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44 Cards in this Set
- Front
- Back
Clausius–Clapeyron relation (Vapor Pressure)
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The cubic lattice types in which crystals have been known to crystallize are
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simple cubic
face centered cubic body centered cubic |
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number of atoms in a face centered cubic unit cell
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4
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number of atoms in a body centered cubic unit cell
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2
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number of atoms in a simple cubic unit cell
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1
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Viscosity
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Resistance of liquid to flow
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Surface tension
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The energy required to expand a liquid surface
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Volatility (of a liquid)
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The tendency of a liquid to vaporize (increases as temperature increases)
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Vapor Pressure
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A state of dynamic equilibrium in which molecules enter and leave the liquid at equal rates.
OR The pressure of a vapor in equilibrium with its non-vapor phases |
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Boiling
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When the vapor pressure equals the atmospheric pressure
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Relative Humidity Formula
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Vapor Pressure of atmosphere divided by equilibrium partial pressure of water vapor at the relevant temperature
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Relative Humidity
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Vapor pressure of of water in the atmosphere
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Vaporization
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liquid -> vapor
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Condensation
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vapor -> liquid
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ΔHºvap or ΔvH - Definition
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Enthalpy of vaporization - Energy required to transform a given quantity of a substance into a gas.
Equals -ΔHºcondensation |
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ΔHºsublimation - Definition
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Enthalpy of sublimation - Energy required to transform a given quantity of a substance into a gas.
Equals -ΔHºdeposition |
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ΔHºfusion - Definition
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Enthalpy of fusion - Energy required to transform a given quantity of a substance into a liquid.
Equals -ΔHºcrystallization |
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Fusion
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Solid -> liquid
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Crystallization
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liquid -> solid
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Sublimation
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solid -> gas
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Deposition
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gas -> solid
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Triple point
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The point in a phase diagram at which all 3 phases of matter are at equilibrium
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Phase Diagram
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chart used to show conditions at which thermodynamically-distinct phases can occur at equilibrium. Every pure substance that exists in all three phases has a distinct phase diagram
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Types of solids
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Ionic
Metallic Molecular Network Amorphous |
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Ionic solid - Structural Units
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positive & negative ions; no discrete molecules
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Ionic sold - Forces holding units together
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Ionic bonding
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Ionic solid - Typical properties
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Hard, brittle; high melting point, poor electrical conductor as solid, good as molten liquid; often water soluble
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Metallic solid - Structural Units
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Metal atoms
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Metallic sold - Forces holding units together
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Metallic bonding
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Metallic solid - Typical properties
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Malleable; ductile; good conductor
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Molecular solid - Structural Units
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Molecules with covalent bonds
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Molecular sold - Forces holding units together
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London Forces, dipole-dipole forces & hydrogen bonds
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Molecular solid - Typical properties
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low melting & boiling point; soft; poor electrical conductor
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Network solid - Structural Units
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Atoms held in infinite one-, two- or three-dimensional network
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Network sold - Forces holding units together
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Covalent bonds
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Network solid - Typical properties
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hardness and melting points decrease with # of bonds in network; poor electrical conductor
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Amorphous solid - Structural Units
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Covalently bonded networks of atoms or collections of large molecules
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Amorphous sold - Forces holding units together
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Covalent bonds
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Amorphous solid - Typical properties
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Noncrystalline; wide temperature range for melting; poor electrical conductor
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Crystal lattice
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The orderly, repeating arrangement of ions, molecules or atoms that shows the position of each particle
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Unit cell
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A small part of a lattice that, when repeated, reproduces the entire crystal structure
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Simple cubic edge - formula
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edge = 2 * atomic radius
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face-centered cubic edge - formula
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edge = 4 * atomic radius / sqrt(2)
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face-centered cubic edge - formula
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edge = 4 * atomic radius / sqrt(3)
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