all matter is comprised of small constantly moving particles experiencing collisions in which energy is conserved (perfectly elastic)
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compressibility
property of matter arising from the empty spaces among particles
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fluidity
property of matter arising from the ease of movement of particles relative to each other
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incompressible not fluid
what can be said about the compressibility and fluidity of solids?
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low compressibility fluid
what can be said about the compressibility and fluidity of liquids?
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high compressibility fluid
what can be said about the compressibility and fluidity of gases?
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ideal gas
PV=nRT no attractive forces point masses (no volume)
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real gas
(P = n^2a/v)(V-nb)=nRT a -> dependent on magnitude of attractive forces b -> dependent on size of molecules
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liquids and solids
no simple equation bc you can't neglect/fix two things: 1) IMFs 2) particle size (relative to volume)
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sublimation
solid to gas
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deposition
gas to solid
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condensation
gas to liquid
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vaporization/evaporation
liquid to gas
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melting/fusion
solid to liquid
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freezing/crystallization
liquid to solid
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vapor pressure
the equilibrium partial pressure of the vapor over the liquid (or solid) at a given temperature (ex: Pwater)
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maxwell-boltzman distribution graph
graph that shows us liquid to gas phases, where the area under the curve is the # of particles able to escape into the gas phase
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boiling point
temperature at which the Pvap of the liquid is equal to the pressure on the liquid surface (Patm unless the vessel is closed)
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normal boiling point
T at which Pvap = 1 atm = 760 mmHg
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freezing point
temperature at which the pure liquid changes to a crystalline solid
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melting point
temperature at which the pure crystalline solid changes to a liquid
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pressure changes
freezing and melting point are both virtually unaffected by ...
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molecular
which type of substance is the easiest to melt/boil
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covalent network
which type of substance is the hardest to melt/boil
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temperature change to see phase changes
what does this graph show us
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-phase changes -all energy goes into changing phases not changing temperature (when it hits equilibrium
what do the horizontal lines indicate, and why does the temperature remain constant
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long line > high IMF; high energy required to change phase > long line
what does the length of each line indicate
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sloped line represents 1 phase high steepness = low specific heat
what does a sloped line represent? and what does the steepness indicate about specific heat?
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clausius-clapeyron equation
related Pvap to Tk of its liquid
NOTE: slope: negative; use R= 8.31 J/mol K need to find B value for each substance ln P = (-change in Hvap/R) (1/T) + B
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two point form
use the log form at two T's, T1 and T2 and subtract equations
ln (P2/P1) = change in Hvap/R (1/T1 - 1/T2)
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1 atm or 760 mmHg
if a problem says normal boiling point in it that means the pressure = ...
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phase diagram
a graphic to summarize the conditions, T and P, under which different states of a substance are stable
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area regions
condition where a given phase is stable
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line segments
conditions where two phases exist in equilibrium
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specific heat
the quantity of heat required to raise the temperature of one gram of a substance by one Celsius degree
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triple point (TP)
conditions where all three phases exist in equilibrium
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critical point (CP)
T above which the liquid does not exist regardless of the pressure (Ek has totally overcome all attractive forces)
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surface tension
energy required to increase the surface area of liquid by a unit amount; results from the net force toward the interior of the liquid experienced by a surface molecule
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capillary rise
phenomenon related to the surface tension -water molecules attract to glass, bc of this attraction, a thin film of water starts to move up inside of the glass capillary, thus making a meniscus
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viscosity
the resistance to flow that is exhibited by all liquids and gases
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liquid is slow
high viscosity, really viscous
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easy to pour
low viscosity
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imfs
the forces of interaction between molecules (typically weakly attractive; abt 100 to 1000 times smaller than bond energies)
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van der waals forces
weak attractive forces (LDF and dipole-dipole)
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london dispersion forces
weak intermolecular attractive forces resulting from the small, instantaneous, synchronized dipoles occurring due to the varying positions of the electrons of the electrons as they move about the nuclei
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increase w molar mass
ldfs tend to
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polarizable
larger atoms are more
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polarizable
molecules that are more spread out tend to be more
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dipole dipole forces
one polar molecule's partial positive charge is attracted to the partial negative of another polar molecule
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stronger
LDF is __ than DD but DD is permanent
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weak Pvap strong surface tension high normal boiling points high viscosity
strong IMFS yield
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ion dipole
the attractive force between a polar molecule and a charge particle ion -the attraction must be between a partial negative and cation or partial positive and anion
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hydrogen bonding
a weak to moderate attractive force that exists between an H atom covalently bonded to an N, O, or F atom and an N, O, or F atom on another molecule
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hydrogen bonding
___ receives its strength from the partial exposure of the proton of the H nucleus when it is bonded to a highly electronegative atom
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molecular
consists of atoms or molecules held together by IMFS; NM/NM
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metallic
consists of positive cores of atoms held together by a "sea" of mobile electrons; M
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ionic
consists of cations and anions held together by the electrical attraction of opposite charges; M/NM
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covalent network
consists of atoms held together in large 3D or 2D networks or chains
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C (diamond) C (graphite) C60 SiO2 SiC
five covalent networks
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LDF, DD/HB, Ionic/Metallic, Covalent Network
list all the force and bond types in order from weakest to strongest
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-high melting points -brittle, hard -poor conductors of heat and electricity -dull