Classical Idea of Oxidation and Reduction reactions

The electron was the first fundamental particle to be found, and it was discovered in 1879. J.J. Thomson is credited with the discovery of the electron and its properties, which was accomplished by research carried out in a discharge tube in his laboratory. He asserted that electrons are required elements of all atoms, which he considered to be true. J.J. Thomson conducted experiments in which he used a discharge tube to hold a gas at a low pressure of 0.01mm Hg and measured the results.

Electrons have certain characteristics.

The atom is the smallest unit of measurement in the composition of matter. The atom is made up of a nucleus in the core and one or more electrons orbiting around the nucleus in the outermost part of the structure. The nucleus is made up of protons and neutrons, which are referred to as nucleons collectively. The protons have a mass of 1.00728 amu and the neutrons have a mass of 1.00867 amu. The protons are positively charged particles with a mass of 1.00728 amu and the neutrons are electrically neutral particles with a mass of 1.00867 amu.

Electronic particles having a mass of 0.000549 amu, electrons are negatively charged particles with a charge of . The protons and neutrons weigh approximately 1836 times as much as the electrons do. The number of electrons in an atom of an element is equal to the number of protons in the atom, resulting in a neutral atom. The chemical properties of an element are determined by its electronic arrangements, whereas the stability and radioactive transition of an atom are dictated by the nuclear structure of the element.

Electrons are one of the fundamental particles.

J.J.Thomson conducted experiments in which he used a discharge tube to hold a gas at a low pressure of 0.01mm Hg and measured the results. A discharge tube is a long glass tube with two metal plates that are linked to the battery’s poles that are charged in opposite directions. These metal plates are referred to as cathode and anode, respectively. The use of high voltage results in the ionisation of gas, which is characterised by the ejection of negatively charged particles known as electrons. Cathode rays are responsible for the formation of these particles.

As a result of an atom’s electrical neutrality, it has been predicted by Goldstein that positively charged particles will exist within it. Goldstein’s discovery of protons was based on the electrical neutrality of an atom, which he observed. Cathode ray experiments were used to make the discovery of protons, which was made possible by Goldstein. The anode was determined to be the source of the positively charged ions that were formed as a result of the ejection of electrons. Anode rays and canal rays are the terms used to describe these types of rays. Anode rays, also known as canal rays, are a stream of particles that are positively charged. When hydrogen gas is placed in a discharge tube, it was discovered that the anode rays were nothing more than protons.

Atomic models, which describe the arrangement of fundamental particles in an atom, were developed following the discovery of electrons and protons as subatomic particles contained within the atom.

Electron Configuration

Electron Configuration is a technical term that refers to the configuration of electrons in a molecule.

We can determine the electron configuration by looking at the way electrons are organised around the nucleus in different energy levels or shells. The electrons in an atom occupy the lowest accessible energy levels, which correspond to the shells that are the most inwardly positioned.

The initial level or shell can only contain a maximum of two electrons due to the nature of the structure.

Following this, the energy levels or shells can hold a maximum of 8 electrons in total.

As an example, oxygen is represented by the number 2, while aluminium is represented by the numbers 2, 8, and 3.

Conclusion 

Therefore it can be concluded, The elements are arranged in the periodic table according to the electronic structure of their atoms. Elements belonging to the same group have the same number of electrons in their outermost shell as elements belonging to other groups. As a result, elements belonging to the same group have attributes that are similar. From left to right, over each period, a certain energy level is gradually filled with electrons as they move from left to right. The next energy level is filled in the following time, and so on.