intermolecular bonding?

Question

at room temperature, chlorine is a gas, bromine is a liquid and iodine is a solid. Explain in terms of intermolecular bonding?

Answer 1

Iodine has the strongest inter. forces, so it stays a solid. Chlorine's are weaker, so it's a gas. This is b/c in London Dispersion Forces (since all 3 are diatomic), the more electrons, the stronger the bonds.

Answer 2

The physical properties of melting point, boiling point, vapor pressure, evaporation, viscosity, surface tension, and solubility are related to the strength of attractive forces between molecules. These attractive forces are called Intermolecular Forces. The amount of "stick togetherness" is important in the interpretation of the various properties listed above.

There are four types of intermolecular forces. Most of the intermolecular forces are identical to bonding between atoms in a single molecule. Intermolecular forces just extend the thinking to forces between molecules and follows the patterns already set by the bonding within molecules.

Answer 3

Chlorine is gas at room temp. b/c intermolecular bonding is weak between the atoms. Bromine is liquid at room temp. b/c intermolecular bonding between the atoms is moderate.(not strong or not weak).Iodine is solid at room temp. b/c intermolecular forces b/w the atoms are very strong.

I hope this helps!!

Answer 4

it is due to the size of the molecule. The larger the molecule, the larger the electron cloud. Hence larger electron cloud will get more polarised(more electron get polarised). As such the strength of induced dipole-induced dipole gets stronger as size of molecule increases. Size(Cl2)

Answer 5

Actually its due to the van Der Waals forces.