From the periodic law, isn t C more reducible than Si?

For elements of the same main group, from top to bottom, the metallicity is enhanced, and the reduction is enhanced. Si is below C, so Si is more reducible than C. For the reaction 2C + SiO2 = high temperature = Si + 2Co, it should be interpreted as follows:

At high temperatures, C is more reducible than Si. Therefore, in general, Si is more reducible than C; At high temperatures, C is more reducible than Si. SI is highly reducible.

In the same group, the reduction is strong and the oxidation is weak. Theoretical analysis: the outermost number of electrons of the same group of elements is the same.

The larger the period, the greater the number of electron layers, the larger the atomic radius, the weaker the gravitational pull of the nucleus on the outermost electron, and the easier it is to lose the outermost electron. Electrons are lost, valency increases, oxidized, and reducible.

Answer: The periodic law refers to the law that the properties of elements change periodically with the increase of the atomic number of the element (that is, the number of electrons outside the nucleus or the number of nuclear charges). The discovery of the periodic law is an important milestone in the process of chemical systematization.

Combined with the periodic table, the periodic law can be expressed as: the properties of an element change periodically with the increasing number of atomic numbers.

The contents of the periodic law:

1. The law of atomic radius:

In the same period (except for noble gases), from left to right, as the atomic number increases, the radius of the atom of the element decreases;

In the same family, from top to bottom, the atomic radius of an element increases as the atomic number increases.

In general, it is said as: bottom left and top right.

In general, the same element:

a.The cationic radius is atomic radius;

b.Anion Radius》Atomic Radius;

c.Anion Radius》Cation Radius;

2. The law of change of valence:

In the same period, from left to right, as the atomic number increases, the highest positive valence of the element increases (from +1 valence to +7 valence), except for the first period, except for the elements o and f in the second period;

The first cycle of the lowest negative valence increase (from 4 valence to 1 valence) is excluded, and since metal elements generally have no negative valence, they start from the A group.

The sum of the absolute value of the most ** element and the absolute value of the lowest price is 8, and the algebraic sum is one of the even numbers of 0, 2, 4, 6 (only for non-metals except o and f).

3. The law of metallicity, oxidation, reduction and stability

In the same period, from left to right, as the atomic number increases, the metallicity of the element decreases and the non-metallicity increases;

a.The stronger the elemental oxidation, the weaker the reducibility, the weaker the reducibility corresponding to the simple anion, and the stronger the oxidation of the simple cation.

b.The easier it is to react with hydrogen, the more intense the reaction, and the more stable its hydride is.

c.The most ** oxide corresponds to the hydrate (oxygenated acid) the more acidic.

In the same family, from top to bottom, with the increase of atomic number, the metallicity of the element increases, and the non-metallicity decreases;

a.The stronger the elemental reducibility, the weaker the oxidation, the stronger the reducibility corresponding to simple anions, and the weaker the oxidation of simple cations.

b.The easier it is to react with water or acid, the more intense the reaction, and the less likely it is to react with hydrogen;

c.The most ** oxide corresponds to the hydrate (hydroxide), the more alkaline it is.

4. There are also some basis for judging the metallicity and non-metallicity of elements, which can be used as a supplement to the periodic law

In order to achieve a steady state, different atoms choose different ways. Among the elements of the same period, the more "empty" the orbital, the more likely it is to lose electrons, and the more "full" the orbital, the easier it is to gain electrons. With the gradual change from empty to full orbital from left to right, the elements also gradually change from predominantly metallic to predominantly non-metallic.

With the same group of elements, because the higher the period, the more electron layers, the larger the atomic radius, the attraction to the electrons outside the nucleus is weakened, and the easier it is to lose, so the elements ranked below are generally more metallic than the elements above.

Carbon and silicon are non-metallic elements, and only oxidation is considered, and reducibility is considered for metals.

For elements of the same main group, from top to bottom, the metallicity is enhanced, and the reduction is enhanced. Si is below C, so Si is more reducible than C.

For the reaction 2C + SiO2 = high temperature = Si + 2Co, the suspicion should be explained as follows: At high temperatures, C is more reducible than Si.

Therefore, in the general situation, the reduction of Si is stronger than that of C; At high temperatures, C is more reducible than Si.

According to the periodic law, the oxidation of the same main group is weaker and the reduction is stronger the lower the element. According to this law, Si is more reducible than C.

It's hard to say, it depends on the conditions.

In the order of the periodic table, C is above Si, and the non-metallic property of C is stronger than that of Si, that is, the oxidation of C is stronger than that of Si, and the reduction of Si is stronger than that of C.

But in industrial production, 2C + SiO2 = High temperature = Si + 2Co is C to reduce Si out, and in this reaction, C is the reducing agent.

Silicon is highly reducible! Carbon can also have a negative price, but silicon cannot.

According to the analysis, it can be seen that: A is oxygen, B is sodium, C is aluminum, D is phosphorus, 1) elemental A is oxygen, which belongs to molecular crystals, elemental B is sodium, belongs to metal crystals, and elemental C is Al, which belongs to metal crystals, so the answer is: molecule; Metal; Metal;

2) Phosphorus elemental celery has white phosphorus, red phosphorus, etc., among which elemental white phosphorus can be dissolved in carbon disulfide and belongs to molecular crystals, so the answer is: molecule; White phosphorus;

3) O and Na ignite to form sodium peroxide, which belongs to the first ion crystal, so the answer is: Na2O2 ion

The product of the reaction of element A with water vapor is the main component of water gas, 1 molb element element reacts with water to produce gas F, 1 molc element element reacts with water to produce gas E, E and F are combined with each other to form water, and element D element reacts with water to form two acids. (1) The ionic equation for the reaction of C element with water is 2Na+2H2O=2NaOH+H2 2)The crystalline particles of the compound formed by C and D are combined by ionic bonds, and there are 8 C particles with an equal distance and the nearest C particle around a D particle. A and D are compounds whose crystals are bonded by covalent bonds between the particles.

3) The most acidic of the four elements, the most acidic oxide hydrate is HCO4 acid filling chemical formula).

The atomic numbers of DA, B, C, and D increase and the atomic radius decreases in turn, indicating that these four elements are the same periodic elements.