Some are better at losing electrons.

> Here's a typical table of standard reduction potentials. Some are better at gaining electrons. This makes them more reactive.

Oxidizing Agents-are reduced (gain e-) Examples metal ions (M+) non metals acids Not all OA's have the same strength. Permanganate is a good oxidizing agent because it is easily reduced but that hardly seems an answer to me. Oxidizing agents normally exist in their highest possible oxidation states and, therefore, have a strong tendency to gain electrons and undergo reduction. However, today, scientists acknowledge that oxidation can be occur with or without the presence of oxygen. An oxidizing agent is a reactantthat removes electronsfrom other reactants during a redox reaction. F 2 is such a good oxidizing agent that metals, quartz Explanation:Halogens can acts as Strong oxidizing agents because of high electronegativity and high electron affinity which makes them to take electrons very mu… In the presence of a strong electron acceptor (strong oxidizing agent), water serves as a reducing agent. Elemental fluorine, for example, is the strongest common oxidizing agent.

You rank oxidizing agents according to their standard reduction potentials. ... Identify the species oxidized, the species reduced, the oxidizing agent and the reducing agent in the following electron transfer reaction. (stronger) R educi ngA ts-are oxidized (lose e-) Examples metals anions (N-) Not all RA's have the same strength. What makes them "good" oxidizing agents, and whats an example?

Ions, Atoms, and molecules having a strong affinity towards electrons are considered to be good oxidizers. The strength of an oxidizing agent can be estimated by several factors. Previously, the term oxidation was applied to reactions that exclusively involving oxygen. Not every oxidant is hazardous in this manner. In chemistry, an oxidizing agent (oxidant, oxidizer) is a substance that has the ability to oxidize other substances — in other words to accept their electrons.Common oxidizing agents are oxygen, hydrogen peroxide and the halogens..

Typically, compounds with high oxidation states, such as nitrates (NO 3-), permanganates (MNO 4-) and chromates (CrO 4 2-) are good oxidizers.

You are right with Fluorine being the best oxidizing agent and your predictions of lithium being the best reducing agent is also is correct. The stronger the electron affinity, the greater the oxidizing power. As a general rule of thumb, good reducing agents are poor oxidizing agents, and good oxidizing agents are poor reducing agents. It can be seen that magnesium (Mg) reacts with oxygen (O2), and that oxygen is the oxidizing agent because it subtracts electrons from magnesium - that is, it is reducing - and magnesium becomes, in turn, in the reducing agent of this reaction.

For example, potassium dichromate is an oxidant, yet is not considered a dangerous substance in terms of transport. (From wps.prenhall.com) The species at the top left have the greatest "potential" to be reduced, so they are the strongest oxidizing agents.

2Fe3+ + Sn2Fe2+ + Sn2+ species oxidized species reduced oxidizing agent reducing agent As . In one sense, an oxidizing agent is a chemical species that undergoes a chemical reaction in which it gains one or more electrons.

Ozone is a common oxidizing agent. The oxidizing agent typically takes these electrons for itself, thus gaining electrons and being reduced. An oxidizing agent is thus an electron acceptor. An oxidizing agent that can cause or aid combustion is considered a dangerous material.

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