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UNIT 11: Intermolecular forces, states of matter - Coggle Diagram
UNIT 11: Intermolecular forces, states of matter
IMFs
Ion-Dipole: Strongest IMF, important when considering solution/solute
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London Dispersion: B/n all molecules, when a molecule has an asymmetrical concentration of electrons and creates an instantaneous dipole, also influencing adjacent molecules
Are more effective in large, high-surface area, high # of electrons, long molecules
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Conceptual thoughts
Principles to always consider: equation for dipole, coulomb's law, ability to form instantaneous dipole, Boltzmann curve
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I think pressure, temp, and IMFs is central idea
Vapor Pressure
Only really matters in closed containers; in an open container, stuff will just evaporate away
(in a closed cont.) Temp of substance is always on a curve. As you heat it, more and more molecules gain enough energy to escape IMFs.
Simultaneously, they are more likely to bounce back into the liquid. Dynamic equilibrium is reached and vapor pressure stabilizes.
Once vapor pressure exceeds external pressure, liquid will boil.
Phase changes/curves
Phase change graph: Endothermic is gaining (kinetic) energy, exothermic opposite. Substance absorbs heat increasing temp until a phase change, then doesn't change temp during phase change.
Graph of temperature and pressure, basically shows intersections of phases. Sublimation points, boiling points, fusion points. Also since water condenses from gas to solid to liquid, pressure will cause solid to go to liquid.