Home
Class 12
CHEMISTRY
What is the difference between London di...

What is the difference between London dispersion forces and dipole-dipole forces ?

Text Solution

AI Generated Solution

To answer the question regarding the difference between London dispersion forces and dipole-dipole forces, we can break it down into several key points. ### Step-by-Step Solution: 1. **Definition of London Dispersion Forces**: - London dispersion forces are weak intermolecular forces that arise from temporary fluctuations in electron density within non-polar molecules. These fluctuations create temporary dipoles that induce further dipoles in neighboring molecules, leading to an attraction. - **Example**: Hydrogen gas (H₂) and other non-polar molecules like Cl₂. ...
Promotional Banner

Similar Questions

Explore conceptually related problems

Point out the difference between London dispersion forces and dipole-dipole forces.

What are the differences between contact and non contact forces?

What is the main difference between London smog and Los Angeles smog ?

The energy order of dipole-dipole forces is'

Which substance has the strongest London dispersion forces ?

Which substance has the strongest London dispersion forces ?

The measure of net molecular polarity is a quantity called dipole moment which is defined as the magnitude of the charge Q at either end of the molecular dipole times the distance 'r' between the charge : mu=Qxxr Molecular polarities give rise to some of the forces that occur between molecules.Such forces are termed as intermolecular forces.These molecular forces are of several different types including dipole-dipole forces, London dispersion forces, hydrogen bonds and ion-dipole forces (operate between ions and molecules).These intermolecular forces are electrical in origin and results from the mutual attraction of unlike charges or the mutual repulsion of like charges. A formal positive charge on the central atom affect the size of orbitals.A formal positive charge on central atom will pull in all electrons towards the nucleus and this will leads to the contraction in size of orbitals. Which of the following molecule does not have dipole moment ?

The measure of net molecular polarity is a quantity called dipole moment which is defined as the magnitude of the charge Q at either end of the molecular dipole times the distance 'r' between the charge : mu=Qxxr Molecular polarities give rise to some of the forces that occur between molecules.Such forces are termed as intermolecular forces.These molecular forces are of several different types including dipole-dipole forces, London dispersion forces, hydrogen bonds and ion-dipole forces (operate between ions and molecules).These intermolecular forces are electrical in origin and results from the mutual attraction of unlike charges or the mutual repulsion of like charges. A formal positive charge on the central atom affect the size of orbitals.A formal positive charge on central atom will pull in all electrons towards the nucleus and this will leads to the contraction in size of orbitals. Select the correct statement.

London Dispersion force is present between :-

What are the main differences between electromotive force of cells and cell potential?