Скачать с ютуб Valence Shell Electron Pair Repulsion (VSEPR) Theory || for Class 11 in HINDI в хорошем качестве

Valence Shell Electron Pair Repulsion (VSEPR) Theory || for Class 11 in HINDI

In this Chemistry video in Hindi for class 11 we explained Velance Shell Electron Pair Repulsion theory, popularly known as VSEPR theory. Lewis concept is unable to explain the shapes of molecules. VSEPR theory provides a simple procedure to predict the shapes of covalent molecules. Sidgwick and Powell in 1940, proposed a simple theory based on the repulsive interactions of the electron pairs in the valence shell of the atoms. It was further developed and redefined by Nyholm and Gillespie in 1957. The main postulates of VSEPR theory are as follows: • The shape of a molecule depends upon the number of valence shell electron pairs (bonded or nonbonded) around the central atom. • Pairs of electrons in the valence shell repel one another since their electron clouds are negatively charged. • These pairs of electrons tend to occupy such positions in space that minimise repulsion and thus maximise distance between them. • The valence shell is taken as a sphere with the electron pairs localising on the spherical surface at maximum distance from one another. • A multiple bond is treated as if it is a single electron pair and the two or three electron pairs of a multiple bond are treated as a single super pair. • Where two or more resonance structures can represent a molecule, the VSEPR model is applicable to any such structure. The repulsive interaction of electron pairs decrease in the order: Lone pair (lp) – Lone pair (lp) Lone pair (lp) – Bond pair (bp) Bond pair (bp) – Bond pair (bp) Nyholm and Gillespie (1957) refined the VSEPR model by explaining the important difference between the lone pairs and bonding pairs of electrons. While the lone pairs are localised on the central atom, each bonded pair is shared between two atoms. As a result, the lone pair electrons in a molecule occupy more space as compared to the bonding pairs of electrons. This results in greater repulsion between lone pairs of electrons as compared to the lone pair - bond pair and bond pair - bond pair repulsion. These repulsion effects result in deviations from idealised shapes and alterations in bond angles in molecules. 👇👇👇👇👇👇 NEXT video 👇👇👇👇👇👇 🔴 VSEPR Theory (Part 2)    • VSEPR Theory - Part 2  🔴  Molecular S...   👇👇👇👇👇👇 𝑷𝑳𝑨𝒀𝑳𝑰𝑺𝑻 👇👇👇👇👇👇 🔴 Full playlist on Chapter 4 of Chemistry : 'Chemical Bonding and Molecular Structure' for Class 11 :    • Chemistry 11th : Chemical Bonding and...   👇👇👇👇👇👇👇👇👇👇👇👇 🔴 Kossel - Lewis Approach to Chemical Bonding    • 🔴 Kossel - Lewis Approach to Chemical...   🔴 Covalent Bond and its Types and Lewis Structure    • 🔴 Covalent Bond and its Types 🔴 Lewis...   🔴 Lewis Representation of Simple Molecules 🔴 Lewis Structure 🔴    • 🔴 Lewis Representation of Simple Mole...   🔴 Formal Charge || Chemical Bonding    • 🔴 Formal Charge || Chemical Bonding 🔴...   🔴 Formal Charges (Part 2) || H₂SO₄    • 🔴 Formal Charges (Part 2) || H₂SO₄ ||...   🔴 Limitations of OCTET Rule    • 🔴 Limitations of OCTET Rule 🔴 Chemica...   🔴 Bond Length    • 🔴 Bond Length  |  Covalent Radius  | ...   🔴 BOND Angle and TORSIONAL Angle    • 🔴 BOND Angle and TORSIONAL Angle || C...   🔴 BOND ENTHALPY    • 🔴 Resonance Structures || Chemistry f...   🔴 Resonance Structures    • 🔴 Resonance Structures || Chemistry f...   🔴 Polarity of Bonds    • 🔴 Polarity of Bonds || Chemistry for ...   🔴 Fajans' Rule    • 🔴 Fajans' Rule || Chemistry for Class...