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Describe the process of distillation.
Separates liquids based on differences in boiling points: vaporize, then condense.
Describe the process of filtration.
Use a filter to separate solids from liquids.
Describe the process of evaporation.
Boil off the solvent to leave the solute behind.
Describe the process of chromatography.
Separates substances based on interaction with a stationary phase.
Describe the dilution process.
Lowering the concentration of a solution, typically by adding more solvent.
What is the effect of increasing temperature on gas particle velocity?
Increases the average velocity of gas particles.
What is the effect of low temperature and high pressure on real gases?
Causes real gases to deviate from ideal behavior.
What happens when light reaches a certain threshold frequency on a metal?
Electrons are ejected from the metal (photoelectric effect).
What is the effect of stronger IMFs on viscosity?
Increases viscosity.
What happens when a nonpolar molecule experiences a temporary shift in electron distribution?
Temporary dipole is created, leading to London Dispersion Forces.
Define intermolecular forces (IMFs).
Attractions between molecules, not within them.
What are London Dispersion Forces (LDFs)?
Weakest IMF, present in all molecules, caused by temporary dipoles.
Define dipole-dipole interactions.
IMFs in polar molecules due to permanent dipoles.
What is hydrogen bonding?
Strong dipole-dipole interaction between H and F, O, or N.
Define ion-dipole interactions.
Strongest IMF, occurs in mixtures of ionic compounds and polar molecules.
Define molarity.
M = moles of solute / liters of solution.
Define solubility.
The ability of a substance to dissolve in a solvent.
Define the term 'photon'.
A discrete packet of light energy.
What is 'Polarizability'?
The measure of a molecule's ability to distort its electron cloud in response to an applied electric field.
Define 'Electrolytes'.
Substances that conduct electricity when dissolved in water or melted.