What is the predominant type of intermolecular force in I2 (iodine)?
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Van der Waals.
To determine the predominant type of intermolecular force in I2 (iodine), we need to consider the nature of the molecule and its intermolecular interactions.
Iodine (I2) is a diatomic molecule composed of two iodine atoms that are covalently bonded. In its solid and liquid phases, I2 molecules come together through intermolecular forces. The predominant type of intermolecular force in I2 is London dispersion forces, also known as van der Waals forces.
London dispersion forces occur in all molecules, including nonpolar molecules like I2. These forces result from temporary fluctuations in electron distribution, leading to temporary dipoles in the molecule. These temporary dipoles induce similar temporary dipoles in neighboring molecules, creating an attractive force between them.
In the case of I2, the London dispersion forces are the dominant intermolecular force because iodine is a relatively large molecule with many electrons. As a result, the temporary fluctuations in electron distribution are more significant, leading to stronger dispersion forces.
It's important to note that while I2 also has polar covalent bonds, the molecule as a whole is nonpolar. Therefore, the contribution of dipole-dipole interactions (another type of intermolecular force) is relatively negligible compared to London dispersion forces in I2.
To summarize, the predominant type of intermolecular force in I2 is London dispersion forces, due to the temporary fluctuations in electron distribution and induced dipoles.