The terms "reducing agent" and "oxidizing agent" are relative. It seems that you already know this; that depending on the specific reaction, a given compound may be the reducing agent or the oxidizing agent, and in some reactions the same compound is both the oxidizing agent and the reducing agent. It is very important to remember that in an oxidization/reduction reaction, the reducing agent is oxidized and the oxidizing agent is reduced.
Examples: 1) Aldehydes are one example of compounds that can act as reducing agents or oxidizing agents. As reducing agents, aldehydes can reduce Ag(I) in the form of [Ag(NH3)2]+ OH- to Ag metal. They can also reduce Cr(VI) to Cr(III) and Cu(II) to Cu(I). In each case, the aldehyde is oxidized to its corresponding carboxylic acid.
As oxidizing agents, aldehydes (and ketones) can oxidize a hydride (H-) in sodium borohydride or lithium aluminumhydride to H+ as the aldehyde (or ketone) is reduced to an alcohol. Aldehydes and ketones are often used to form carbon-carbon bonds in aldol condensation reactions where a carbanion or an enolate ion attacks the carbonyl carbon of the aldehyde or ketone. In these reactions, the aldehyde or ketone is also reduced to an alcohol.
2) The nitrite anion is another example of a species that can serve as an oxidizing agent or a reducing agent in many reactions. Nitrite (formal charge of N+3) is readily oxidized to nitrate (formal charge of N+5) by the permanganate anion or it can be reduced all the way to ammonia (formal charge of N-3) by hydrogen sulfide. That's an impressive difference of six in the respective nitrogen oxidation states. Like aldehydes and ketones, nitrite can oxidize hydride to H+ in certain borohydride compounds in which nitrite is reduced to N2O, also known as laughing gas.
A series of common examples for red-ox reactions is the reaction of metals with mineral acids. Laboratory experiments such as titration of dichromate ions against oxalic acid are also examples for red-ox reactions.
The compounds which can donate the oxygen as well as can accept the oxygen may act as reducing agents as well as oxidizing agent (depending upon conditions) such compounds include oxides of non metals as SO2, CO, NO etc.
Yes, there are some substances known that can do, but NEVER in the same reaction, with the same reactant that is.
Examples:
(Remember: an oxidant accepts electrons, a reductant donates them)
oxidant: Fe2+ + 2e- --> Fe
reductant: Fe2+ --> Fe3+ + e-
oxidant: Cu+ + e- --> Cu
reductant: Cu+ --> Cu2+ + e-
Even auto redox ouples are known:
At higher temperature CO + CO --> C + CO2
An oxidizing agent is reduced in a chemical reaction by gaining electrons. Some examples are halogens, nitric acid and potassium nitrate.
napthalene powder is reducing or oxidising agenr
because it is gay
So2 , no
because it is both strong oxidising and reducing agent
An oxidizing agent oxidizes the reducing agent, while the reducing agent reduces the oxidizing agent. In simple terms, both processes occur simultaneously. Oxidizing is defined as: the gain of oxygen, loss of hydrogen or loss of electrons. E.g.: C + O2 -> CO2 In this case oxygen would be the oxidizing agent as it supplies oxygen to the carbon. Similarly carbon would be the reducing agent in this case.
it is both oxidizing as well as reducing agent
Sulfuric acid can act as both as an oxidizing agent as well as a reducing agent. It has hydrogen and sulfur which can be reduced, and oxygen which can be oxidized.
When H2O2 serves as an oxidizing agent, the oxygen is reduced to H2O. When H2O2 serves as a reducing agent, the oxygen is oxidized to O2 and bubbles are noticed.
because it is both strong oxidising and reducing agent
An oxidizing agent oxidizes the reducing agent, while the reducing agent reduces the oxidizing agent. In simple terms, both processes occur simultaneously. Oxidizing is defined as: the gain of oxygen, loss of hydrogen or loss of electrons. E.g.: C + O2 -> CO2 In this case oxygen would be the oxidizing agent as it supplies oxygen to the carbon. Similarly carbon would be the reducing agent in this case.
it is both oxidizing as well as reducing agent
Sulfuric acid can act as both as an oxidizing agent as well as a reducing agent. It has hydrogen and sulfur which can be reduced, and oxygen which can be oxidized.
oxygen is the oxidizing agent in both corrosion and combustion
When H2O2 serves as an oxidizing agent, the oxygen is reduced to H2O. When H2O2 serves as a reducing agent, the oxygen is oxidized to O2 and bubbles are noticed.
Yes it can, depending on the acidity of the solution.
No, sucrose is not a reducing agent. The disaccharide sucrose can be 'inverted' breaking the molecule into the monosaccharides glucose and fructose, both of which are reducing sugars. This is commonly done by enzymatic action.
The pure compound is colorless, but older samples tend to acquire a yellow Nitric acid is also commonly used as a strong oxidizing agent.
The Fehling's and the Benedict's Test are the just two of the many tests conducted in identifying reducing and non-reducing sugars. Reducing sugars like the monosaccharides can reduce cupric hydroxide from the reagents used. This is because the reducing sugars have a free oH group at their anomeric carbon that can cause the reduction of mild oxidizing agents like fehling and Benedict solution.In non reducing sugars this oH is involved in glycosidic bond formation.
The term oxidation is named after oxygen, which is the most common oxidizing agent. Oxygen has a strong attraction for electrons, and in most chemical reactions it will take two electrons away from another atom (or from two atoms, such as in the case of the famous water molecule which is composed of one oxygen atom and two hydrogen atoms). So when an atom loses one or more electrons, it is oxidized.
Either one or both of the substances are not magnetic.