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Theme: Quantum numbers.
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Quantum numbers
The first atomic structure was proposed by E.R. Rutherford and colleagues in 1911, and this theory is called the planetary model of the atom. According to this theory, the positively charged nucleus is the center of the atom. Electrons revolve in orbit around the nucleus, and the size of the atom depends on the size of the electron-moving orbits. The Rutherford model played an important role in the development of atomic theory and helped to understand the results of many experiments. The Danish physicist N.Borr predicts that the electron divides electron energy into quantum (small parts). According to this theory, the electron moves in a certain orbit around a certain distance. It can move along the orbit without separating electron energy. The closest orbit to the nadir corresponds to the "most stable" position of the atom. When an atom is energized, its electron can move to a higher energy level. This condition is called an 'interrupted' state for the electron. The absorption or separation of the atomic energy is only observed when the electron moves from one electron to another.
The modern atomic structure is the basis of quantum theory. The corresponding electron has both a particle and a wave, and its probability of existence in space is explained by modern quantum theory of atomic structure. According to this theory, it is located in a small fraction of the electron space. 90% of the electron availability of space is called atomic orbit. This means that the electron does not rotate the orbit around the nucleus, but is located in the three-dimensional space of the nucleus - the atomic orbit (it is necessary to differentiate orbit from the orbit). When you imagine the atom, you should think of it as a nucleus surrounded by electron clouds. These clouds have different shapes: spherical (sphere) form are called s-orbital, dumbbells are p-orbital, two adjacent dumbbells are d-orbital and three adjacent dumbbells are f-orbital.
In the atom, the orbitals are formed by the energy layers. According to quantum theory, the energy of an electron is known to be small and accurate. The atom contains quantum numbers to describe the energy and movement of an electron, four of them:
1.prime quantum n,
2.number of orbital quantum l,
3.magnetic quantum number m,
4.spin quantum ms. The prime quantum number describes the energy of the n-electron, its distance from the nucleus, that is, the electron-moving layer. The prime quantum can have all integers (n = 1, 2, 3 ...) at once.
As the prime quantum number of the orbitals in which the electrons are located increases, the distance between the electron and the nucleus in the orbit (the orbital radius of the atom) increases, thus reducing the gravitational energy of the electron with the nucleus. The smaller the prime quantum, the greater the electron-binding energy of the electrons, and the higher the n value, the greater the energy of the electron. An electron located close to the quadrant can be converted to a position with higher quantum quantities (atomic excited state) by consuming extra energy from the outside (temperature, electrical discharge, etc.). When the energy is high, the electron goes out of the atom and turns into an ionized state.
The orbital quantum number l represents the form of the atomic orbit. All integers from 0 to n-1 can be [l = 0, 1, 2 ... (n-1)]. When l = 0, the atom has an orbital balloon (s-orbital), if l = 1, the atom takes the form of an orbital dumbbell (p-orbital). When L is higher (2, 3, and 4), we have more complex orbitals (called d, f, g-orbitals).
The maximum number of electrons in the stem is determined by the formula 2 (2 l + 1). At each energy level, they range from one to s. There is only one step in the first step. The second step consists of one s- and three p-orbitals. The third energy phase consists of one s-, three p-, and five d - orbitals. The fourth energy level is made up of one s -bitals, three p-, five d-and seven f -bitals. The number of steps in each energy step is the number of orbitals in formula n2. For example: in the third energy level there are 32 = 9 steps - 1 s-, three p- and five d-orbitals.
The magnetic quantum number ml - determines the position of the atomic orbit against external magnetic or electric fields. The magnetic quantum number changes depending on the number of orbital quantities; its value ranges from + l to l and is equal to 0. Consequently, each value of l corresponds to a magnetic quantum number (2 l + 1). For example:
When l = 1, ml has three values, that is, 1, 0, +1.
When l = 2, the value of ml 5 is +2, +1, 0, -1, -2,
When l = 3, ml 7 represents +3, +2, +1, 0, -1, -2, -3.
The spin quantum can accept only two values of ms and only.
These values correspond to two opposite directions of the electromagnetic moment of the electron. The c-orbital is the first point of any energy step to the core; it consists of a single c-orbit, a p-second stem, it consists of three p-orbitals, a d-third stem that consists of five d-orbitals; The f-th axis is composed of seven f-orbitals.
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