The strength of metallicity is related to temperature, and what is related to the strength of metall

bWhat does the strength of oxidation and reduction depend on?

A: Depends on the standard electrode potential (or bit) in an acidic or alkaline solution at 25 degrees Celsius. The oxidizing type on the left is the oxidizing type, and the oxidized type is from the weakest oxidant at the top to the strongest oxidant at the bottom, and the electron gain or oxidation ability is increased sequentially; On the contrary, the reduction prototype is from the weakest reducing agent to the strongest reducing agent at the top, which is electron loss or reduction ability is enhanced, and then compares the size from positive to negative value from bottom to top against the E* value.

This is a quantitative comparison, if it is only a rough comparison, there is: the principle is that the relative strength of the oxidizing agent and the reducing agent can only be determined by the difficulty of gaining and losing electrons, not the number of electrons gained and lost. (1) Determined by the position of the periodic table, (2) Determined by the order of metal activities, (3) Determined by the order of non-metal activities:

F2>Cl2>O2>Br2>I2>S>N2>P>C>Si>H2, the oxidation is weakened from left to right, and the reducibility is enhanced(4) The same element is determined by the difference in valence states; It is divided into two situations: metal and non-metal: (5) comparison of non-metallic hydride reduction, (6) comparison of oxidation of inorganic oxygenated acids, (7) concentration influence, (8) medium influence, (9) temperature influence, etc. It's not possible to list a lot of these details, sorry.

There is no fixed law for this, just the different properties of certain metals at different temperatures. For example, mercury metal can achieve superconductivity at more than minus 200 degrees Celsius, and so on.

I guess the higher the temperature, the more metallic it is, because it's easier to lose electrons.

Summary. Hello, practice has shown that the properties of metals at low temperatures are different from those at room temperature, and as the temperature decreases or increases, some mechanical properties of the object change.

Effect of low temperature on metal properties.

Hello, practice has shown that the properties of metals at low temperatures are different from those at room temperature, and as the temperature decreases or increases, some mechanical properties of the object change.

Too general, generally speaking, temperature has the greatest impact on the mechanical properties of steel, too low temperature will cause cold brittleness, too high temperature will produce grain creep.

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

1. In the same period, from left to right, with the increase of the number of nuclear charges, the metallicity weakens; In the same main group, from top to bottom, the metallicity increases as the number of nuclear charges increases.

2. According to the strength of the alkalinity of the hydrate of the most ** oxide: the weaker the alkalinity, the stronger the metallicity of its elements.

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

4. The degree of intensity of the 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 temperature.

8. Electrochemical methods.

Metallic Bonds Overview.

A crystal composed of electron cations and free electrons through metallic bonds. Its constituent particles are metal cation free electrons, which are essentially electrical. Its strength is usually inversely correlated with the distance radius of the metal and positively correlated with the density of free electrons inside the metal (which can be roughly seen as positively correlated with the number of electrons around the atom).

1. Generally, with the increase of temperature, the strength of metal materials decreases and the plasticity increases.

2. If the influence of the environmental medium is not considered, it can be considered that the mechanical properties of the material at room temperature and static load have little relationship with the load duration. However, at high temperatures, the load duration has a great influence on the mechanical properties.

3. With the increase of the test temperature, the fracture of the metal transitions from the common transcrystalline fracture at room temperature to the transcrystalline fracture.

A metallic bond is a type of chemical bond that is mainly found in metals. It is formed by a combination of electrostatic attraction between free electrons and metal ions arranged in a lattice. Due to the free motion of electrons, the metallic bond does not have a fixed direction and is therefore a non-polar bond.

Metallic bonds have many properties of metals. For example, the melting and boiling points of general metals increase with the strength of metal bonds. Its strength is usually inversely correlated with the radius of the metal ions, and positively correlated with the density of free electrons inside the metal (which can be roughly seen as positively correlated with the number of electrons around the atom).

An ionic bond refers to the interaction between oppositely charged ions. Ionic bonds belong to chemical bonds, and most salts, alkalis formed from alkali metals or alkaline earth metals, and active metal oxides have ionic bonds. Compounds that contain ionic bonds are called ionic compounds.

Ionic bonds are related to the melting boiling point and hardness of an object.

Covalent bond is a kind of chemical bond, two or more atoms use their outer electrons together, ideally to reach a state of electron saturation, thus forming a relatively stable chemical structure called covalent bond, or covalent bond is the interaction between atoms formed by sharing electron pairs. Its essence is that after the overlapping of atomic orbits, there is a high probability of electrons between two nuclei and the electrical interaction between two nuclei. It should be noted that:

Hydrogen bonds, although there is orbital overlap, are usually not counted as covalent bonds, but rather as intermolecular forces. There is no strict boundary between covalent bonds and ionic bonds, and it is generally believed that when the electronegativity difference between two elements is greater than that, ionic bonds are formed; When it is less than, it becomes a covalent bond.

From a chemical point of view, metal atoms easily lose electrons and become cations, while non-metal atoms easily combine with electrons and become anions. The ability of an element's atom to gain and lose electrons is obviously very closely related to the gravitational pull of the nucleus on the outer electrons, especially the outermost electrons. The strength of the electron attraction of the nucleus to the outer shell is mainly related to the number of nuclear charges, the radius of the atom and the electron shell structure of the atom.

We often use ionization energy to express the difficulty of an atom losing electrons, and the electron affinity energy to express the difficulty of an atom to bond with an electron.

The energy required to remove 1 electron from a gaseous atom in the lowest energy state of an element to become a monovalent gaseous cation is called the first ionization energy of the element, and the energy required to remove another electron from a monovalent gaseous cation is called the second ionization energy, which is usually used in electron volts (EV).

The data of ionization energy show that the ionization energy of the elements of the same main group decreases from top to bottom, i.e., the lower the element, the more likely it is to lose electrons. From left to right for the same period element, the ionization energy increases. Generally speaking, the greater the ionization energy of an element, the weaker its metallicity.

The electron affinity energy of an atom is the energy emitted by a gaseous atom of an element when it acquires one electron to become a monovalent gaseous anion. The greater the electron affinity energy, the easier it is for the atoms of the element to bond with the electrons. Generally speaking, the greater the electron affinity energy of an element, the stronger its non-metallic properties.

The ability of an element's atom to attract electrons to itself in a compound molecule is called the electronegativity of an element. The electronegativity of an element is related to ionization energy and electron affinity. The value of electronegativity can be used as a composite measure of the metallicity or non-metallicity of an element.

The electronegativity of a metal is less, and the less electronegativity a metal is, the more active it is. The electronegativity of a non-metal is greater, and the greater the electronegativity of a non-metal, the stronger its activity.

In the same period, the number of electron layers outside the nucleus of each element is the same, but from left to right, the number of nuclear charges increases in turn, the atomic radius gradually decreases, the ionization energy tends to increase, it becomes more and more difficult to lose electrons, and the ability to obtain electrons gradually increases, so the metallicity gradually weakens and the non-metallicity gradually increases. This gradual change is significant in short periods, but in long periods, the metallicity of the elements weakens slowly from left to right. Because the increased electrons of the transition elements in the long period enter the subouter shell that has not yet been filled, i.e., the d orbital (the lanthanide electrons in the sixth period enter the penultimate third layer, that is, the f orbital), the number of outermost electrons in the atoms of each element in the first half of the long period does not exceed 2, and the metallicity weakens very slowly because the atomic radius and ionization energy of these elements change only slightly in turn.

In the second half of the long period, the number of electrons in the outermost shell of the atoms of each element increases sequentially, so that the weakening of metallicity and the enhancement of non-metallicity become significant.

In each main group, from top to bottom, with the increase of atomic number, although the number of nuclear charges of the atom increases, the number of electron shells of the atom also increases, the radius of the atom also increases, and the shielding effect of the inner electrons also increases. For these reasons, the gravitational pull of the nucleus on the outer electrons weakens, and the atoms lose electrons easily, so the metallicity of the element increases.