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CHEMI
intermolecular force
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Cards (28)
States of
matter
The fundamental difference between states of matter is the
strength
of the intermolecular forces of
attraction
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Condensed phases
Solids
and
liquids
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Intermolecular forces
Attractions between
molecules
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Types of intermolecular forces
Dispersion
forces
Dipole-dipole
forces
Hydrogen
bonding
Ion-dipole
forces
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London
dispersion forces
Attractions between an
instantaneous
dipole and an
induced
dipole
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Factors affecting the strength of London dispersion forces include
size
and
polarizability
of the molecules
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Dipole-dipole forces
Attractions between
polar
molecules
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For molecules of approximately equal mass and size, the more
polar
the molecule, the
higher
its boiling point
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Hydrogen bonding
Occurs when
hydrogen
is bonded to highly
electronegative
atoms like N, O, or F
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Ion-dipole
forces
Attractions
between an ion and a
polar
molecule
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Liquid properties affected by intermolecular forces include
boiling point
, viscosity, surface tension, and
vapor pressure
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Boiling point
The
temperature
at which a liquid converts into a
gas
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Strong intermolecular forces of attraction
High boiling point
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Vapor pressure
A measure of the tendency of a material to change into the
gaseous
or
vapor
state
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Strong intermolecular forces of attraction
Low
vapor pressure
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Crystalline
solids
Held together by
ionic
, covalent, or
metallic
bonds
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Phase changes
Transitions between the
states
of
matter
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Types of phase changes
Melting
Boiling
Sublimation
Deposition
Condensation
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Endothermic process
Absorption
of heat/energy
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Heating curve
A plot of
temperature
and
heat
added to a substance
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Cooling curve
A plot of
temperature
and
heat
removed from a substance
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Solid-liquid
equilibrium
When solid and
liquid
phases of a substance
coexist
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Liquid-vapor
equilibrium
When liquid and
gas
phases of a substance
coexist
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Phase diagram
Shows the
physical states
of a substance under different conditions of
temperature
and pressure
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Supercritical fluid
A phase that occurs for a gas at a specific temperature and pressure such that the gas will no longer
condense
to a liquid regardless of how
high
the pressure is raised
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Critical temperature
The temperature above which a gas cannot be
liquefied
by
pressure
alone
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The phase diagram of water shows the three areas of solid, liquid, and
gas
, as well as the critical
temperature
and pressure
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The phase diagram of CO2 shows the
supercritical fluid
region
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