Iodine molecules are held in the crystal lattice by: a) London forces b) dipole-dipole interactions c) Covalent bonds d) Coulombic forces

Iodine molecules are held in the crystals lattice by

Dry ice is a crystalline solid in which particles are held together by London force Dipole-Dipole attraction Covalent bond Coulombic force

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

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

The high density of water compared to ice is due to (a)hydrogen bonding interactions (b)dipole -dipole interactions (c)dipole - induced dipole interactions (d)induced dipole -induced dipole interactions

The intermolecular forces operating between two constituent particles depends on the distance between the centres of the molecules. Dipole-dipole interactions are inversely proportional to 3rd power of the distance where as dipole induced dipole interaction are inversely proportional to the sixth power of intermolecular distances. The forces in dry ice are proportional to (r = intermolecular distance)

The intermolecular forces operating between two constituent particles depends on the distance between the centres of the molecules. Dipole-dipole interactions are inversely proportional to 3rd power of the distance where as dipole induced dipole interaction are inversely proportional to the sixth power of intermolecular distances. In which of the following the extent of interaction is proportional to 1/r^(6) where (r = intermolecular distance)

Arrange the following types of intermolecular forces in order of decreasing their strength (a) Ion dipole (b) Keesom forces (C ) Dispersion or London forces (d) Dipole-induced dipole (e) lon-induced dipole (Debye forces) .

Polar covalent molecules exhibit dipole moment. Dipole moment is equal to the product of charge separation , q and the bond length d for the bond. Unit of dipole moment is debye. One debye is equal to 10^(-18) esu cm. Dipole moments is a vector quantity. It has both magnitude and direction. Hence, dipole moment of a molecule depends upon the relative orientation of the bond dipoles, but not on the polarity of bonds alone. A symmetrical structure shows zero dipole moment. Thus, dipole moment helps to predict the geometry of a molecules. Dipole moment values can be distinguish between cis- and trans- isomers, ortho, meta and pare-forms of a substance, etc. Q. Which is a polar molecule?

Polar covalent molecules exhibit dipole moment. Dipole moment is equal to the product of charge separation , q and the bond length d for the bond. Unit of dipole moment is debye. One debye is equal to 10^(-18) esu cm. Dipole moments is a vector quantity. It has both magnitude and direction. Hence, dipole moment of a molecule depends upon the relative orientation of the bond dipoles, but not on the polarity of bonds alone. A symmetrical structure shows zero dipole moment. Thus, dipole moment helps to predict the geometry of a molecules. Dipole moment values can be distinguish between cis- and trans- isomers, ortho, meta and pare-forms of a substance, etc. Q. Which is a polar molecule?