What is a reducing agent, a common reducing agent

In redox reactions, substances that lose electrons

In general, reactants that contain a substance with an elevated valency are reducing agents.

The reducing agent itself is reducible and oxidized, and its products are called oxidation products. The reduction and oxidation reactions are carried out at the same time, that is, the reducing agent is oxidized itself while carrying out the redox reaction with the reduced substance, and becomes an oxidation product.

CommonReducing agentHydrogen (H2), Carbon (C),Carbon monoxide（co）。

Reduction of copper oxide by hydrogen.

Iron oxide (H2+CuO=Cu+H2O; 3h2+fe2o3=2fe+3h2o）；carbon reduction copper oxide (C+2CuO=2Cu+CO2); Carbon monoxide reduces copper oxide and iron oxide (CO+CuO=Cu+CO2; 3co+fe2o3=2fe+3co2）。

Typical reducing agent: Purity.

Active metal elements, such as Na, Al, Zn, Fe, etc. Some non-metallic elements, such as H2, C, Si and other elements (such as C, S, etc.) are in low valency.

When oxides, such as Co, SO2 and other elements (such as Cl, S, etc.) are in low valency, such as HCl, H2S and other elements (such as Fe, S, etc.) are in low valency, such as Na2SO3, FeSO4, etc.

In valency there is an altered redox reaction.

The substance whose valency changes from low to high is called a reducing agent, and envy can be used as an antioxidant.

Reductive.

is oxidized, and its products are called oxidation products.

A reducing agent is a relative concept, as the same substance may exhibit the properties of a reducing agent or an oxidizing agent depending on the reactive substance.

For example, in the reaction of SO2+2HNO3 H2SO4+2H2O+NO2, SO2 is the reducing agent. But in H2S+SO2 S+H2O, SO2 is an oxidizing agent.

The above content reference: Encyclopedia - Reducing Agent.

Organic universal reducing agent.

Lithium aluminium hydride. Sodium borohydride.

Do not restore the double bond).

Reduced nitro group to amino group.

Fe+HCl is commonly used

The reduction of the unsaturated bond is done with Ni+H2

If you just revert the three bonds to the double bonds.

With LinDLAR (PD+

Baso4 + quinoline.

Catalyst hydrogenation which is cis.

To trans with sodium + liquid ammonia.

Inorganic commonly used COC, ZNFE and other active metals, according to the order of metal activity in the first element, can be replaced by the later ions, which is also reduction.

The reductibility of SO2 is also good.

SN4+ ions also have a strong reducing ability.

I won't talk about the repetition upstairs.

Hope you can be satisfied.

Common oxidants are substances that are easily reduced in chemical reactions.

1) Typical non-metallic elements such as F2, O2, Cl2, Br2, I2, S, etc. (their oxidation is basically the same as that of non-metallic activity).

2) ** compounds containing valence elements, such as KMNO4KCLO3

h2so4hno3

MNO2 and others. (3) Metal cations such as: Fe3+, Cu2+, (H+) (in the displacement reaction of metal with acid and salt solution, such as the reaction Fe CuSO4=FeSo4 Cu, in essence, Cu2+ ions oxidize Fe atoms, Cu2+ is used as an oxidant, and Fe is a reducing agent).

A common reducing agent is a substance in which volatile electrons are oxidized in a chemical reaction.

1) Typical metal elements such as: K, Ca,

Na, Mg, etc. (their reducibility is basically the same as that of metal activity) (2) Some non-metallic elements and their compounds such as: H2, C, Co.

3) The lowest valence compounds with valence elements, such as: H2S, Hi, HBR, HC (4) Non-metal anions, such as: S2-, I-, Br-, Cl-

In the redox reaction with changed valency, the substance whose valency changes from low to high is called a reducing agent, which can be used as an anti-stage grinding hail oxidant.

Reducing agent refers to the pure substance of free radicals and reactive oxygen species scavengers, blockers and repair agents.

In redox reactions, substances that lose electrons or have electrons deviated. Reducing agents are also antioxidants, which are reductive and oxidized, and their products are called oxidation products. The reduction and oxidation reactions are carried out at the same time, that is, the reducing agent is oxidized and becomes an oxide while oxidizing the reduced substance.

The dispersion reactants with an elevated valency of a substance contained are reducing agents.

The reducing agent loses electrons and is oxidized into oxidation products, such as the reaction of reducing copper oxide with hydrogen, hydrogen loses electrons and is oxidized into water. The reducing agent exhibits reductiveness in the reaction. The reducing ability is the strength of the reducing agent's electron loss ability, such as the number of electrons lost by sodium atom is less than that of aluminum atom, and the reducing ability of sodium atom is stronger than that of aluminum atom.

Reduction reaction:

Oxidation-reduction reaction (also known as redoxreaction) is a chemical reaction in which the valency of elements before and after the reaction has a corresponding rise and fall change. A chemical reaction pattern in which the valency of an element changes during the reaction is called a redox reaction. This reaction can be understood as consisting of two halves, namely oxidation and reduction.

All such reactions observe conservation of charge. In redox reactions, oxidation and reduction must be carried out in equal quantities at the same time. The two can be likened to the relationship between yin and yang that is interdependent, transformed, ebb and flow, and oppositional to each other. Redox reactions are also present in organic chemistry.

Question 1: What are the common reducing agents in chemistry? Active metal elements: such as Na, Al, Zn, Fe, etc

Reactive metal hydrides: such as lithium aluminum hydride LialH4

Some non-metallic elements: such as H2, C, Si and other elements (such as C, S, etc.).

Alkali metal elements: such as Li, Na, K, etc. Oxides at low valency: such as Co, SO2, H2O2, etc.

Non-metallic hydrides: such as H2S, NH3, HCl, CH4, etc.

Salts at low valency: such as Na2SO3, FeSO4, etc.

stannous chloride SNCL2, oxalate denier H2C2O4, potassium borohydride KBH4, sodium borohydride NaBH4, ethanol mold C2H5OH

Question 2: What are the common oxidants and reducing agents 1 Important oxidants.

In secondary school chemistry, the following important oxidants are generally available:

1) Active non-metallic elements, such as Cl2, Br2, O2, etc.

2) Oxides when elements (e.g., Mn, etc.) are in high valency, such as Mno2, etc.

3) Oxygen-containing acids when elements (such as S, N, etc.) are in high valency, such as concentrated H2SO4, HNO3, etc.

4) Salts when elements (such as Mn, Cl, Fe, etc.) are in high valency, such as KMNO4, KCLO3, FeCl3, etc.

5) Peroxides, such as Na2O2, etc.

2 Important reducing agents.

In secondary school chemistry, the important reducing agents are generally in the following categories:

1) Active metal elements, such as Na, Al, Zn, Fe, etc.

2) Some non-metallic elements, such as H2, C, Si, etc.

3) Oxides when elements (such as C, S, etc.) are in low valency, such as CO, SO2, etc.

4) Acids when elements (such as Cl, S, etc.) are in low valency, such as HCL, H2S, etc.

5) Salts when elements (such as S, Fe, etc.) are in low valency, such as Na2SO3, FeSO4, etc.