High redox reaction, high chemical redox reaction

1.The number of electrons transferred is 2e-, Oxidant: Copper sulfate Oxidation product: Iron sulfate.

Reducing agent: Iron Reducing product: copper.

2.The number of electrons transferred is 6e-, Oxidant: Chlorine Oxidation product: Nitrogen.

Reducing agent: ammonia Reducing product: ammonium chloride.

3.The number of electrons transferred is 2e-, Oxidant: Hydrogen Peroxide Oxidation Product: Oxygen.

Reducing agent: hydrogen peroxide Reducing product: water.

It should be noted that this is the self-redox reaction of hydrogen peroxide catalyzed by manganese dioxide, and only the valency of oxygen is changing, and the valency of hydrogen is not changing.

4.The number of electrons transferred is 6e-, Oxidizing agent: mercury sulfide and oxygen Oxidation product: sulfur dioxide.

Reducing agent: mercury sulfide Reducing products: mercury and sulfur dioxide.

It should be noted in this question that sulfur in sulfur chemicals is -2 valent.

The equation of the fifth question is not completely put, I remember that I wrote the equation of this question when I was in high school, but I forgot, and I can't make it up, change it correctly, and I didn't write it for you at will.

fe+cuso4==feso4+cu

Fe gives Cu electron 2ge

Reducing agent Oxidant Oxidation product Reducing product.

3cl2+8nh3==6nh4cl+n2

n gives 6 electrons to cl.

Oxidant Reducing agent Reducing product Oxidation product.

2H2O2===Mno2===2H2O+O2O give O electrons 2.

Oxidant Reducing agent Reducing product Oxidation product.

hgs+o2===hg+so2

S gives o electrons 4 pcs.

S gives 2 to hg electrons.

Oxidant Reducing Agent Oxidant Reduction Product Oxidation Product Reduction Product.

nh4no3====n2o+2h2o

n to n electrons 4 pcs.

Oxidant reductant Oxidation product reduction product.

It's tiring! Do you see it?

Oxidation-reduction reaction is a type of reaction in which the oxidation number of an element changes before and after a chemical reaction. The essence of a redox reaction is the gain or loss of electrons or the shift of shared electron pairs.

In the reaction, the substances that undergo oxidation reactions, called reducing agents, produce oxidation products; A substance that undergoes a reduction reaction, called an oxidant, produces a reduction product. Oxidation products are oxidizing but weaker than oxidants; The reducing product is reducing, but weaker than the reducing agent.

Common Oxidants:

1. Potassium permanganate (KMNO4).

Potassium permanganate has strong oxidation, and can oxidize alkyls, aldecordehydes, and aryl groups of primary alcohols, aldehydes, and aromatic ring side chains into acids.

2. Manganese dioxide (mnO2).

Manganese dioxide is a milder oxidizing agent that oxidizes methyl groups in the side chains of aromatic rings to aldehydes.

Knowledge points of chemical redox reaction in high school:

Redox reactions:

1. The essence of redox reaction: there is electron transfer (including the gain, loss or offset of electrons).

2. The characteristics of redox reaction: there is an increase in the valency of elements.

3. The basis of redox reaction: all chemical reactions with the valency of elements rising and falling or the transfer of electrons belong to redox reactions.

Reducing agent (reducible): loss (loss of electrons) liter (increased valency) oxygen (oxidized or oxidation reaction) to generate oxidation products.

Oxidant (with oxidizing properties): obtain (electrons) drop (reduce valency) and also (be reduced or reduce reaction) to generate reducing products.

The law of the strength and weakness of oxidative reduction:

In the same period from left to right, the number of electron layers is the same, the number of nuclear charges of the atom gradually increases, the attraction of the outermost electron of the nucleus gradually increases, and the atomic radius gradually decreases. The electron-obtaining ability gradually increases, the non-metallic property of the element gradually increases, and the oxidation of the corresponding elemental gradually increases. The ability to lose electrons gradually decreases, the metallicity of the element gradually weakens, and the reducibility of the corresponding elemental gradually decreases.

From top to bottom, the number of outermost electrons in the same main group is the same, the number of atomic layers gradually increases, the gravitational force of the nucleus on the outermost electrons gradually decreases, and the atomic radius gradually increases. The ability to obtain electrons gradually weakened, the non-metallic properties of the elements gradually weakened, and the oxidation properties of the corresponding elemental substances gradually weakened. The ability to lose electrons is gradually enhanced, the metallicity of the element is gradually enhanced, and the reduction of the corresponding element is gradually enhanced.

Basic concepts. Redox reaction: any chemical reaction with the valence of elements rising and falling (both a characteristic and a basis for judgment).

The essence of a redox reaction: the gain or loss (or shift) of electrons of an atom or ion.

Oxidation reaction: A reaction in which electrons are lost or the shared electron pair is deviated.

Reduction reaction: A reaction in which an electron is obtained or a pair of electrons is shared. Conceptual Judgment:

1. The essence of redox reaction: there is the transfer of electrons (gain and loss) 2. The characteristics of redox reaction: there is the rise and fall of valency (judging whether it is a redox reaction) 3. The oxidant has oxidation.

Essentially, a redox reaction is the transfer of electrons between atoms of different substances, which is manifested as an increase or decrease in the valency of an element.

1) Iron ions oxidize iodine ions to iodine elementals, and iron ions are reduced to ferrous ions by iodine ions. Depending on the electron transfer, it is the iron ions that transfer 2mol E- to iodine ions instead of iodine elemental matter.

2kmno4+16hcl===2kcl+2mncl2+5cl2↑+8h2o

1.From +7 valent MN to Cl2, 10*E- is obtained, which is reduced and reductive.

2..From -1 valent Cl to +2 valent Mn, 2*5E-, oxidized, oxidized.

In fact, what electrons are depends on the valency. No matter what you do, it will be nice to fall on the valence.

And the transfer of electrons is the transfer of valency multiplied by the previous stoichiometric number. The number of electrons and lost electrons in a reaction is the same. That is, the total number of valence rises and falls is the same.

This place is important, including later trimming, and there are a lot of short answers to the first fill-in-the-blank are to look at it. The key is to find questions to practice, and there may be a big problem at the beginning, so you can't ask your classmates and teachers, and you can feel it yourself and get familiar with it.

There is also the question of centering, the centering reaction and the disproportionation reaction are both redox occurring on the same element.

I'll give you an example:

Centering: H2SO3 2H2S 3S 3H2O, S in sulfurous acid is +4 valence, sulfur in hydrogen sulfide is +2 valence, and the generated S element 0 valence, that is, the same element in the reactant is centering when it approaches a valence state in the middle. Generally there are reactants; Two or more elements of the same element, there is only one spawn.

There is also Fe+2FeCl3 3FeCl2, which is very important.

Disambiguation: It is to turn the elements of one valence, some up, some down, into two. For example, the reaction of sodium peroxide and carbon dioxide with water in the future. And many, many more.

Normalization means that the valency of the same element in the reactant is different, and the valency of the element produced after the reaction is between the two before the reaction.

Liter loss of oxygen: The increase in valency represents the loss of electrons, which is oxidized, and is a reducing agent.

Drop also: Reduced valency means that electrons are obtained, which are reduced, and are oxidants.

The meaning of the centering reaction is that if the elements with the same chemical symbol and different valencies are high and low during the reaction, the valency of the element obtained after the reaction is between high and low, which is called centering. However, there is no reaction between the adjacent valence states of the elements.

For example, if the sulfur ion is -2 valence, it can react with the sulfur in the sulfate (+6 valence), and the valence state of the sulfur formed after the reaction may be 0 or +4 valence. However, sulfite ((SO3)2-, where sulfur is +4 valence and the whole sulfite is -2 valence) and sulfur elemental (0 valence) cannot react because sulfur does not show +1, +2, +3 valence.

In addition, it is necessary to pay attention to the reaction of chlorine gas in the laboratory: KCLO5 + 6HCl = KCL+Cl2 + H2O, only 5 Cl in Cl2 comes from HCl, and the other is from KCL5 (potassium chlorate). The remaining HCl is used as an acid.

This is also typical of the centering reaction. Cl in KCLO5 drops from +5 to 0, and Cl in HCL rises from -1 to 0So the ratio between the oxidant (KCLO5) and the reducing agent (HCl) is 1:

5 instead of 1:6It's easy to get it wrong.

There is also the most important principle of redox reaction, there is a rise and a fall. The sum of the rises and falls must be equal, and the coefficients on both sides of the equation can be balanced according to this principle.

No matter how many reactants there are, as long as the one with an increased valency is a lost electron, add the number of lost electrons of each element, and in the same way add the number of electrons of all the elements with reduced valency, and check whether the two are equal.

As for the centering reaction and disproportionation reaction, it is a redox reaction for the valence change of the same element, the reaction between different valence states, the high falls, the low rises, and moves closer to the intermediate valence state, which is the centering reaction, such as 2H2S + SO2 = 3S + 2H2O, the valence state of sulfur +4 and -2 all change to the middle 0 valence, just pay attention not to stagger it; In the same valence state, some of them increase and some of them decrease, which is a disproportionation reaction, such as the reaction of chlorine and water.

The answer is that AB chlorine will oxidize Nabr and Nai, of course, first oxidizing Nai, and then oxidizing NaB, because BR2 is more oxidizing than I2. During heating, BR2 will volatilize and I2 will sublimate.

If the chlorine gas is introduced in excess, only NaCl, Na2SO4 are left in the solid.

If the amount of chlorine is insufficient, NaCl, Nabr, and Na2SO4 will remain.

A small amount of chlorine will produce NaCl, Nabr, Nai, Na2SO4.

c is wrong because i2 heating sublimates.

In addition, the subject of the building is written incorrectly, it is na2so4, not na2co3.

I wish the landlord progress in learning

AB Chlorine can oxidize Br- and I- to elemental matter, Br can oxidize I- to elemental, after burning, halogen elements cannot still exist, so C should be excluded first, and option D has NAI but no NABR, which is also impossible. So choose AB

The reaction products may be Nabr, Nai, Na2SO3, Cl2, BR2, I2, Na2SO4, NaCl. After evaporation, Cl2 is a gas and will volatilize, and Br2 is a liquid and will evaporate. After burning, NAI will decompose into Na elemental and I2 elemental, I2 will sublimate, and Na will be oxidized by oxygen.

So the last remaining substances are Nabr, Na2SO3, Na2SO4, NaCl.

So AB is correct.

ab The carbonate in the title is sulfate, right? This question tests the sequence of oxidation of oxidants, chlorine can replace I2 and BR2 successively, the former will sublimate when heated, and the latter is volatile, so C cannot have I2, and D will not have only Nai and no NABR

First of all, we know that iodine is volatile, when we learn about the three-state change in junior high school, iodine will sublimate when heated, the solution will be evaporated and burned, even if there is iodine element, it will be sublim......ated

1.I choose N2O

First of all, we know that 2mol of metal loses electrons and 1mol of saltrate sells acid to get the same number of electrons. When the metal is +1, +2, and +3 valence after oxidation, it corresponds to the loss of electrons of 2, 4, and 6mol, respectively, and the electrons obtained by 1mol of nitric acid are 4mol when they are n2o, and the electrons are conserved when the metal is bivalent.

2.According to the analysis of the title, when Na2SO3 is used as a reducing agent, it can only be converted from SO32- to SO42-, each SO32- should lose 2 electrons, 60 SO32- will lose 120 electrons, and for 24 XO(OH)2+ ions, it is exactly 120 electrons, if each XO(OH)2+ Lizhou jujube scatterer should get n electrons in the reaction, then there are: 24N=60 2, and the solution should be n=5

Since the X element shows +5 valence in XO(OH)2+, the final valence state of the X element should be 0 valence when it is reduced by 5 electrons per ion and the 5 valence is lowered. That is, the final valence state of x is 0.

agno3+hg2(no3)2+3hcl===agcl+hg2cl2+3hno3

The chemical formula of mercurous nitrate is Hg2(NO3)2 instead of HgNO3

This is because the chemical bonds in Hg2(NO3)2 are covalent and Hg2(NO3)2 expresses its true structural composition.