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51 Cards in this Set
- Front
- Back
van der Waals forces
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collectively forces between molecules, everything has them
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Dipole-Dipole interaction
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Polar molecule encounters polar molecule
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Hydrogen Bonding
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O, N, F that have a lone pair bond to a Hydrogen
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Dipole-Induced Dipole Interactions
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When a dipole pushes a molecule into a induced dipole (water and O2)
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polarization
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process of inducing a dipole
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polarizability
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the degree to which the electron cloud of an atom or a molecule can be distorted
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Induced-Dipole/Induced-Dipoloe---London Dispersion Factors
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nonpolar, everything has them pretty much
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vaporization
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evaporation the process from liquid to gas
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molar enthalpy of vaporization
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the energy required to vaporize a sample
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condensation
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gas to liquid by losing energy
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dynamic equilibrium
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when the masses of liquid and vapor in the flask remain constant
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equilibrium vapor pressure
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is the pressure exerted by the vapor in equilibrium with the liquid phase
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volatility
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the measure of the tendency of the liquid molecules to escape from the liquid phase and enter the vapor pressure at a given temperature
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Clausius-Clapeyron equation
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provides a method for determining the delta vaporization H not
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normal boiling point
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the temperature when the substance boils at 1 atm or 760 mmHg
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critical point
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liquid/vapor exist at the same time
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supercritical fluid
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gas and a liquid properties and the critical point
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surface tension
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the energy required to break through the surface or to disrupt a liquid drop and spread out the material
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capillary action
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climbing of the water in a thin tube
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adhesive forces
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water to wall
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cohesive forces
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water to water
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viscosity
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resistance to flow
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solution
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homogenous mixture of two or more substances in a single phase
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solvent
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water usually large quantity
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solute
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usually solid, what is mixed into something
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colligative properties
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properies of solution that depend only on the number of solute particles per solvent molecule and not on the identity of the solute
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molality
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moles of solute/mass of solvent in kg
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mole fraction
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mole of n/moles total
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weight percent
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mass of n/mass of total
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parts per million
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dilution of a solution
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saturated
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no more particles can dissolve in it
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solubility
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the concentration of solute in equilibrium with undissolves solute in a saturated solution
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miscible
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mix
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immiscible
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don't mix
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hydration
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water is solvent, exothermic, when ions dissolve in water
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Henry's Law
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solubility of a gas in a liquid is directly proportional to the gas pressure
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Le Chatelier's Principle
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states that a change in a any of the factors determining an equlibirum cases the system to adjust by shifting in the direction that reduces or coutneracts the effects of the change
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Raoult's Law
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vapor pressure of a solvent over a solution is some fraction of the pure solven tequilibirum vapor pressure......P solvent=Xsolvent*Pnotsolvent
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osmosis
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movement of solvent molecules through a semipermeable membrane from a region of lower solute concentration to a region of higher solute concentration
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osmotic pressure equation
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Pi=cRT
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osmotic pressure
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pressure counterbalancing from atmosphere and the water in a tube
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van't Hoff factor
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i=usually 1 unless ion, then count them
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colloidal dispersion (Colloids)
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represent a state intermediate between a solution and a suspension
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Tyndall effect
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colloids scatter visible light when dispersed in a solvent, making the mixture appear cloudy
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sol
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colloidal dispersion of a solid substance in a fluid medium
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gel
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colloidal dispersion that has a structure that prevents it from being mobile
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hydrophobid/hydrophyllic
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water hating/water loving
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emulsions
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colloidal dispersion of one liquid in another, such as oil in water
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emulsifying agent
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soap that allows for milk (water and oil) to form
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surfactants
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substances such as soaps that affect the properties of surfaces
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detergent
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special sufactant
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