Methods to compare the strength and weakness of non metallic properties in general What are the acid

The initial specific non-metallic strength can be placed in the periodic table: from top to bottom homogeneity, the non-metallic is weakened; From left to right, the same period, the non-metallic property is enhanced; Weak on the lower left, strong on the upper right; The non-metallic properties of the upper left and lower right diagonals are similar.

Compare the magnitude of electronegativity (specific data should be remembered, so it is slightly more difficult): the greater the electronegativity, the stronger the non-metallic;

Electronegativity is compared with valence: electronegativity is compared as above; For the same element, the higher the valence state, the stronger the non-metallic property.

The acidity of oxygenated acids is comparable when the structure is the same: the more acidic, the stronger the non-metallic nature of the acid-forming elements.

The stronger the non-metallic nature of the element, the electronegativity of the element.

The stronger it is, the stronger its ability to attract electrons.

The structure of its most ** oxide corresponding to the hydrate acid is generally -OH connected to the non-metal atom, and the stronger the non-metallic element due to the strong ability to attract electrons, the OH bond is easier to break, and it is easier to ionize H+ in water, so the more acidic the hydrate corresponding to its most ** oxide.

The strength of acidity depends on the amount of H+ ionized, and sulfuric acid is a binary strong acid, the amount of substance.

When the same is, of course ionized out of H+ than nitric acid.

Many. So sulfuric acid is more acidic than nitric acid.

The acidity describes the strength of the ability of electricity to produce H+, and the h atom in the hydrate corresponding to the most ** oxide generally forms a polar covalent bond with the o atom, and the o atom is bonded with the atom of the element. Taking perchloric acid in the figure as an example, Cl is strong in non-metallicity and has strong electronic ability, o and its shared electron pair is more inclined to cl (compared with atoms of other non-metallic elements such as: c) o The surrounding electron cloud density is reduced, and its electronegativity is weakened, which can also be said to be electronerosis enhanced, so it is easier to attract electrons in H atoms, and the repulsion of H nuclei is hydrogen ions, so it is easier to ionize H ions, and the most ** oxide hydrate is highly acidic.

It's just a rule of thumb, don't pay too much attention to it. The theoretical explanation is roughly as LS says, the stronger the electronegativity, the stronger the ability to attract electrons, and the easier the O-H bond of the corresponding acid to break, the stronger the acidity.

But this explanation is actually insufficient, as you gave the example, nitric acid sulfuric acid is a counter-example. There are also examples, such as selenic acid being a strong acid and periodic acid being a weak acid, which also contradicts this law. In addition, the oxygenated acids corresponding to the most ** oxides of some metals are also very acidic, such as permanganic acid, which is less acidic than sulfuric acid, and much stronger than carbonate silicate phosphoric acid, is the non-metallic property of manganese stronger than that of carbosilicon phosphorus?

As you said in the second half of the sentence, it would be perfect if you applied this rule to the comparison of elements of the same family. Blind promotion is not a no-go.

The acidity of oxygenated acids generally follows the law, the non-metallic nature of the elements is about strong, the stronger the acidity of the oxygenated acid, and the oxidation of oxygenated acids is often irregular, which cannot be used as the basis for judging the strong non-metallic nature of the central element of oxygenated acids.

For example: silicic acid (weak acid), phosphoric acid (medium strong acid), sulfuric acid (strong acid), perchloric acid (strongest acid). The sequential increase in acidity is consistent with the sequential increase in the non-metallic properties of their central elements, silicon, phosphorus, sulfur, and chlorine.

Another example: periodic acid (medium strong acid) perbromine acid (strong acid) perchloric acid (strongest acid) non-metallic refers to the properties of the element, oxidation refers to the elemental element, or the atom of the element, molecules such as: chlorine has strong non-metallic properties, chlorine or chlorine atoms have strong oxidation.

It would be inappropriate to say that chlorine is highly non-metallic.

Judging the strength of non-metallic elements by the oxidation of inorganic oxygenated acids is only a cognitive method at the middle school chemistry stage, which is convenient for qualitative understanding, and strictly speaking, it is neither completely correct nor rigorous enough. Because the oxidation of oxygenated acids is related to a variety of factors, there are many bases for measuring the non-metallic properties of elements that need to be comprehensively analyzed, which are two independent concepts, and there are still many controversies in theory.

A brief analysis of the following points:

First of all, for the elements of variable polyvalent states, a variety of oxygenated acids (such as halogenated hyperhalogenic acids, halogenic acids, haloic acids, hypohalogenic acids, etc.) are formed

There is no obvious rule for the oxidation of oxygenated acids of different valence states of the same element, and the oxidation-reduction electrode potential is only used as a thermodynamic criterion, but there are also kinetic factors that often contradict the two (e.g., hypochlorous acid and perchloric acid).

Secondly, the oxidation of the highest positive valence oxyacids of the same main group elements from top to bottom also shows irregular gradual changes (such as perbromate acid, perchloric acid and periodic acid), and the oxygenated acid properties of acid earth metals in the subgroup are more complex (manganese group, chromium group, etc.).

Thirdly, non-oxygenated acids such as fluorooxygen are extreme exceptions for the same period, and the diagonal rule effect in the periodic table often makes it difficult to compare the non-metallic properties of the elements in this positional relationship (sulfuric acid and nitric acid, phosphoric acid and selenic acid, etc.).

In fact, the non-metallic properties of elements are also measured by ionization energy, electron affinity energy, electronegativity and other quantitative means, in addition to the electrode potential of redox half-reactions, the bond energy of different reaction products, the heat of reaction and other thermodynamic data can also indirectly reflect the non-metallic properties of elements, but these are only from one or several aspects. The manifestation of the non-metallicity of the elements is multi-angled, and the phenomenon of contradiction is universal. (For example, the atomic parameters and corresponding molecular properties of oxygen and chlorine are very inconsistent), it is more appropriate to say that oxidation is only a manifestation of the non-metallic nature of the elements.

In summary, the oxidation of oxygenated acid is not suitable to measure the non-metallic properties of elements, while the gradual change law of acidity and non-metallic properties of elements is in good agreement, and it is suitable to make a qualitative simple explanation in combination with the periodic table.

Think of them all as r o h structures, and of course, there can be multiple ohs.

If R is metallic, that is, the ability to lose electrons is strong, the electrons on the R O bond will be strongly biased towards O, so under the action of water molecules, it is easy to ionize OH-, that is, it is alkaline.

If R is strong in non-metallic, that is, it has a strong ability to obtain electrons, so that the electrons on the R O bond are not biased towards O, so O can only go to H to get electrons, and it is easy to ionize H+, that is, it is highly acidic.

All these statements, in standard chemical terms, are the ion potential, the radius of r is small, the positive charge is high, the ion potential is large, the attraction of r o electrons is large, it is easy to ionize H+, and it is acidic.

1 To put it simply, the stronger the non-metallic property, the greater the attraction ability to electrons, and the easier it is to change from the ** state to the low-valence state, which also oxidizes others and restores itself.

Oh, acidic, electronegativity, the ability to attract electrons, this attraction can affect oxygen, the electron pairs between oxygen and hydrogen are more inclined to oxygen, and the hydrogen connected to oxygen is easier to fall off, and it is highly acidic.

The use of strong acid to prepare weak acid, a is a strong acid, can react with copper at room temperature, a is nitric acid; B is a lumpy solid, after opening the piston of the separating funnel, white precipitate formation can be observed in C, then B is calcium carbonate, C is sodium silicate or potassium silicate, so the answer is: Hno3; caco3；Na2SiO3 (or K2SiO3);

The reaction of nitric acid and calcium carbonate occurs in the flask, and the equation is 2Hno3+CaCO3=Ca(NO3)2+H2O+CO2, so the answer is: 2Hno3+CaCO3=Ca(NO3)2+H2O+CO2;

Carbon dioxide can react with sodium silicate to form silicic acid, and produce sodium carbonate, if carbon dioxide is excessive, sodium bicarbonate can be generated, the chemical equation of the reaction is CO2 + H2O+Na2SiO3 = H2SiO3 + Na2CO3 or 2CO2 + 2H2O+Na2SiO3=H2SiO3 +2NaHCO3, so the answer is: CO2 + H2O+Na2SiO3 = H2SiO3 + Na2CO3 or 2CO2 + 2H2O+Na2SiO3 =h2sio3 +2nahco3；

The stronger the non-metallic nature of the element, the stronger the acidity of the hydrate corresponding to the most ** oxide, and the acidity can be known from the experiment: nitric acid is greater than carbonic acid, and carbonic acid is greater than silicic acid, then the non-metallic nitrogen carbon silicon, so the answer is: nitrogen carbon silicon

Why non-metallic.

The stronger, the most acidic oxide.

The conclusion of your title is actually wrong. Only for alkali metal burial, alkaline earth metal.

Rare earth metals are true, but not for all metals. For example, the active metals AL and ZN, hydrate amphoterinomy; Inactive metals AG, HG, hydrate alkaline.

Since you asked, you can give a passable explanation. The basic nature of hydroxides lies in the ionic bonds between metal ions and OH- under the action of water.

Fracture, OH- frees out into the solution, thus appearing alkaline. The stronger the metallicity, the easier it is for the metal to lose electrons, the more stable the corresponding metal ions, and the weaker the force between the metal ions and oh-, so that the ionic bonds are easier to break, and thus the more alkaline they are.

Analysis: The hydrate of the most ** oxides of the element can be written as r(oh)x

The stronger the acidity, the easier it is to break the hydrogen-oxygen bond in Ro-H, the more stable the Ro bond in Ro-H, the stronger the gravitational attraction of R to the shared electron pairs, and the stronger the non-metallic property.

The stronger the alkalinity, the easier it is to break the RO bond in R-OH, the more stable the OH bond in R-OH, the weaker the gravitational attraction of R to the shared electron pairs, and the stronger the metallicity.

For example, S, its most ** is +6, and oxygen dissolved in water is called hydrate, so S is the most ** oxide corresponding to hydrate.

h2so3。