Intermolecular Forces Quiz

Intermolecular Forces Overview

• Hydrogen bonds are the strongest intermolecular force, formed between a slightly positive hydrogen and a slightly negative atom on another molecule.
• Hydrogen bonds lead to molecules being packed closely together in liquids and solids.
• Ion-dipole interactions involve a neutral molecule with a dipole and an ion, occurring when polar solvents dissolve ionic compounds.
• Ion-dipole interactions are weaker than hydrogen bonds but stronger than dipole-dipole forces.
• Dipole-dipole forces occur between the positive end of one polar molecule and the negative end of another due to unequal electron distribution.
• Amino acids are an example of polar molecules that undergo dipole-dipole interaction.
• Strong intermolecular forces cause substances to have higher melting, boiling, and freezing points, as well as higher viscosity and surface tension.
• Intermolecular forces act between molecules, while intramolecular forces hold a molecule together.
• Intramolecular forces enable molecules to retain their basic atomic and subatomic makeups during interactions.
• London dispersion forces are intermolecular forces caused by the attraction of negative and positive charges, classified into three types: dispersion forces, dipole-dipole attraction forces, and hydrogen bonds.
• Dispersion forces are the weakest intermolecular force, followed by dipole-dipole attraction forces and hydrogen bonds.
• These forces are essential for understanding the behavior and properties of substances in various states.

Intermolecular Forces and Molecular Polarity

• London dispersion forces are also known as induced dipole-induced dipole forces and explain variations in boiling points.
• Dipole-dipole attraction and London dispersion forces are main intermolecular forces.
• Molecular polarity results from non-zero net dipole in a molecule due to differing electronegativities.
• Determining molecular polarity involves checking shape and presence of lone pairs of electrons.
• Methane is non-polar due to its symmetrical tetrahedral shape.
• Hydrogen fluoride and ammonia are polar due to asymmetrical shapes and electronegativity differences.
• Chloromethane is polar due to the highly electronegative chlorine atom.
• Carbon tetrachloride and ethene are non-polar due to their symmetrical structures.
• Determining a molecule's dipole moment involves assessing shape and electronegativity differences.
• Water is polar due to its asymmetrical shape and electronegativity differences.
• Carbon tetrachloride is non-polar due to its symmetrical structure.
• Carbon dioxide is non-polar due to its linear, symmetrical shape and canceling polar ends.