What type of intermolecular force must be overcome in...

What type of intermolecular force must be overcome in converting each of the following from a liquid to a gas?
(a) liquid $\mathrm{O}_{2}$
(b) mercury
(c) $\mathrm{CH}_{3} \mathrm{I}$ (methyl iodide)
(d) $\mathrm{CH}_{3} \mathrm{CH}_{2} \mathrm{OH}$ (ethanol)

Key Concepts

Intermolecular Forces

Intermolecular forces are the attractive forces between molecules that determine many physical properties of substances, such as boiling and melting points. These forces include a variety of interactions that range in strength, and understanding them is essential for predicting how substances behave during phase changes like vaporization.

London Dispersion Forces

London dispersion forces are the weakest type of intermolecular force and arise due to temporary fluctuations in electron distribution around atoms or molecules, creating momentary dipoles. They are present in all molecules and are the only forces acting in nonpolar molecules, making them the primary force to overcome during the vaporization of substances like oxygen.

Dipole-Dipole Interactions

Dipole-dipole interactions occur between molecules that have permanent dipoles, where the positive end of one molecule attracts the negative end of another. These forces are stronger than London dispersion forces and are important in molecules that are polar, contributing significantly to the overall intermolecular attraction in such substances.

Hydrogen Bonding

Hydrogen bonding is a special, stronger type of dipole-dipole interaction that occurs when hydrogen is covalently bonded to highly electronegative atoms such as oxygen, nitrogen, or fluorine. This bond forms a significant attraction with lone pairs on nearby electronegative atoms, markedly increasing boiling points as more energy is required to overcome these interactions.

Metallic Bonding

Metallic bonding is the force that holds metal atoms together in a metallic lattice, where electrons are not bound to any specific atom but move freely throughout the structure. This delocalized electron 'sea' results in a bond that, while different from typical molecular intermolecular forces, must be overcome to convert a liquid metal to its gaseous form.

Transcript

Please give Ace some feedback