11.Liquids, Solids, and Phase Changes

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  • Created by: kpaul1234
  • Created on: 24-05-21 10:39
Define viscosity
the measure of a liquid’s resistance to
flow
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Define surface tension
the resistance of a liquid to
spreading out and increasing its surface area
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Define phase
a state of matter
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Define phase change
a process in which the physical
form but not the chemical identity of a substance
changes
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Define vapor pressure (Pvap)
the partial pressure of a
gas in equilibrium with liquid
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Define amorphous solids
a solid whose constituent
particles are randomly arranged and have no
ordered, long-range structure
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Define crystalline solids
a solid whose atoms, ions, or
molecules have an ordered arrangement extending over a long range
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Define ionic solids
a solid whose constituent particles
are ions ordered into a regular three– dimensional arrangement held together by ionic bonds
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Define molecular solids
a solid whose constituent
particles are molecules held together by intermolecular forces
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Define metallic solids
a solid consisting of metal
atoms, whose crystals have metallic properties
such as electrical conductivity
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Define unit cells
a small repeating unit that makes up a
crystal
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Define Simple cubic packing
a packing arrangement of
spheres into a primitive-cubic unit cell
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Define a primitive-cubic unit cell
a cubic unit cell with
an atom at each of its eight corners
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Define Body-centered cubic packing
a packing
arrangement of spheres into a body-centered
cubic unit cell
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Define a body-centered cubic unit cell
a cubic unit
cell with an atom at each of its eight corners and
an additional atom in the center of the cube
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Define Cubic closet packing
a packing arrangement
with three alternating layers, a-b-c-a-b-c.
a-b layers are identical to those in the hexagonal
closest-packed arrangement, but the third layer is
offset from both a and b layers
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Define face-centered cubic unit cell
a cubic unit cell
with an atom at each of its eight corners and an
additional atom on each of its six faces
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Define hexagonal closet-packing
g a packing arrangement two alternating layers, a-b-a-b. Each
layer has a hexagonal arrangement of touching
spheres, which are offset so that spheres in a
b layer fit into the small triangular depressions
between spheres in an a layer
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Define a phase diagram
a plot showing the effects of
pressure and temperature on the physical state of
a substance
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Define a normal melting point
the temperature at
which melting occurs when there is exactly 1 atm
of external pressure
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Define normal boiling point
t the temperature at
which boiling occurs when there is exactly 1 atm
of external pressure
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Define a triple point
a unique combination of pressure
and temperature at which gas, liquid, and solid
phases coexist in equilibrium
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Define a critical point
a combination of temperature
and pressure beyond which a gas cannot be
liquefied
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Define a supercritical fluid
a state of matter beyond
the critical point that is neither liquid nor gas
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State the Clausius-Claperyon equation
ln Pvap = ( -∆Hvap/R) 1/T + C
where ∆Hvap is the heat of vaporization, R is the gas constant, and C is a constant characteristic of the specific substance.
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State the Two-point form of the Clausius–Clapeyron equation
ln(P1/P2)= ∆Hvap/R(1/T2-1/T1)
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State the Bragg equation
d = (nwavelength)/(2 sin u)
where d is the distance between layers of atoms, l is the wavelength of the X rays, and u is the angle at which X rays strike the atomic layers.
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Other cards in this set

Card 2

Front

Define surface tension

Back

the resistance of a liquid to
spreading out and increasing its surface area

Card 3

Front

Define phase

Back

Preview of the front of card 3

Card 4

Front

Define phase change

Back

Preview of the front of card 4

Card 5

Front

Define vapor pressure (Pvap)

Back

Preview of the front of card 5
View more cards

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