The extra nuclear electron configuration of the high I chemistry, the electron movement state and th

The electronic layer is divided into k, l, m, n, o, and p layers.

Premise: The K layer can hold up to 2 electrons, the L layer can hold up to 8 electrons, the M layer can hold up to 18 electrons, and the N layer can hold up to 32 electrons.

Then in the electron configuration, the outermost and last shell (you probably don't know the number of electron layers outside the nucleus), which holds up to 8 electrons; The sub-outer shell, which is the penultimate shell, has up to 18 electrons; The penultimate layer holds up to 32 electrons. This condition coexists with the premise above.

For example, when there are five electron shells of k, l, m, n, and o, the o shell can only have a maximum of 8 electrons, and the m and n layers can have a maximum of 18 electrons. However, if there are six electron shells of k, l, m, n, o, and p, there are up to 8 electrons in the p shell, 18 electrons in the o shell, 32 electrons in the n shell, and so on.

For example, al283

The 3 layer is the outermost layer, the 8 layer is the secondary outer layer, and the 2 layer is the penultimate layer.

These 2 sentences are regular, just remember it.

Take a 400-meter runway as an analogy:

The outermost layer is Runway 8.

The second outer layer is Runway 7.

The third floor from the bottom is Runway 6.

The outermost layer is the outermost layer, and the outer layer is the penultimate level.

If you learn the structure, there's no contradiction.

See for yourself.

For example:

There are 7 electrons outside the nucleus of nitrogen (n), and according to the principle of lowest energy and the principle of Paulie's incompatibility, there are first 2 electrons arranged into the 1s orbital of the first shell and 2 electrons arranged in the 2s orbital of the second shell. According to Hunt's rule, the remaining three electrons will be arranged in the same spin pattern into three 2p orbitals with different directions but the same energy. The electronic configuration of the nitrogen atom is 1s22s22p3.

This arrangement of electrons, expressed by quantum numbers n and l, is called electron configuration or electron configuration, and the number in the upper right corner is the number of electrons in the orbital. The magnetic and spin quantum numbers of these electrons can also be compared with the following equation:

The number of electrons in the outermost shell is the number of the main group, and the number of electrons is the number of periods.

Extranuclear electrons are arranged according to three laws:

The principle of lowest energy (electrons are always filled with low-energy orbitals first, followed by high-energy orbitals) Pauli's principle of incompatibility (only two electrons can be accommodated in an orbital, and their spins are opposite) Hunt's rule.

Hunt's first rule (when there is a vacant orbit at the same energy level, electrons will first occupy an empty orbital alone, and when there is no empty orbital, they will be arranged in an orbital with one electron).

Hunt's second rule (the energy will be lower when the orbit is full, half-full, and empty, and the electrons will tend to this arrangement).

n 2 is the "most" number of electrons that can be accommodated.

2. The outer shell refers to all the electronic shells outside the nucleus; The outermost shell refers to the electron shell farthest from the nucleus, or the electron shell with the largest number of electron shells; The subouter shell refers to the second largest atomic shell only closer to the nucleus than the outermost shell.

3. It is numbered from the inside to the outside, the innermost layer closest to the nucleus is the first layer, and the outermost ordinal number increases sequentially, and the outermost layer is the seventh layer.

The maximum number of orbitals that each electron shell may have is n2.

Each orbital can hold up to 2 electrons.

So the total number of electrons that can be accommodated in each electron shell is 2n2.

An introduction to the electron layer.

Also known as the energy layer and electronic shell, it is a group of atomic orbitals with the same principal quantum number n in atomic physics. The electron shell cannot be understood as the movement of electrons in a thin layer of space outside the nucleus, but is divided by the region with the highest probability of electron occurrence and distance from the nucleus.

The electron shell is available n(n....) indicates that n=1 indicates the first electron shell (k layer), n=2 indicates the second electron shell (l layer), and n in turn indicates the third (m layer), fourth (n layer), and fifth (o layer).

Generally, with the increase of n value, i.e., by k, l, m, n, o....The energy of the electrons gradually increases, and the average distance of the electrons from the nucleus increases. The maximum number of electrons that can be accommodated in the electron layer is 2N2.

There are rules according to the different periods.

Extranuclear electron shell.

The law of arrangement is 2*n 2

n is the number of electron layers.

If it's a three-tiered one.

That's 2*9=18

In other words, the third layer has 18 electrons before it reaches the fourth layer. But the KCA

Not so. They are 2

1.The maximum number of electrons held in each electron shell of an atom is 2n2

Niobium Nb: 2, 8, 18, 13 molybdenum Mo:

Palladium PD: uuu: 2, 8, 18, 32, 32, 18, 1

uub:2,8,18,32,32,18,2

uuq:2,8,18,32,32,18,4

Electrons in the nucleus of Huchi.

The state of external movement is quite complex. The state of motion of an electron depends on the electron shell, the electron subplane, the spatial extension direction of the orbit, and the spin state in which it is located. Scientific experiments have also told us that it is impossible to have two electrons in an atom with exactly the same electron shell, electron sublayer, orbital spatial extension direction and spin condition.

This principle is called the Pauli incompatibility principle.

According to this principle, it can be known that only two electrons with opposite spins can be accommodated in each orbital. Based on this, the maximum number of electrons that can be accommodated in each electron layer can be calculated.

2.The law of the arrangement of electrons outside the nucleus.

Extranuclear electron configuration.

Follow Pauli's Incompatible Pants Friend Lee Principle, Energy Lowest Principle, and Hundt's Rule.

The Pauli incompatibility principle has been mentioned above. The principle of lowest energy is that under the premise of not coincidentally violating Pauli's incompatibility principle, the electrons outside the nucleus always occupy the orbital with the lowest energy first, and only when the orbital with the lowest energy is occupied, the electrons enter the orbital with higher energy in turn. That is, to make the system as low energy as possible.

Hunt's rule states that electrons arranged in equivalent orbitals (i.e., orbitals on the same electron shell and electron subplane) will occupy as different orbits as possible and spin in the same direction. Later by quantum mechanics.

It is proved that the electrons are arranged in such a way that the energy may be the lowest, so Hunt's rule can also be included in the principle of lowest energy.

3.The relationship between the metallicity and non-metallicity of an element and the atomic structure.

From a chemical point of view, metal atoms lose electrons and become cations.

Non-metallic atoms easily combine with electrons and become anions.

The ability of an element's atom to gain and lose electrons is obviously closely related to the gravitational attraction of the nucleus to the outer electrons, especially the outermost electrons. The strength of the attraction of the nucleus to the outer electrons is mainly related to the number of nuclear charges of the nucleus.

The atomic radius is related to the electron shell structure of the atom, etc.

Extranuclear electrons are arranged according to three laws:

The principle of lowest energy (electrons are always filled with low-energy orbitals first, followed by high-energy orbitals) Pauli's principle of incompatibility (only two electrons can be accommodated in an orbital, and their spins are opposite) Hunt's rule. Hunt's first rule (when there is a vacant orbit at the same energy level, electrons will first occupy an empty orbital alone, and when there is no empty orbital, they will be arranged in an orbital with one electron).

Hunt's second rule (the energy will be lower when the orbit is full, half-full, and empty, and the electrons will tend to this arrangement).

First of all, we are studying high school chemistry, not junior high school ......

Secondly, in the junior high school range, you are correct when you say that the number of electrons outside the nucleus is not more than 8 in the outermost shell, and in the case of ions is 8 or 2. Why? Because in junior high school, we only talked about the main element, and the main element was like that.

In high school, the parafamily element, that is, the transitional element, is not in line with what junior high school says.

In addition, "we say that the number of electrons outside the nucleus is no more than 8 in the outermost shell" is correct, and this is true for both the main and minor groups. I don't know which book you mean by "in the book".

However, it should be noted that if it is not an "atom", it can be more than 8, just like iron ions.