaction, then combine them to get a net potential for the reaction. The two (2) half-reactions are:Fe2+ (aq) + 2 e- ------> sắt (s), E° = -0.44 VCd2+ (aq) +2 e- ------> Cd (s), E° = -0.40 VNotice that both half-reactions are shown as reductions -- the species gains electrons, & is changed to a new form. But in the complete reaction above, sắt is oxidized, so the half-reaction needs lớn be reversed. Quite simply, the potential for the half-reaction of iron is now 0.44 V. Khổng lồ get the potential for the entire reaction, we showroom up the two (2) half-reactions to lớn get 0.04 V for the standard potential.The question now is: what is the total potential (in volts) for a nonstandard reaction? Suppose again that we have the same reaction, except now we have 0.0100 M Fe2+ instead of the standard 1.0 M. We need to lớn use the Nernst equation to lớn help us calculate that value. If you go to lớn the Redox Half-Reaction Calculator, you should notice that the reaction is selected và the appropriate values are entered into the boxes. Since we don"t have any species "B" or "D", we have entered zero for their concentrations. The concentration of the solid sắt is 1.0 M (actually, concentrations of solids & solvents (liquids) don"t enter into the Nernst equation, but we phối them to 1.0 so that the mathematics works out). If you click on the "Evaluate" button, you should learn that the standard potential is -0.44 V, while the nonstandard potential is -0.5 V. If you scroll down on the calculator, you can enter 0.5 as the first half-reaction. We again change the sign since we"re actually reversing the sắt reactionUsing the calculator again, we calculate the nonstandard potential of the Cd reaction. Suppose we now have a concentration of Cd2+ of 0.005 M, what is its potential? The calculator should return a standard potential of -0.4 V & a nonstandard potential of -0.47 V. Place this value in the box for the second half-reaction, then click on "Evaluate". You should learn that the net nonstandard potential is 0.03 V, slightly less than the value of the net standard potential. Since this value is less than the net standard potential of 0.04 V, there is less of a tendency for this reaction to lớn transfer electrons from reactants khổng lồ products. In other words, less iron will be oxidized và cadmium will be reduced than at standard conditions.Test your use of the redox calculator by calculating the net standard potential for this reaction:2 Ag+ (aq, 0.80 M) + Hg (l)------> 2 Ag (s) + Hg2+ (aq, 0.0010M)Answer: 0.025 V. Since the value is positive, the reaction will work to khung the products indicated. Negative values of the potential indicate that the reaction tends to lớn stay as reactants & not form the products. The net standard potential for this reaction is 0.01 V -- since the nonstandard potential is higher, this reaction will khung products than the standard reaction.Free energy & the standard potential can also be related through the following equation:Where:ΔG = change in không tính tiền energyn = number of molesIf a reaction is spontaneous, it will have a positive Eo, & negative ΔG, and a large K value (where K is the equilibrium constant-this is discussed more in the kinetics section).The energy released in any spontaneous redox reaction can be used khổng lồ perform electrical work using an electrochemical cell (a device where electron transfer is forced khổng lồ take an external pathway instead of going directly between the reactants. Think of the reaction between zinc & copper. Instead of placing a piece of zinc directly into a solution containing copper, we can form a cell where solid pieces of zinc and copper are placed in two different solutions such as sodium nitrate. The two solids are called electrodes. The anode is the electrode where oxidation occurs and mass is lost where as the cathode is the electrode where reduction occurs và mass is gained. The two electrodes are connected by a circuit và the two (2) solutions are connected by a "salt bridge" which allows ions khổng lồ pass through. The anions are the negative ions và they move towards the anode. The cations are the positive ions và they move towards the cathode.The following is a diagram of an electrochemical cell with zinc and copper acting as the electrodes. An external electric current hooked up khổng lồ an electrochemical cell will make the electrons go backwards. This process is called electrolysis. This is used, for example, lớn make something gold plated. You would put the copper in a solution with gold and add a current which causes the gold ions to lớn bond lớn the copper và therefore coating the copper. The time, current, và electrons needed determine how much "coating" occurs. The key khổng lồ solving electolysis problems is learning how to convert between the units.

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Useful information: 1 A=1 C/sec; 96,500 coulombs can produce one (1) mole of e-; the electrons needed is determined by the charge of the ion involvedExample Problem: If you are trying to lớn coat a strip with aluminum và you have acurrent of 10.0 A (amperes) running for one hour, what mass of Al is formed?The solution of this problem involves a lengthly unit conversion process:Practice Redox Problem: balance the following redox reaction in acidic solution:S(s) + NO3-(aq) --> SO2(g) + NO(g)The redox solution is available.Practice Electrolysis Problem: It takes 2.30 min using a current of 2.00 A to lớn plate out all of the silver from 0.250 L of a solution containing Ag+. What was the original concentration of Ag+ in solution?The electrolysis solution is available.
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