At room temperature, bromine (Br2) is a corrosive red liquid, whereas iodine (I2) is a volatile

step 1 Both I2 and BR2 are non -polar molecules, therefore the only intermolecular force that they both

At room temperature, bromine (Br2) is a corrosive red...

At room temperature, bromine $\left(\mathrm{Br}_{2}\right)$ is a corrosive red liquid, whereas iodine $\left(\mathrm{I}_{2}\right)$ is a volatile violet solid. The differences point to different strengths of intermolecular forces between these halogens, with those for $\mathrm{I}_{2}$ being stronger. What kind of intermolecular force is responsible for these differences?

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Key Concepts

Intermolecular Forces

Intermolecular forces are the forces of attraction or repulsion between molecules, which play a crucial role in determining physical properties like boiling points, melting points, and states of matter. They include various types such as hydrogen bonding, dipole-dipole interactions, and London dispersion forces, with the latter being significant in nonpolar molecules.

London Dispersion Forces

London dispersion forces are a type of intermolecular force that arises from temporary fluctuations in electron density, creating instantaneous dipoles that induce dipoles in neighboring molecules. These forces are present in all atoms and molecules but are particularly influential in nonpolar substances where they are the dominant force. Their strength increases with the size and thus the polarizability of the molecule.

Polarizability

Polarizability refers to the ease with which the electron cloud around an atom or molecule can be distorted by external electric fields. A larger, more easily distorted electron cloud leads to stronger London dispersion forces. Thus, in similar nonpolar molecules, the one with a higher polarizability will typically have stronger intermolecular attractions, affecting its physical properties such as phase at room temperature.

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