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Intermolecular Forces of Attraction: - Coggle Diagram
Intermolecular Forces of Attraction:
IMFs occur in molecular solids
Types of solids
Ionic (lattice structure between ions and )
Molecular (molecules that experience IMFs)
Network Covalent (3D network of covalent bonds)
Metallic (metal atoms surrounded by sea of electrons)
ex. London Dispersion Forces, Hydrogen Bonds, Dipole-Dipole Attraction, Ion-Dipole, Ion-Induced Dipole, Dipole-Induced Dipole
In an ideal situation, gases do not experience IMFs
Ideal Gas Law
Kinetic Molecular Theory
Gas particles are in constant, random motions.
Size of gas particle is so small compared to the distance between particles, that volume becomes negligible.
Average kinetic energy is proportional to the Kelvin temperature of the gas.
Particles are assumed to have no attractive or repulsive forces (IMFs negligible)
PV=nRT
Boyle's Law: As gas pressure increases, gas volume decreases (P1V1=P2V2)
Charle's Law:As number of moles of gas increases, gas volume increases (V1/T1=V2/T2)
Avogadro's Law: As gas pressure increases, gas volume decreases (V1/n1=V2/n2)
Gay-Lussac's Law:There is a direct relationship between pressure and temperature (P1/T1=P2/T2)
Deviations from Ideal Gas Law
High pressure and low temperature both lead to LEAST Ideal situation.
With low temp, IMFs become significant because they slow molecules. With high pressures, molecules take up a significant part of the volume meaning they are no longer negligible.
IMFs influence solubility (Substances w/ similar IMFs to solvent will dissolve)
Solutions
Hydration; process where water molecules surround ions to dissolve them (Ion-dipole Attraction)
Aqueous solution is one where water is solvent
Solution will form if solvent-solute interactions are equal to or greater than solvent-solvent and solute-solute interactions.
Methods of Separating Mixtures
Distillation (Homogeneous)
Chromatography (Homogeneous)
Filtration (Heterogeneous)
Concentration
Measured in molarity-> M=n moles of solute/
L liters of solvent
Using UV-visible light spectroscopy you can shine a light through a solution to measure absorbance
Spectroscopy (how matter interacts with radiation)
Types of Radiation/Spectroscopy
Microwave Radiation (transitions in rotational motion)
Infrared Vibrational Spectroscopy (translations in vibrational motion)
UV-visible light spectroscopy (transition in electronic energy levels_
Photoelectric Current
How light shines on the surface of metal, causing electrons to be ejected from the surface if the frequency is higher than the threshold frequency determiines by the binding energy
Energy is proportional to frequency but inversely proportional to the wavelength
E=hv where e is energy, h is plank's constant (6.626x10^-34) and v is frequency
C=v(wavelength) where c is speed of light (3.00x10^8), v is frequency and wavelength is measured in m
E=hc/wavelength
Beer-Lambert Law
Measures the absorbance of a light shone through a solution and registered by a spectrophotometer/colorimeter
A=Ebc
where A is absorbance, E is the molar absorptivity constant and c is the concentration in terms of M