The problem of the chemical redox reaction equation in the third year!

It is easy to remember, what oxidant, what reducing agent, in a simple way to say: "Rise and lose oxygen, drop and return, if it is the agent is the opposite." ”

The rise and fall of it refers to the valence.

Explain again: Oxidation reaction occurs when the valency increases.

Reduction is also returned: The reduction reaction occurs when the valency is reduced.

If the agent is the opposite: the substance corresponding to the element with increased valency is the reducing agent, and the substance corresponding to the element with reduced valency is the oxidant.

If you ask, what is the product obtained by the oxidant? What is the product obtained by the reducing agent? It is to ask what is an oxidation product and what is a reduction product.

Oxidation products are substances with increased valency of elements, and vice versa are reduction products.

In this question, Hg is positive 2 valence, and the decrease is 0 valence, so the oxidant is Hgo

o is reduced from negative bivalent to zero valence, so the reducing agent is hgo

The rest of the methods used to give will be rolled out soon.

The answer is: What is a reducing agent (HGO), what is an oxidizing agent (HGO), what is oxidized (HGO), what is reduced (HGO), what is oxidizing (HGO), what is the reducing reaction (HGO), and what is the product obtained by the oxidant? What is the product obtained by the (O2) reducing agent?

hg) What elements in it are oxidized? (o)

When I got to high school, I still have to talk about it. So there's no need to rush.

In the chemical reaction, the reduced valency is the oxidant (itself to oxidize others, itself is beaten to the prototype) The reducing agent with increased valency.

The oxidant is reduced.

The reducing agent is oxidized.

The oxidant is reduced to obtain a reduction product.

The reducing agent is oxidized to obtain oxidation products.

2hgo---2hg+o2

Both oxidizing agents and reducing agents are HGO

Oxidation product O2

Reduction product Hg

It's still very understandable.

Remember, in chemical reactions, it is the oxidant that decreases in valency (it deoxidizes others, and it is beaten to the prototype) and the reducing agent with increased valency.

The oxidant is reduced.

The reducing agent is oxidized.

The oxidant is reduced to obtain a reduction product.

The reducing agent is oxidized to obtain oxidation products.

That's it!

What is a reducing agent, what is an oxidizing agent: hgo

Oxidized Oxidation reaction occurs Oxidation products: 0 elements.

Reduced Reduction reaction occurs Reduction product: Hg element.

Aerobic reactions: "aerobic redox agent, oxygen loss oxidant". By extension, those with increased valency are oxidized as reducing agents, and those with reduced valency are reduced as oxidants.

In this question, HGO is an oxidizing agent and a reducing agent,..

The oxidant is also reduced.

The reducing agent loses oxygen.

Summary. In**yes.

In**yes.

Request**. It does not react under neutral and alkaline conditions.

Because even if the reaction produces iodine element, it will react with the base to form potassium iodide and potassium iodate.

Let's explain the problem.

At the beginning, because it is a neutral environment, so they do not react, there is no phenomenon, after the dropwise addition of Bichai acid is disturbed, iodine Chundan elemental is produced, which makes the starch blue, and finally after adding alkali, the blue color disappears again, and the reaction equation is as follows.

Cu Hno3 (concentrated) = Cu (No3)2 No2 H2O

cu + 4 h+ +2 no3- =cu2+ +2 no2↑ +2 h2o

As can be seen from the second equation (ionic reaction equation), out of 4 molecules NO3- (nitrate-1 valence), there are 2 molecules NO3- that have no electrons to gain or lose (no change in valency) - so they are not written; In addition, N5+ in 2 molecules of NO3- gives 2 electrons that are reduced to N4+ (from NO3- to NO2).

A chemical reaction in which there is a change in the valency of an element during the reaction is called a redox reaction. This reaction can be understood as consisting of two halves, namely oxidation and reduction. The essence of the reaction is that there is a transfer (or shift of electrons) in electrons, which is characterized by the rise and fall of valency.

The half-reaction in which the valency increases, i.e., the electron loss is an oxidation reaction; The reaction in which the valency decreases and the electrons are obtained is a reduction reaction. The substances with increased valency reduce each other, and they are oxidized and ascended, so they are called reducing agents, and their products are called oxidation products; Substances with reduced valency oxidize each other and are reduced themselves, so they are called oxidants, and their products are called reducing products. Namely:

Reducer. Oxidant.

Oxidation products. Generally speaking, the reducing product in the same reaction is weaker than the reducing agent, and the oxidation of the oxidation product is weaker than that of the oxidant, which is the so-called "strong reducing agent to weak reducing agent, strong oxidant to weak oxidant". Summary:

The oxidant undergoes a reduction reaction to obtain electrons, the valency is reduced, it is oxidized, it is reduced, and the reduction product of the chain is generated. The reducing agent undergoes an oxidation reaction, loses electrons, increases the valency, has reducibility, is oxidized, and generates oxidation products. Notation:

Redox is inseparable, and the gain and loss of electrons is fundamental. Those who lose electrons are oxidized, and those who gain electrons are reduced. Reducing agent for those who lose electrons, oxidizing agent for those who gain electrons.

Oxidant. Reducing agents, interdependent and inseparable. Notation 2: Ascend and lose oxygen and return oxygen, and drop and return oxygen to explain:

1.The valency increases, electrons are lost, an oxidation reaction occurs, and it acts as a reducing agent, and the product has less oxidation than the oxidant in the reactant. 2.

The valence of the orange chain is low, the electrons are obtained, the reduction reaction occurs, and acts as an oxidant, and the product has a weaker reducing property than the reducing agent in the reactant. Notation 3: Rise and loss are returned to oxygen and oxygen is returned to oxygen Explanation:

1.The valency increases, electrons are lost, and they are oxidized as reducing agents. 2.

The valency decreases, electrons are obtained, and they are reduced to oxidants. Notation 4: Peel off the camouflage coat (lose electrons), the real face is reduced is the reducing agent, the reducing agent of course oxidation reaction, the electron is negative valence, the loss of electrons is negative, the valency is increased and put on the camouflage coat (to get electrons), the real face is oxidized is the oxidant, the oxidant of course undergoes a reduction reaction, the electrons are negative valence, the electrons are positive and negative, and the valency is reduced.

The reaction of CO, H2 and C to reduce metal oxides, and the displacement reaction are all redox reactions, and the redox reaction is essentially the gain and loss of electrons, that is, the increase and decrease of valence, and it is the reducing agent that can seize O in the reaction.

A reducing agent is a substance that loses electrons (or deviates from electron pairs) and increases the valency of the elements contained in the reaction.

The reducing agent is reductive and is oxidized itself during the reaction.

Substances commonly used as reducing agents are active metal elements such as Al Zn, Fe and C, hydrogen, Co, etc.

Hydrogen, carbon monoxide, carbon dioxide.

Junior Chemistry - Carbon Monoxide Reduction Copper Oxide.