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Point out the difference between London ...

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

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### Step-by-Step Solution: 1. **Definition of Forces**: - **Dipole-Dipole Forces**: These are attractive forces that occur between molecules that have permanent dipoles, meaning they are polar. A permanent dipole arises from the uneven distribution of electron density between atoms in a molecule, leading to regions of partial positive and negative charge. - **London Dispersion Forces**: These are weak intermolecular forces that exist between all molecules, whether they are polar or non-polar. They arise due to temporary fluctuations in electron density that create instantaneous dipoles, which induce dipoles in neighboring molecules. 2. **Nature of Molecules**: - **Dipole-Dipole Forces**: Operate specifically in polar molecules. For example, hydrogen chloride (HCl) exhibits dipole-dipole interactions because of the difference in electronegativity between hydrogen and chlorine, resulting in a permanent dipole. ...
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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. Select the correct statement.

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Between ionic and covalent bonds, there are large majority of bonds, in which the bonding electrons are shared unequally between two atoms but are not completely transferred.Such bonds are said to be polar covalent bonds and the bond polarity is due to difference in electronegativity, the ability of an atom in a molecule to attract the shared electrons in a covalent bond. The measure of net polarity is a quantity called the dipole moment, mu , which is defined as the magnitude of the charge Q at either end of the molecular dipole times the distance r between the charges : mu=Qxxr .Molecular polarities give rise to some of the forces that occur between molecules and these forces are of several different types including dipole-dipole forces, London dispersion forces, and hydrogen bonds. All these intermolecular forces are electrical in origin and result from the mutual attraction of unlike charges or the mutual repulsion of like charges. Which of the following statements is incorrect ?

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