Commonality of non metallic elements ??

The number of electrons in the outermost electron shell of non-metallic elements is 4, except for hydrogen, which has only 1 electron, helium has 2 electrons, and boron has 3 electrons, and the number of electrons in the outermost electron shell of other non-metallic elements is 4, which is the same as the main group ordinal number in which they are located in the periodic table. Non-metallic elements have a small atomic radius and tend to combine foreign electrons to form a stable structure in chemical reactions, so they tend to exhibit oxidation. If its atoms are more likely to bind electrons, the stronger the non-metallic nature of the element, and generally speaking, the stronger the oxidizing ability of its elemental substances, which is a reactive non-metal.

The most reactive of the non-metallic elements is fluorine, followed by oxygen and chlorine.

Typical non-metals tend to achieve a stable structure because of the large number of electrons in the outermost shell of their atoms, so they are often used as oxidants (such as oxygen, chlorine, bromine, fluorine, iodine, etc.) like H2, carbon, silicon, phosphorus and other elemental elements, and their main chemical properties are mainly reducible. Elements such as nitrogen and sulfur are used as oxidants in most reactions, but they can exhibit reducibility when encountering stronger oxidants.

The chemical activity of some non-metallic elements is not consistent with the non-metallic properties of the elements. For example, the non-metallic properties of nitrogen are stronger than carbon, but carbon can react with oxygen under heating conditions, while nitrogen does not react with oxygen under the same conditions, which is quite stable, which is due to the existence of n n bonds in nitrogen molecules, and its bond energy is very large, it is usually difficult to open n n bonds and chemical reactions with other substances, and nitrogen and oxygen will only have chemical reactions under discharge conditions. Therefore, the chemical properties of a non-metallic element are not only related to the atomic structure that composes it but also to its molecular structure or crystal structure.

Non-metallic oxyacids are all covalent compounds, and in the solid state they are molecular crystals. Phosphoric acid and silicic acid are solid at room temperature. Among the above-mentioned oxygenated acids, only silicic acid is insoluble in water, and the rest are soluble in water.

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Let's start with the answer: Non-metallic elements are also metallic. (I don't know if the subject and I are talking about the same metallic nature).

Metallicity refers to the ability to lose electrons and is also known as oxidation. Nonmetallic refers to the ability to get electrons, also known as reduction. Generally speaking, in the periodic period, the non-metallic elements are on the upper right side of the periodic table (with the periodic table attached), and the green ones are the non-metallic elements.

The outermost extra-nuclear electrons are generally stable at 8 (the first extra-nuclear electrons are stable at 2 layers), that is, they are all full (2 8 8 18 18 etc. are full). However, the number of electrons outside the outermost nucleus of most non-metals is greater than 4, such as: halogen F, Cl, Br, I.

There are 7 electrons in the outermost shell and it is easy to get 1 electron, Cl2+H2=2HCl. However, the number of electrons in the outermost shell of h is 1, and it is easy to lose electron-apparent oxidation, that is, metallicity.

Most of the elements (inert elements are not discussed) are metallic and non-metallic, i.e., oxidizing and reducing. It's just that for an element, it's more metallic or non-metallic. The general rule is that the elements in the periodic table gradually increase in non-metals from left to right, and gradually increase in metallicity from right to left.

What is Metallic?

Metallity refers to the ability of an element's atoms to lose electrons in a chemical reaction. The stronger the electron-losing particle, the more metallic the element belongs; Conversely, the weaker it is, the stronger its non-metallic properties are. It can be said that metallic and non-metallic properties are relative concepts and not absolute.

Silicon sits between aluminum and phosphorus in the periodic table and belongs to the transition elements. Although normally, we would think of silicon as a non-metallic element, silicon has a metallic luster, and there are freely movable electrons, so it can be said to have a certain metallicity.

Non-metallic elements get electrons more easily. In general, the number of electrons in the outermost shell of a metal element is relatively small, so the electrons in its outermost shell are easily snatched away, and finally it loses its electrons. The outermost electrons of a non-metallic element have more electrons, so it is easier for it to prey on the electrons of other elements to meet its own needs.

The division of metallic and non-metallic elements is not based on the number of electrons in the outermost shell, but according to the electronegativity of the elements. The ability of an element's atoms to attract electrons is known as the electronegativity of the element. The higher the electronegativity value of the element, the stronger the ability of the Li's atoms to attract electrons in the compound. Conversely, the lower the electronegativity value.

Generally speaking, the electronegativity is greater than the non-metallic elements and the smaller is the metallic element, while the electronegativity of the "metal-likes" (such as germanium, antimony, etc.) located at the boundary of the non-metallic triangle is around, and they have both metallic and non-metallic properties. As for the question of the number of electrons in the outermost shell, it is nothing more than a general law summarized by the periodic table after dividing the metallic and non-metallic elements, and it is not surprising that there are counterexamples, because metals and nonmetals are not originally divided according to this.