Atomic Structure

Introduction Metallic conduction is commonly caused by moving charged particles that do not become trapped when the material cools. This differs from a semiconductor, where moving charges are present but become stuck or re-join a non-conducting collection when the material cools. Materials whose conductivity increases as they cool are considered metallic, while those whose conductivity […]

The melting point and boiling point are attributes of a compound that define the involvement of the number of electrons from (n-1)d. These points also show the electrons participating in interatomic metallic bonds. When more electrons are added in the metallic lattice, the metallic bonds become stronger. Due to this strong bond, d-block elements have

Ionic radius is the distance from the nucleus of an ion till it has an influence on its electron cloud.When an atom loses or gains electrons it forms ions. Cations are formed when an atom loses an electron and anions are formed when an atom gains an electron.The Ionic radius can be delineated as the

Hund’s Rule Introduction Hund’s rule can be defined as a largest total spin state of an atom which increases the stability of an atom. Hund’s rule is very reliable for determining the phase of a given excited electronic configuration. Friedrich Hund discovered this rule in 1925. Hund’s rule states that: Pairing of electrons in the

General introduction, electronic configuration, occurrence, and features of the phenomenon  META DESCRIPTION: Electrons orbit the nucleus of an atom, while protons and neutrons are enclosed within it.  An atom’s electronic configuration is a numerical depiction of the distribution of electrons in the orbitals of the atom. This dictates an element’s position in the periodic table

We know that every object will have a definite shape and that they gain this shape from the close arrangements of atoms and molecules. When we take crystal lattices into consideration, they arrange their ions in a strict layout, but sometimes one ion may go missing or shift its spot. There are many reasons for

The elements of groups 3-12 are found in the d-block of the periodic table, where the d orbitals are gradually filled throughout each of the four long periods.  The d–block is flanked by the s– and p–blocks in the middle section of the periodic table. Because of their position between s– and p– block elements,

There are six groups of p-block elements altogether as a p-subshell contains three degenerate p-orbitals, each of which can accommodate two electrons. Thanks to their susceptibility to losing an electron, they’re lustrous and typically strong conductors of electricity and heat.  Electronic configuration    The general electronic configuration of group 14 elements is ns2np2. There are

In chemistry, the electronic configuration of atoms is the arrangement of electrons in specific orbitals of an atom or a molecule. The first example of electronic configuration was provided in Bohr’s model of an atom. The electronic configuration involves the placement of different electrons in different shells and subshells of an atom. Though Niel Bohr

The allocation of electrons in an element’s atomic orbitals is described by its electron configuration. Atomic electron configurations follow a paradigm nomenclature in which all electron-containing atomic subshells are arranged in a sequence (with the number of electrons they possess written in superscript). The electron configuration of sodium, for example, is 1s22s22p63s1.The conventional notation, on