The definition of London forces and their effect with respect to the size, number of atoms and the shape of the molecule are to be determined. Concept Introduction: The forces present between molecules that hold them together are known as intermolecular forces. There are different types of forces known. These include dispersion forces, hydrogen bonding, ion-dipole forces, dipole-dipole interactions, and so on. These forces play an important role in the polarizability of a molecule. London or dispersion forces refer to the type of intermolecular forces present in a non-polar molecule. London force (dispersion force; London dispersion force): A noncovalent molecular force caused by attraction of polarized electron clouds. The electron cloud polarization is induced: it is caused when the electron clouds repel each another, creating adjacent regions of electron deficiency (δ+) and electron excess (δ-). It has also been suggested the polarizations result from random fluctuations in electron density.
The definition of London forces and their effect with respect to the size, number of atoms and the shape of the molecule are to be determined. Concept Introduction: The forces present between molecules that hold them together are known as intermolecular forces. There are different types of forces known. These include dispersion forces, hydrogen bonding, ion-dipole forces, dipole-dipole interactions, and so on. These forces play an important role in the polarizability of a molecule. London or dispersion forces refer to the type of intermolecular forces present in a non-polar molecule. London force (dispersion force; London dispersion force): A noncovalent molecular force caused by attraction of polarized electron clouds. The electron cloud polarization is induced: it is caused when the electron clouds repel each another, creating adjacent regions of electron deficiency (δ+) and electron excess (δ-). It has also been suggested the polarizations result from random fluctuations in electron density.
Solution Summary: The author explains the definition of London forces and their effect with respect to the size, number of atoms, and the shape of the molecule.
The definition of London forces and their effect with respect to the size, number of atoms and the shape of the molecule are to be determined.
Concept Introduction:
The forces present between molecules that hold them together are known as intermolecular forces.
There are different types of forces known. These include dispersion forces, hydrogen bonding, ion-dipole forces, dipole-dipole interactions, and so on.
These forces play an important role in the polarizability of a molecule.
London or dispersion forces refer to the type of intermolecular forces present in a non-polar molecule.
London force (dispersion force; London dispersion force): A noncovalent molecular force caused by attraction of polarized electron clouds. The electron cloud polarization is induced: it is caused when the electron clouds repel each another, creating adjacent regions of electron deficiency (δ+) and electron excess (δ-). It has also been suggested the polarizations result from random fluctuations in electron density.
London forces become more important as the number of electrons in a molecule increases. Why?
Why are covalent bonds typically much stronger than inter-molecular forces?
Why does the temperature remain constant during a phase change?
The heat added during a phase change is only used to increase the motion of molecules.
The heat added during a phase change is only used to disrupt the attractive forces between molecules.
The heat added during a phase change is used to disrupt the attractive forces between molecules and to increase the
motion of the molecules.
The heat added during a phase change is only used to increase the vibration of molecules.