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61 Cards in this Set
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- Back
- 3rd side (hint)
phase
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Any part of a system that looks uniform throughout
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phase change
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a change from one physica state to another (liquid, solid, gas)
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heat of fusion
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the heat needed to melt 1mol of a pure substance
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heat of vaporization
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heat needed to boil 1mol of a pure substance
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phase diagram
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graph that summarizes conditions which different states of a substance are stable
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liquid is more dense then curve leans left &melting point decrease with pressure
less dense,leans right and increases with pressure |
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london dispersion force
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occurs in all atoms
weak attractive forces increases with molar mass |
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dipole-dipole
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weak attractive forces between molecules with DIPOLE MOMENTS
must have polar covalent bonds and asymmetric |
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vapor pressure
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partial pressure of the vapor over a liquid
temp increases, vp increases intermolecular forces increase, vp decreases |
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boiling point
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temp at which vp of a liquid is equal to the pressure exerted on liquid
normal bp is 1 atm |
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surface tension
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energy required to increase the surface area of a liquid by a unit amount
intermolecular forces increase, surface tension increases |
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viscosity
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the resistance to flow exhibited by all liquids and gases
intermolecular forces increase, viscosity increases |
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hydrogen bonds
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a force that exists between a hydrogen atom covalently bonded to a very electronegative atom (N,O,F)
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solid
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nearly incompressible state of matter with a well defined shape
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molecular solid
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atoms or molecules
intermolecular forces low melting point soft and brittle non conductive ex: Ne, H2O, CO2 |
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polymeric solid
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very large molecules
intermolecular forces low melting point soft to hard non conductive ex:rubber, plastics, proteins |
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ionic solids
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ions
ionic bonding low to very high melting point hard and brittle non conductive, except as liquids ex: NaCl, K2SO4 |
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metallic solids
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metal atoms
metallic bonding variable melting point various hardness, malleable conductive ex: Fe, Cu, Ag |
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network solids
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atoms
covalent bonding very high melting point very hard usually non conductive ex: diamond, graphite |
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crystalline solid
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composed of one or more crystals
well defined ordered structure in 3D |
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amorphous solid
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disordered structure
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how many atoms are in a simple cubic cell
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1atom
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how many atoms are in a body centered cubic cell
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2atoms
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how many atoms are in a face centered cubic cell
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4atoms
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coordinating number
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number of nearest neigboring atoms to an atom
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solution
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a homogeneous mixture of two or more substances
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solute
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dissolved in substance
lesser amount |
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solvent
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dissolving medium
greater amount |
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solubility
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amount of a substance that will dissolve in a solvent
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saturated solution
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solution holding as much solute as is allowed at a stated temperature
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supersaturated solution
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a solution that contains more solute than is allowed at a given temperature. unstable solutions
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like dissolves like
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the more similar 2 compounds are the more likely one is soluble in the other (polar or non polar)
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miscible fluids
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fluids that dissolve each other in all proportions
these are solutions |
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immiscible fluids
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2 fluids that do not mix
these are not solutions |
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henry's law
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S=(kH)(P)
S is solubility of the gas kH is henry's law constant characteristic of the solution P is partial pressure of the gas |
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percent composition
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amount of solute / amount of solution × 100%
w/w = g/g v/v = mL/mL w/v =g/mL |
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molarity (M)
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moles of solute / liter of solution
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molality (m)
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moles of solute / kg solvent
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mole fraction
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X = moles of solute (solvent) / moles solute + moles solvent
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diluton equation
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c1v1 = c2v2
concentration and volume of a solution are inversely proportional |
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vapor pressure of solution
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uses mole fractions
change in Psolvent = (Ppuresolvent)(Xsolute) Psoln = Ppuresolvent - change in Psolvent |
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Raoult's law
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vapor pressure total = PsolventXsolvent + PsoluteXsolute
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freezing point depression
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find ◇Tf (◇Tf = Kf × cm)
Tf = Tof - ◇Tf uses molality |
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boiling point elevation
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find ◇Tb (◇Tb= Kb × cm)
Tb = Tob - ◇Tb uses molality |
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colligative properties
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properties that depend on solute concentration in a solution but not on the chemical identity of the solute
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semipermeable membrane
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certain membranes allow passage of solvent molecules but not solute particles
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osmosis
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phenomenon of solvent flow through a semipermeable membrane to equalize solute concentrations on both sides of the membrane
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osmotic pressure (pi)
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equal to the pressure that, when applied to the solution, just stops osmosis
pi as a variable pi = (i)(CM)(R)(T) R= ideal gas constant .0831 T=temp in K CM= molarity i= number of particles |
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osmolarity (osmol)
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osmolarity = i × CM
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colloid
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a solution in which the solute diameter is between 1nm and 1000nm
very large surface areas scatter light form stable dispersions |
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tyndall effect
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phenomenon in which light passing thru a colloid is scattered by colloid sized particles
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sol
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consists of solid particles dispersed in liquid
ex: jelly |
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aerosol
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consists of liquid droplets OR solid particles dispersed in gas
ex: clouds, smoke |
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emulsion
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consists of liquid droplets dispersed in another liquid
ex: milk, mayo |
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foam
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consists of gas dispersed in a solid or liquid
ex: whipped cream, marshmallows |
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gel
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consists of liquid dispersed throughout a solid
ex: cheese, butter |
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melting
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solid to liquid
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freezing
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liquid to solid
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vaporization
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liquid to gas
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condensation
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gas to liquid
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sublimation
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solid to gas
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deposition
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gas to solid
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