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Understanding Intermolecular Forces: The Glue of Molecular Interaction

Dive into the fascinating world of intermolecular forces that hold molecules together in various forms – dipole-dipole, hydrogen bonding, and London dispersion forces. Explore how these forces impact the physical properties of substances and distinguish them from intramolecular bonds. Discover the essential role of forces like dipole attraction and dispersion in determining whether a substance is solid, liquid, or gas at different temperatures. Unravel the secrets behind molecular cohesion and learn why size and structure matter in intermolecular interactions.

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Understanding Intermolecular Forces: The Glue of Molecular Interaction

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  1. Intermolecular ForcesForces that hold molecules together! Not to be confused with forces that hold atoms together to form a molecule (intramolecular). May the Force Be with You!

  2. Dipole – Dipole page 489 • Polar molecules are attracted to each other • Like a magnetic field • “sticking power” of the molecules • Not as strong as ionic or covalent bonds • Insignificant in gases because molecules are so far apart

  3. Hydrogen bonding page 490 • Strong dipole forces between molecules in which hydrogen is bonded to a very electronegative atom such as N, O, or F. • Electronegative atom “hogs” hydrogen’s only electron leaving it pretty much a proton that is very attracted to any unshared electrons on a molecule that happens by. • A type of dipole-dipole attraction

  4. London Dispersion Forces • Forces that exist among noble gas molecules and nonpolar molecules • Electrons are not really equally distributed at every instant • Have “moments” of attraction – induced or instantaneous dipole • Weak and does not last long • More significant as the size of molecules increases

  5. Type of Force Determines Properties • If the molecules have a lot of “sticking” power, they will be solids or liquids at room temperature. • If the molecules don’t stick together, they are gases. • Molecules that don’t stick together very well have low melting and boiling points. • Size of molecule is also a factor – generally, smaller, lighter molecules have lower mp & bp’s.

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