Determine the kinds of intermolecular forces that are present in each element or compound. b. I₂

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Identify the molecular structure of iodine (I_2). Iodine is a diatomic molecule consisting of two iodine atoms bonded together.

Recognize that iodine (I_2) is a nonpolar molecule because the two iodine atoms have the same electronegativity, resulting in an equal sharing of electrons.

Understand that nonpolar molecules primarily exhibit London dispersion forces, which are the weakest type of intermolecular force and arise due to temporary dipoles induced in atoms or molecules.

Consider the size of the iodine molecule. Larger molecules like I_2 have more electrons, which can lead to stronger London dispersion forces compared to smaller molecules.

Conclude that the primary intermolecular force present in iodine (I_2) is London dispersion forces.

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Key Concepts

Here are the essential concepts you must grasp in order to answer the question correctly.

Intermolecular Forces

Intermolecular forces are the attractive forces between molecules that influence physical properties such as boiling and melting points. These forces include hydrogen bonding, dipole-dipole interactions, and London dispersion forces. Understanding these forces is crucial for predicting the behavior of substances in different states of matter.

London Dispersion Forces

London dispersion forces are a type of intermolecular force that arise from temporary fluctuations in electron density within molecules, leading to temporary dipoles. These forces are present in all molecules, but they are the only type of intermolecular force in nonpolar substances, such as iodine (I2). The strength of these forces increases with the size and polarizability of the molecules.

Molecular Polarity

Molecular polarity refers to the distribution of electrical charge across a molecule, which determines the type of intermolecular forces it can exhibit. Polar molecules have a significant difference in electronegativity between their atoms, leading to dipole-dipole interactions, while nonpolar molecules, like I2, exhibit only London dispersion forces. Understanding polarity is essential for predicting how substances will interact with each other.