Questions about the basis for comparing the strength of metallicity

Yes, so two elements have to react with water, or two elements with the same acid, to compare.

How can it be inaccurate, just because you said that, if metal A can replace the hydrogen in the acid, but not the hydrogen in the water, and the metal B can replace both, then it can show that the metallicity of metal B is stronger than that of A!

The basis for judging the strength of the non-metallic properties of the elements is as follows:1. Judge according to the periodic table.

In the same period, from left to right, the non-metallic property gradually increases; The non-metallic properties of the same main group gradually weaken from top to bottom.

2. Compare the difficulty of elemental elements and hydrogen gas.

The easier it is for non-metallic elements to be combined with H2, the stronger the non-metallic properties.

3. Judge from the stability of hydride formation.

The more stable the hydride, the stronger the non-metallic properties.

Comparative law of non-metallic properties.

1. Judging by the oxidation of the element, in general, the stronger the oxidation, the stronger the corresponding non-metallic.

2. From the perspective of the degree of reaction between elemental matter and acid or water, the more intense the reaction, the stronger the non-metallic property. (For example, the intensity of the reaction of F2, Cl2, Br2 and H2O decreases sequentially, and the non-metals decrease sequentially).

3. It is judged by the stability of the corresponding hydride. The more stable the hydride, the stronger the non-metallic properties.

4. Judging by the difficulty of combining with hydrogen. The easier the chemical reaction, the stronger the non-metallic properties.

Basis for judging the strength of non-metallics:

1. Judging by the oxidation of the element atoms: in general, the stronger the oxidation, the stronger the corresponding non-metallic. (Counter-example: nitrogen atoms are less oxidizing than chlorine atoms).

2. Judging by the degree of reaction between elemental matter and aqueous acid: the more intense the reaction, the stronger the non-metallic.

3. Judging by the stability of the corresponding hydride: the more stable the hydride, the stronger the non-metallic. (Counter-example: methane is more stable than ammonia).

4. Judging by the difficulty of combining with hydrogen: the easier the synthesis, the stronger the non-metallic property. <>

5. Judging by the acidity of the hydrate corresponding to the most ** oxide: the stronger the acidity, the stronger the non-metallic. (Counter-example: nitric acid is weaker acidic than sulfuric acid and perchloric acid, and selenic acid is more acidic than sulfuric acid).

It is worth noting that fluorine has no positive valence, oxygen currently has no highest positive valence, and nitric acid is weaker due to intramolecular hydrogen bonding, so the most acidic oxide corresponding to hydrate is the strongest perchloric acid, not nitrogen oxide fluorine, which is higher than chlorine.

6. Judging by the reducibility of the corresponding anion: the stronger the reducibility, the weaker the corresponding non-metallic. (Counter-example: sulfur ions are more reducible than astatine ions, and hydroxide ions are more reducible than chloride ions).

Metallicity: The property of a metallic gaseous atom that loses its ability to electron;

Metal activity: The property of metal atoms in an aqueous solution that loses their ability to electron.

Note: Metallicity and metal mobility are not the same concept, and the two are sometimes inconsistent, 1In the same period, from left to right, as the number of nuclear charges increases, the metallicity weakens; In the same main group, from top to bottom, with the increase of the number of nuclear charges, the metallicity increases.

2.According to the alkalinity of the hydrate of the most ** oxides; The more alkaline it is, the stronger the metallicity of its elements;

3.According to the order of metal activity (with rare exceptions);

4.the degree of reaction with the acid at room temperature;

5.the intensity of the reaction with water at room temperature;

6.displacement reaction with salt solution;

7.Displacement reaction with metal oxides at high temperatures.

1.Hydrate of the most ** oxides of the element.

Comparison of acidity and alkalinity. The stronger the acidity (alkalinity), the stronger the non-metallic (metallic).

2.The ease with which elemental matter can be combined with H2. The easier it is, the stronger the non-metallic properties.

3.its hydrides.

stability. The more stable it is, the stronger the non-metallic properties.

4.The degree to which the elemental reacts with H20 violently. The more intense the (non)metallic, the stronger.

1. Judging by the difficulty of converting hydrogen from the reaction of elemental matter with water (or acid), the easier it is to replace hydrogen with elemental matter and water (or acid), the stronger the metallicity of the element.

2. Judging by the alkalinity of the hydrate of the most ** oxide, that is, hydroxide. The more alkaline the hydroxide, the stronger the metallicity of the element.

3. It is judged by the order table of metal activity. In order of metal activity, the metallicity of metal elements decreases sequentially.

4. Destruction is judged by the reduction of elementality. Or the stronger the reduction of the element, the stronger the metallicity of the corresponding element.

5. It is judged by the displacement reaction between the element and the compound. Follow the law of forced weakness.

6. Judging by the oxidation strength of metal cations. In general, the weaker the oxidation of metal cations, the stronger the metallicity of the corresponding element. Special case: Trivalent iron is more oxidizing than bivalent copper, but iron is more metallic than copper.

7. Judged by the positive and negative electrodes of the galvanic battery. Generally, in the case of Yu Xiao, the metal electrode with strong activity is used as the negative electrode.