The Shielding Effect and Effective Nuclear Charge: A Comprehensive Explanation скачать в хорошем качестве

The Shielding Effect and Effective Nuclear Charge: A Comprehensive Explanation

Learn about the fundamental concepts of the shielding effect and effective nuclear charge in this detailed video tutorial. Our expert explains the physics behind these concepts and how they impact the behavior of atoms and molecules. Increase your understanding of chemistry and physics with this informative video. Shielding effect is defined as: A decrease in the force of attraction between the nucleus and valance electrons due to incoming and intervening electrons is called the screening effect. Basically, the shielding effect is used to describe the balance between the force of repulsion between inner electrons and the attractive forces between the protons and electrons. So, the force between the protons and electrons is called the effective nuclear charge. So, we can calculate the effective nuclear charge very easily but we should calculate the screening constant before calculating the Zeff. It is also used to explain the removal of electrons from the outermost shell, atomic size & radii of the atom as well as all the periodic properties like ionization energy, electron affinity and, electronegativity. By the following relation “Fnet = Fattraction – Frepulsion“ it is noticed that if there are several electrons in an atom then there are higher repulsive forces between them. Higher repulsive forces mean weakness of attractive forces so there is a decrease in effective nuclear charge. Due to increased repulsive forces in inter electron of an atom, there is a reduction in the nuclear charge because of the shielding effect or screening effect. A reduced nuclear charge is called an effective nuclear charge. Effective nuclear charge is denoted by Zeff. Basically effective nuclear charge is the net charge which is experienced at the outermost electron due to intervening electrons. Ineffective nuclear charge, the term “Effective” refers to the shielding effect of electrons which disallows higher energy orbits electrons to experience full nuclear charge. The shielding effect of inter electrons is called core charge. Effective nuclear charge is measured by the following formula: Zeff = Z – σ In this formula, it is easy to calculate the effective nuclear charge. Z is the atomic number of an atom and σ is the shielding or screening constant “Screening constant is the measure of repulsion between the inter electrons“. Now we are going to discuss a relation between the effective nuclear charge, σ Shielding constant, and interelectronic repulsion.