What does the electronic configuration of potassium look like? In order to answer this question, we consider the structure of the atom, as well as the rules for the distribution of electrons over levels and sublevels.
Quantum mechanics
The electronic configuration of potassium is described by the Schrödinger equation. It binds the potential energy of interaction of the nucleus and electrons, as well as the magnitude of the repulsion between particles having an equal charge. Quantum mechanics uses the postulates of this equation, explaining the presence of a certain energy reserve for each energy level.
Multi-electron atoms
The electronic configuration of potassium is recorded taking into account the Pauli Prohibition principle. Given the peculiarities of the wave nature of electrons, he suggested that each negative particle is located on the "orbital", that is, it has a certain spatial existence. As for the multi-electron atom, to which potassium belongs, no more than two electrons can be located on each orbital. As a result, four quantum numbers were selected that characterize the state of the electron in the considered time period.
Klechkovsky's rule
The electronic configuration of potassium is compiled on the basis of a rule deduced by Klechkovsky. Let's consider it in more detail. Depending on which orbital the electrons are located, they have a certain energy reserve. First comes the distribution of particles with less energy.
The main quantum number corresponding to the period number acts as the main energy characteristic for the electron.
In a multi-electron atom, not only the attraction of electrons to the nucleus occurs, but also their repulsion between themselves. With an increase in the total spin of the particles, the energy of the electron shell decreases, and the number of electrons with the same orientation of their own moments of motion increases. A similar relationship in quantum chemistry is called the Hund rule.
Based on these two rules, the electronic configuration of the potassium atom is compiled. Atomic spectra make it possible to determine the ground state of electrons, that is, to identify those particles that have a minimum energy reserve.
The essence of constructing an electronic formula for a multi-electron potassium atom is quite simple: the electronic system must have minimal energy, comply with the Pauli principle of prohibition.
Examples of electron energy distribution
Before considering what the electronic configuration of the potassium ion is, we give simple examples. In a hydrogen atom, the nucleus contains one positive proton. Around the nucleus, one electron rotates in orbit. In the ground state, the electronic formula of hydrogen has the following form: 1s. Consider the features of the orientation of the spin of this electron. According to the Hund rule, it is aligned with the spin of the nucleus.
For helium, which has a second serial number in the table of elements, two electrons are placed on the same orbital. Each of them has ½ back, has a different direction of rotation.
Elements of the second energy level have two shells, each with its own energy supply.
Potassium is an element of the fourth period of the system of elements; therefore, it has four electronic levels, each of which contains different types of sublevels.
In the normal state, the atom of this alkali metal has the following configuration: 1s22s22p63s23p64s1.
The electronic configuration of the potassium ion is different from the atom. At the external energy level of the metal, there is one valence electron. Since potassium exhibits reducing properties, during interactions with other atoms it gives off a valence electron, turns into a positive ion (cation), which has the following electronic configuration: 1s22s22p63s23p64s0.
Conclusion
For each chemical element located in the periodic table, you can make electronic configurations, armed with the Hund rule, the Pauli prohibition principle, as well as the Klechkovsky formula. In addition to the electronic configurations of atoms in inorganic chemistry are also the formulas of cations and anions formed as a result of chemical interactions.