Why if it is an ionic ion, that is, subtract or add the number of charges it carries

Maybe you understand that there is a deviation, the reason why ions are called ions is that they are not electrically neutral. The formation of ions should be different for each atom valence electrons, which will lead to the instability of some types of atoms, so each atom tries to stabilize itself, and they will take measures to stabilize themselves, for example: through ionic bonds, the so-called ionic bonds are an atom with fewer valence electrons and an atom with more valence electrons When they collide together, the atom with less valence electrons will throw away their valence electrons, which is essentially an atom with more valence electrons to suck its valence electrons and then the two atoms will be stable. However, an atom with less valence electrons should have lost its valence electrons, although it is stable, it has more positive charge than electrons, so it is not electrically neutral and therefore becomes an ion, and an atom with more valence electrons should have more electrons than a positive charge to become an ion, and then they combine to become ionic compounds through ionic bonds.

Of course, there may be more than two atoms involved in the formation of ions, but they will be stabilized by gaining and losing electrons (on the premise of becoming ionic compounds), as I said above, when the atom with less valence electrons should lose its valence electrons, then it is a cation, he has a part of the positive charge and the electrons neutralized, but there are still some positive charges that cannot be neutralized by the electrons, so the number of electrons should be subtracted from the number of positive charges, and the same is true for adding.

You can follow up.

If it is an anion, the number of charges === the number of protons of this atom + the number of charges it carries.

If it is the number of charges carried by the cation === the number of protons of this atom - the number of charges it carries.

Not equal. If the central atom (ion) is associated with the anion.

Coordination, then the number of charges carried by the ligand ion and the number of charges carried by the central ion are generally not equal. For example, [Fe(scn)6]3-, [CuCl4]2-, etc. Nawei.

Applications

Due to the complexes.

It is electrically neutral, therefore, the total charge of the external ion is equal to the total charge of the ligand ion, and the sign is reversed, so the charge of the ligand ion and the oxidation value of the central atom can be inferred from the charge of the external ion.

For example, in K4[Fe(CN)6], the total charge of the external ions = 4x(+1) =4, so the charge of the matching ion Chang Lipei is -4, and the oxygen rot disturbance value of the central atom iron can be deduced as Fe(II).

An ion is an electrocharged atom or cluster of atoms that conform to the type of sizzle charge and electrical hidden charge that the ion is supposed to denote the ion, such as Na+

cl-etc.; Qinglu Hall.

Therefore, the answer is: na+cl-etc.;

than slag removal, such as: Fe3+ 3+

Concentration (mol l) 1 3

Concentration (mol l) x 3x

From the above circle, it can be seen that the charge number 3 multiplied by the corresponding ion concentration is the concentration of the charge, because the same brigade bend is quietly in the same system, the volume is the same.

Number of charges = number of elements in the periodic table + number of electrons obtained (or minus the number of lost electrons) = number of charged charges. Some elements may have multiple valencies and therefore different charges, depending on the type of compound. The cation is positively charged and loses electrons, and the anion is negatively charged and gets electrons.

The amount of charge is called the "amount of charge". In the International System of Units, the symbol for the amount of charge is q, and the unit is c (coulomb, or "ku"). The discipline that studies the interaction of charged matter is called "electrodynamics" and can be divided into classical electrodynamics and quantum electrodynamics.

If quantum effects can be ignored, classical electrodynamics can quite correctly describe the physical behavior of charged matter in terms of electromagnetism.

At the beginning of the twentieth century, the famous oil drop experiment confirmed that the charge has quantum properties, that is, the charge is made up of a bunch of individual small units called the elementary charge. The local charge in the kitsa is marked with the symbol E and is approximately the amount of charge (electric charge). The exception is quarks, which carry a multiple of e 3.

Protons carry an electric charge e; Electrons carry the amount of charge-e. The academic field that studies charged particles and their interactions between them by photonic media is called quantum electrodynamics.

Electroscopes are often used in laboratories to check whether an object is electrified. When the charged body touches the metal ball of the electroscope, a part of the charge is transferred to the two pieces of metal foil of the electroscope, and the two pieces of metal foil have the same kind of charge and open due to mutual repulsion.

(1) Potassium ferric cyanide ( ) Charge number of central ions: +3 Number of matching ion charges: +1

2) The charge number of the central ion of silver hydroxide ( ) is +1 and the number of the distribution ion is -1

3) Dichloride monochloride. 6 1 Charge number of the central ion of the tetraammonia chromium ( ) : +3 The number of charge of the liganda ion: -1

4) The charge number of the central ion of copper tetraaminohydrate ( ): +2 and the charge number of the matching ion: -2

1. For particles of the same element, the more electrons, the larger the radius. Such as sodium atom "sodium ion", chlorine atom "chloride ion.

2. For the particles of the element in the same period, the anion radius is greater than the cation radius. Such as oxygen ions" lithium ions.

3. The same kind of ions are compared with the atomic radius. Such as sodium ions, magnesium from Xiang Suizi, aluminum ions, fluoride ions, chloride from the digging of the high son, "bromine ions.

4. For ions (single nuclei) with the same electron shell structure, the smaller the number of nuclear charges, the larger the radius. Such as oxygen ions, fluoride ions, sodium ions, magnesium ions, aluminum ions, sulfur ions, chloride ions, potassium ions, calcium ions.

5. The cationic radius of the same element is smaller than the low-valent cation radius and smaller than the atomic radius of the metal. For example, copper ions, cuprous ions, copper atoms, negative divalent sulfur, sulfur atoms, tetravalent sulfur, and hexavalent sulfur.

Factors influencing the size of the ionic radius.

There are three factors that affect the radius of an atom:

1. The number of nuclear charges, the greater the gravitational pull of the nucleus on the electrons outside the nucleus (causing the electrons to shrink to the pronucleus), the smaller the atomic radius; When the number of electron layers is the same, its atomic radius decreases as the number of nuclear charges increases.

2. The number of outermost electrons, the more the number of outermost electrons, the larger the radius.

3. The number of electron shells (the hierarchical arrangement of electrons is related to the size of the space near and far from the nucleus and the mutual exclusion between the electron clouds), the more electron shells, the larger the atomic radius. When the electron shell structure is the same, the larger the number of protons, the smaller the radius.

The above content refers to Encyclopedia - Ionic Radius.