Atomic Structure

Introduction The electron is a negatively charged, low-mass particle. When moving close to other electrons or the positive nucleus of an atom, it may be easily deflected as a result of this effect. The first fundamental particle found was the electron. J.J. Thomson is credited with discovering the electron and its properties through studies conducted […]

Introduction The electronic configuration typically yields especially for components having a comparatively massive atomic number. In such cases, an abbreviated or condensed notation could also be used rather than the electronic configuration. Within the abbreviated notation, the sequence of utterly stuffed subshells that correspond to the electronic configuration of an inert gas is replaced with

What are Electronic Configurations? Electron Configurations is the symbolic representation of  arrangements of the electrons of atoms  in different atomic orbitals.  The arrangement of electrons determines how the atom will react with other atoms, particularly in what kinds of bonds it will form. A simple way to consider this is to view each electron as

The electron configuration is defined in atomic physics and quantum chemistry as the distribution of electrons from an atom or molecule (or other physical structure) into atomic or molecular orbitals of an atom or molecule (or other physical structure).  An orbital diagram is useful in determining the electron structure of an element. The electron configuration

One of the pillars of quantum physics is Heisenberg’s uncertainty principle, although those who have not extensively studied it frequently do not have a thorough understanding of it. Even while it, as its name suggests, defines a certain degree of uncertainty at the most basic levels of nature itself, that uncertainty appears in a very

Iron and nickel are isobars. Iron and nickel have atomic numbers of 26 and 28, respectively. However, they both have the same mass number of 58. Isobars can also be found in argon and calcium, which have different atomic numbers of 18 and 20, respectively. They do, however, have the same atomic mass of 40.

In the transition elements from group 3 to group 6, the atomic and ionic radii of the transition elements drop due to the inadequate shielding provided by the small amount of d-electrons in the transition elements. Those placed between groups 7 and 10 have atomic radii that are roughly similar, whereas those placed between groups

“The orbitals of the atom are filled in the sequence of their increasing energies in the ground state.” As a result, electrons first occupy the lowest energy orbitals available to them before progressing to higher energy orbitals. The (n+l) rule is used to calculate the energy of an orbital. The Aufbau principle, which is based

Solids have a structure that may be compared to that of a three-dimensional piece of wallpaper. A regular repeating design runs from one edge to the other on wallpaper. The repeating pattern in crystals is similar, but it stretches in three dimensions from one edge of the solid to the other. Solids have a structure

In crystalline materials, a Frankel defect is a form of point defect named after its discoverer Yakov Frankel. When an atom or smaller ion (often a cation) departs its lattice position, it creates a vacancy and then becomes an interstitial by settling in a nearby spot. They are generated primarily during particle irradiation in elemental