What does FDS mean in the electron configuration outside the element

Indicates the type of atomic orbital.

Your writing looks like it was copied from **. If there is a D layer, such as 3D4S, then you have to fill in 3D first, because the 3D energy is less than 4S. If there is an F layer, such as 4f5d, you need to fill in 4f first, as above.

For details, you can refer to University Chemistry or Inorganic Chemistry at Dalian University of Technology. detailed answers can be found

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The arrangement of electrons in the periphery of an element atom refers to the arrangement of all electrons outside the nucleus of the atom of this element. Valence electrons, on the other hand, refer to the electrons in the outer nucleus that can interact with other atoms to form chemical bonds. For example, the extranuclear electronic configuration of sodium is 1s2

2s2 2p6 3s1.Whereas, the valence electron is only 3s1

1.If you are a junior high school student, you can memorize the periodic table before the 20th CA, if you want to learn chemistry well in high school, it is recommended to memorize the periodic table, which will improve the speed of doing questions and broaden your thinking;

2.Outer electron configuration symbols? I don't know if you are asking at that height and depth, if you ask me why potassium (k) is 2881, then I can tell you that according to the knowledge of the introduction to chemistry in middle school, electrons outside the nucleus are distributed in an electronic shell, the innermost shell, that is, the k layer, can hold up to two electrons, down is the l layer, which can hold up to eight, the m layer can hold up to eight, and the n layer can hold up to 18 ......The electron configuration is sequentially arranged from the k-layer closest to the nucleus; If you ask about the energy level arrangement of the elements of the periodic table, then it is another explanation, for example, oxygen (o) is 2s2 2p4, and its complete arrangement is 1s2, 2s2, 2p4, this is because there are only two electrons in the k layer, all of which are distributed in the s orbital to ensure the lowest energy, that is, to reach the most stable; There are 6 electrons in the l shell, and the s orbital can only hold 2, then the remaining four will go to the p orbital, and the p orbital has three, which can hold up to 6 electrons; If there are more electrons, they continue to be arranged in equal orbitals.

1.You don't need to memorize the periodic table, but it's better to memorize the first 20 elements.

2.Representing the number of electron layers and the distribution of electrons in each layer, each layer from the inside to the outside is k, l, m... It means that the outer shell is filled only when the inner layer is filled, and the innermost shell has two electrons, 8 in the L layer, 8 in the M layer, and 18 in the N layer...

Chemical properties and electron transfer are most closely related to the number of electrons in the outermost shell. Each electron layer is divided into s, p, d, f... A sublayer, which represents the quantum number change of an atom.

s one track, p three, d5... Each sublayer orbital has a maximum of two electrons with opposite spins, and when it is insufficient, it is preferentially to fill up the orbitals--- and the last sublayer or something is studied at the time of college.

3.The outermost shell has one electron, possibly +1 valence, and one electron, -1 valence. For example, H and F can form a substance, so that the chemical valence is generally 0 to ensure external neutrality.

For example, Ca has two electrons in the outermost shell, and Cl lacks one electron in the outermost shell, so CaCl2 is formed, and two Cl and one Ca ensure electrical neutrality.

The symbols representing the electron layer, the symbols of the first to seventh layers of the electron layer from the inside to the outside are klmnopq, high school chemistry elective 3 and inorganic chemistry or general chemistry at university.

What letters. klmn？Represents the number of electron layers 1234

3 The arrangement of electrons outside the nucleus.

1) The principle of lowest energy.

A general law of nature is that the lower the energy, the more stable it is, and the electrons outside the nucleus always occupy the atomic orbital with the lowest energy first, and only when the orbital of the atom with lower energy is full, the electrons enter the orbital with higher energy in turn, so that the atom is in a stable state with the lowest energy. Such a state is the ground state of an atom.

The energy level of the atomic orbital (also known as the energy level) is mainly determined by the principal quantum number n and the angular quantum number l, and the order of electron filling outside the nucleus can be seen from the approximate energy level diagram of the atomic orbital.

2) Pauli incompatibility principle.

No two electrons in the same atom have exactly the same four quantum numbers, or no electrons in the same atom that are in exactly the same state of motion. According to this principle, the maximum number of electrons that can be accommodated in each electron shell can be deduced:

The principal quantum number n (electron shell symbol).

The orbital of an atom determined by the angular quantum number l.

The number of spatial orientations of atomic orbits determined by the magnetic quantum number m.

The maximum number of electrons can be accommodated in each electron layer.

The relationship between the maximum number of electrons in each electron layer and the number of electron layers.

3) Hunt's rule.

In orbitals with equal energy, electrons occupy as many different orbits as possible and spin in the same direction, which is called Hunt's rule. The Hundt rule is actually a complement to the principle of lowest energy. Because when two electrons occupy one orbital, the repulsion between the electrons will increase the energy of the system, and only the equivalence of the orbital can help reduce the energy of the system.

As a special case of Hunt's rule, the equivalence orbital is fully filled, half-filled, or fully empty.

With the increase of atomic number, the extranuclear electron configuration becomes complex, and the principle of extranuclear electron configuration cannot satisfactorily explain the facts of some experiments, such as the first.

Paragroup elements of the fifth, sixth, and seventh cycles. For the atomic electron configuration of a specific element, the results of spectroscopic experiments shall prevail.

1. The first layer can be arranged up to 2, the second layer can be arranged at most 8, the outermost layer can not exceed 8, and 2. Each layer can be arranged at most 2n squares.