Having contrasted many reaction to the standard hydrogen potential, we deserve to now do a table of reduction potentials for every half-reactions, (or oxidation potentials yet we must pick one and stick to it).
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Below is an abbreviated table reflecting several half-reactions and also their connected standard potentials. All "standard potentials" are reduction potentials uneven told otherwise.
Oxidizing Agents: at the top left the the table (where the green arrowhead is pointing) room the substances that are simplest to reduce. A much better statement would certainly be that those substances room ones that "want desperately" to it is in reduced, so lot so that they will "forcefully" withdraw electrons from other varieties so that they deserve to be reduced. This is the very an interpretation of a good oxidizing agent. Fluorine gas is one of the finest oxidizing agents there are and also it is at the height of the table through the best most positive standard potential (+2.87 V).
Reducing Agents: in ~ the various other end, are reactions with an adverse standard potentials. This method that the preferred path the the reaction is actually the reverse reaction. Top top the appropriate side (product side) are substances the "want desperately" to shed their electrons and also undergo an oxidation. This substances (ruled unsurprisingly by the alkali metals) will certainly "force" their unwanted electrons upon various other species. In doing so they come to be the meaning of a powerful reducing agent. Therefore the finest reducing agents are at the bottom of the table on the appropriate side and also have the most an unfavorable standard potentials.
When looking at the table, we should be careful since everything is composed as a reduction. For example, indigenous this table we can find the substance the is simplest to reduce. That is at the the optimal of the table (the F2/2F- oxidation couple). Every the substances on the left room being reduced yet the reactions become less and also less likely as the potential walk from confident to negative. Contrary to this space the substances that are being oxidized. Every the species being oxidized room on the appropriate side of the table (a product). Li(s) is clear the easiest to oxidize due to the fact that it is the extreme situation of this situation.
Look on the LEFT next of the half-reactions for substances that are going to be reduced. Look at on the best side to find substances that are going to be oxidized.
Since Li is simple to oxidize, it is fantastic reducing agent (it reduces something else when it is oxidized). F2 is a an excellent oxidizing certified dealer (it oxidizes something else as soon as it is reduced).
From this table, we can now figure out what reactions will be spontaneous. Because that example, if something is higher in the table (higher typical potential) it will run in the forward direction and the active reactant will certainly be reduced. The reactions that are reduced on the table (more negative standard potentials) will often tend to operation in turning back (right come left) and also the reaction will be one oxidation where the active types on the best (aka: the product) is gift oxidized.
Will Ag+ oxidize Fe? Yes. Just how do we know? The reduction potential for Ag+ is more positive than that for Fe2+. Therefore Ag+ is a strong enough oxidizing agent to oxidization Fe (look because that it on the best side) come Fe2+. On the other hand it could not oxidize chloride ions, Cl-, to chlorine gas, Cl2. Why? because chlorine gas is a more powerful oxidizing agent than silver ion.
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Below is an image of our eBook"s an ext extensive table of conventional reduction potentials. You can discover an also larger data set via the wikipedia link below the image.