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Question	Answer
Intermolecular Forces	Forces that exist between molecules
Intramolecular Forces	Forces that exist within molecules
Melting	Solid to liquid phase change
Boiling/Vaporization	Liquid to Gas phase change
Sublimation	Solid to gas phase change
Freezing	Liquid to solid phase change
Condensation	Gas to liquid phase change
De-sublimation	Gas to solid phase change
Molecular Solids	Solids held together by dispersion forces Likely to dissolve in most solvents
Metallic Solids	Positive nuclei of metal atoms held together by valence electrons
Network Solids	Solids held together by covalent bonds Not likely to dissolve in most solvents
Ionic Solids	Held together by electrical forces between molecules
Collodial Suspension	Molecules uniformly disperses throughout the medium Between solutions and mixtures Between different phases
Miscibility	If a solute with dissolve in a solvent
Solubility	How much a solute will dissolve in a solvent
Saturation Point	Point where no more solute can be dissolved in the solvent
Alloy Substitution	Replacement of one solid atom with another to maintain general lattice shape
Alloy Interstitial Placement	Introduction of new solid atom distorts normal lattice structure
Dynamic Equilibrium	Rate of gas escaping the liquid phase is equal to the rate of gas dissolving into the liquid phase In a closed system
Surfactants	Hydrophobic tail and hydrophilic head Keep like phases near each other Reduce surface tension of a liquid
Monolayers	One row of surfactants to separate phases
Micelles	Surfactants form circle to enclose one phase from another
Vesicles	Bilayer of surfactants
Colligative Properties	Properties that change based on the amount of solute present
Vapor Pressure Reduction	Number of available solvent molecules at the surface to escape to gas phase is reduced with the introduction of a solute
Freezing Point Depression	Fewer solvent molecules available to change into solid phase because of introduction of solute
Boiling Point Elevation	Fewer solvent molecules able to reach surface and change into gas phase because of introduction of solute
Osmotic Pressure	Pressure applied to a solution to prevent the flow of solvent across a semi-permeable membrane
Properties of Liquids	Surface tensions, capillary action, viscosity, vapor pressure
Simple Cubic Unit Cell	Repeating unit form a 3D shape to represent the solid
Body-Centred Cubic Cell	Repeating unit centred around a cell
Face-Centred Cubic	Repeating unit centred around a cell with faces sticking out of the sides
Ion-Dipole Forces	Between ion and permanent dipole eg, Ion dissolved in water
Hydrogen Bonding Forces	Slightly polar hydrogen attracted to a lone pair eg, Water and ethanol
Dipole-Dipole Forces	Mutual attraction of two dipoles eg, HCl & HCl
Ion-Induced Dipole	Ion induces a dipole in another molecule then it is attracted to it eg, Ca2+ and O2
Dipole-Induced Dipole	Dipole induces a dipole in another molecule eg, HCl and Cl2
Dispersion Forces	Shifts of electron cloud density induce momentary attractions eg, CH4 &CH4
Intermolecular Forces - Strongest to Weakest	Ion-Dipole Hydrogen bonding Dipole-Dipole Ion-Induced Dipole Dipole-Induced Dipole Dispersion

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	Created by Andrea Smith almost 11 years ago