Systematics of Anomalies in the Filling of Electron Orbitals of Chemical Elements

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Introduction

It is known that the sequence of filling the electron energy levels and sublevels in many-electron atoms is determined by increasing their energy sequence. The energy of electrons in a many-electron atom, depending on the principal quantum numbers n, which characterizes the energy level (shell), and orbital quantum number l, characterizing the shape of the electron cloud (orbital or sublevel). There are four kinds of forms orbitals s, p, d, f. Orbital orientation in space is characterized by the value of the magnetic quantum number m_l. Pointing to the value of the principal quantum number 1, 2, ..., 7, and type of forms of electronic orbitals, it is possible to record the serial number of the experimental increase in energy orbitals located at different energy levels (Gray, 1965).

1s, 2s, 2p, 3s, 3p, 4s, 3d, 4p, 5s, 4d, 5p, 6s, 4f, 5d, 6p, 7s, 5f, 6d, 7p, 6f, 7d(1)

If to look at the number (1) it can be seen, that the energy of the d - orbital of the previous energy level is more energy of the s - orbital subsequent energy level nd > (n + 1)s (for example, 4d > 5s). Besides the energy of the f - orbitals of the certain energy level is less energy of the d - orbital by increasing the number of the energy level on 2 (for example, 4f < 6d). Consistently filling orbitals at different energy levels, taking into account the capacity of the orbitals (i.e. the presence of each orbital is a certain amount of quantum cells), it is possible in principle to obtain periods, groups and subgroups of the table of chemical elements of Mendeleev (1934). When filling out the orbital electrons it is recommended to use a number (1), as well as the Pauli’s principle (1925) and Hund's rule (1927).

According to the Pauli’s principle (1925) in quantum cell cannot be more than two electrons with opposite spins (spin quantum number m_s equal to ± 1/2 respectively). The atom cannot have two electrons with the same values of the four quantum numbers. The number of possible quantum cells at this sublayer (orbital) is m_l = 2l + 1. The maximum number of electrons in that sublevel equal to 2 m_l. The number of possible quantum cells at any level is equal to n², and the maximum number of electrons at this level is 2n².

According with Hund's rule the filling of the orbitals it is at first by one electron in each quantum cell with the same orientation of the spins, and only after this the quantum cells it are filled with second electrons with opposite spins. Thus, the total spin orbitals must be maximized.

Filling the orbitals on the Pauli principle and Hund's rule corresponds to the ground state of the atom with the lowest energy. When atom reporting additional energy than one or more electrons in the atom move to a higher energy level. In this case, the atom to become excited.

However, for increasing the number of electrons in the atom among of the chemical elements appearing elements in order to fill electron orbitals are the deviations at a number (1) and Hund's rule. It is assumed that these anomalous cases are not significant as a whole for the entire table of chemical elements (Arkel, 1931; Karapet'yants & Drakin, 1994). However, a detailed analysis of the electronic formulas of chemical elements table of D.I. Mendeleev shows that these anomalous elements are many and it is important that in their number reach elements with exceptional properties such as chromium, platinum, gold, silver, uranium, and others. In the light of the opening of all the new elements with many electrons is of interest to 1) organize the anomalies in the filling of the atomic electron orbitals, 2) try to find patterns in these anomaly-filled electron orbitals, and 3) determine the characteristics of the compounds of anomalous elements.