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NDSU CHEM 122 - Intermolecular Forces
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CHEM 122 1st Edition Lecture 1 Outline of Last LectureN/A Outline of Current Lecture I. Three Physical States of Mattera. Gasesb. Liquidsc. SolidsII. Intermolecular/Intramolecular Forcesa. PolarizabilityCurrent LectureThree Physical States of Matter:Gases:- Expand to fill its container- Low density- Diffusion is rapid- Very compressible- Free molecular motion- Very fluid, flows easilyLiquids:- Have a definite volume but take the shape of the container- High density- Diffusion is slow- Only slightly compressible- Molecules can move past one another- Very fluidThese notes represent a detailed interpretation of the professor’s lecture. GradeBuddy is best Used as a supplement to your own notes, not as a substitute.Solids:- Have a definite volume and shape- High density- Diffusion is extremely slow- Only slightly compressible- Molecules are held in fixed positions- Not fluid*Almost all substances that are liquids at room temperature (25 degrees C) are molecular*Intramolecular force: atoms that are held together by strong forces (Covalent bonds)Intermolecular Force: weaker forces acting between molecules to hold them close together.Three types of intermolecular Forces/van der Waals Forces:- London Dispersion- Dipole-Dipole- Hydrogen BondingInstantaneous dipole: positions of the electrons at a particular instant in time resulting in electrostatic attraction.London Dispersion Forces: Electrons constantly in motion with the instantaneous dipoles constantly changing but all changing together resulting in electrostatic attraction.- All molecules have this force of attractionPolarizability: how easily the electron distribution of a molecule can be distorted.- The more electrons the more polarizable it is and the stronger the London forces


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NDSU CHEM 122 - Intermolecular Forces

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