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Thus, in the reaction, the reductant or reducing agent loses electrons and is oxidized, and the oxidant or oxidizing agent gains electrons and is reduced. The pair of an oxidizing and reducing agent that are involved in a particular reaction is called a redox pair. The reduction potential is a measure of the tendency of the oxidizing agent to be reduced. Its value is zero for H + + e − → ½ H 2 by definition, positive for oxidizing agents stronger than H + (e.g., +2.866 V for F 2) and negative for oxidizing agents that are weaker than H + (e.g., −0.763 V for Zn 2+). The term redox comes from two concepts involved with electron transfer: reduction and oxidation. It can be explained in simple terms: 1  Oxidation is the loss of electrons or an increase in oxidation state by a molecule, atom, or ion. 2  Reduction is the gain of electrons or a decrease in oxidation state by a molecule, atom, or ion. The reduction potential is a measure of the tendency of the oxidizing agent to be reduced. Its value is zero for H + + e − → ½ H 2 by definition, positive for oxidizing agents stronger than H + (e.g., +2.866 V for F 2) and negative for oxidizing agents that are weaker than H + (e.g., −0.763 V for Zn 2+). Oxidizing and Reducing Agents. Oxidation and reduction occur together. If a chemical change results in a more positive oxidation number for an atom (“loss” of electrons), some other atom (or atoms) necessarily acquires a more negative oxidation number (“gain” of electrons). Note the formation of MgCl2, above.  A reducing agent is oxidized because it loses electrons in the redox reaction. Thus reducers are oxidized by oxidizers and oxidizers are reduced by reducers; reducers are by themselves reduced (have more electrons) and oxidizers are by themselves oxidized (have fewer electrons). Since the reducing agent is losing electrons, it is said to have been oxidized. If any chemical is an electron donor (reducing agent), another must be an electron recipient (oxidizing agent). The Ce 4+ ion, which is reduced acts as the oxidizing agent. So oxidation reactions need not involve oxygen. This redox reaction is actually the sum of two separate half-reactions (a reduction half-reaction and an oxidation half-reaction). Another example is hydrogen peroxide, in which the oxygen atom is in the -1 oxidation state. Because this oxidation state lies between the extremes of the more common 0 and -2 oxidation states of oxygen, H 2 O 2 can act as either an oxidizing agent or a reducing agent. weaker oxidizing agent. weaker reducing agent. On the basis of many such experiments, the common oxidation-reduction half-reactions have been organized into a table in which the strongest reducing agents are at one end and the strongest oxidizing agents are at the other, as shown in the table below. Of course, it is oxidized in the process. Since oxidation and reduction are symmetric processes, always occurring together, there is always an oxidizing agent and a reducing agent in the reaction. -2.38. Lithium, having the largest negative value of electrode potential, is the strongest reducing agent. By convention, the standard electrode potentials are reduction potentials, or the tendency to be reduced. Thus, the MnO 4 - ion acts as an oxidizing agent in this reaction. Oxalic acid, on the other hand, is a reducing agent in this reaction. By giving up electrons, it reduces the MnO 4 - ion to Mn 2+ . Atoms, ions, and molecules that have an unusually large affinity for electrons tend to be good oxidizing agents. Elemental fluorine, for example, is the strongest common oxidizing agent. weaker oxidizing agent. weaker reducing agent. On the basis of many such experiments, the common oxidation-reduction half-reactions have been organized into a table in which the strongest reducing agents are at one end and the strongest oxidizing agents are at the other, as shown in the table below. We start by writing a balanced chemical equation for the reaction that occurs in this cell. The table of standard-state reduction potentials suggests that zinc is a better reducing agent than copper and that the Cu 2+ ion is a better oxidizing agent than the Zn 2+ ion. The overall reaction therefore involves the reduction of Cu 2+ ions by zinc metal. 
https://en.wikipedia.org/wiki/Redox https://en.wikipedia.org/wiki/Redox http://web.pdx.edu/%7Elutzr/redox.doc https://en.wikipedia.org/wiki/Reducing_agent http://www.chemistry.wustl.edu/~coursedev/Online%20tutorials/Redox.htm http://chemed.chem.purdue.edu/genchem/topicreview/bp/ch19/oxred_3.php http://hyperphysics.phy-astr.gsu.edu/hbase/chemical/oxred2.html http://chemed.chem.purdue.edu/genchem/topicreview/bp/ch19/oxred_3.php http://chemed.chem.purdue.edu/genchem/topicreview/bp/ch20/electro.php
does a reduction agent become positive