Part 3
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| How is kinetic energy and vapor pressure related? | kinetic energy allow molecules to overcome the attractive force between the molecules; the weaker the force, more molecules escape, the more molecules escape the greater the vapor P.
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| why does vapor P increases with T? | at higher T, more molecules have the KE to escape the attractive force of the liquid phase. The more molecules in the vapor phase, the higher the vapor pressure
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| What will the interior bubble do if the external P is greater than the vapor P? | it will collapse
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| If the external P is equal to or lower than the vapor P, then the bubble will... | remain or expand and the liquid boils
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| At 100 C the vapor P of water is what? | 760 torr (1 atm), water boils.
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| "triple point" | condition of T and P where are 3 physical states are in equilibrium
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| gases are most likely under... | high T
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| solids are most likely under... | high P
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| which is denser, liquid water or ice? | liquid, the liquid state is more compacted than the solid state for water
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| what T will water boild? | 100 C if the water is at 1 atm of pressure
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| at pressure below 4.58 torr, water will be... | a gas or solid, there can be no liquid phase.
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| give examples of crystalline solids | diamonds, and quartz crystals,
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| crystalline solids | atoms/molecules/ions pack together in an ordered arrangement. Have flat surfaces w/unique angles between faces and unique 3-dimensional shape
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| amorphous solids | no ordered structure, no well defined faces/angles/or shape. Often are mixtures of molecules which do not stack together well, or large flexible molecules.
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| examples of amorphous solids | glass and rubber
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| crystal lattice | identical points on each unit cell of the crystal.
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| cubic | shape of unit cell. all sides are equal length, all angles are 90 degrees
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| does a unit cell have to be cubic? | no
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| what are the 2 arrangement that sphere can be pack in 3 dimensions | hexagonal close packing and cubic close packing
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| hexagonal close packing | layer 3 sits in depressions of layer 2 and is directly above positions in layer 1
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| cubic close packing | layer 3 sits in depressions of layer 2 but is not directly above positions in layer 1
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| coordination number | number of particles surrounding a particle in the crystal structure
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| what intermolecular forces hold molecular solids together? | dipole-dipole, dispersion, and hydrogen bonds
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| Why are molecular solids soft and have low melting T? | because their intermolecular forces are weaker than chemical (covalent) bonds
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| dispersion bond energy (kJ/mol) | about 1.0
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| hydrogen bond (strongest dipole-dipole) bond energy (kJ/mol) | about 12 - 16
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| ionic bond energy (kJ/mol) | about 50 - 100
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| covalent bond energy (kJ/mol) | about 100 - 1000
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| what are the force that holds covalent solids together? | covalent bonds
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| what is the force that holds ionic solids together? | ionic bonds
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| What does the strength of the ionic interaction dependent on? | the strength of the charge of the ions
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| the bonding of metallic solids increases with what? | the #s of electrons available for bonding
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| why can metals carry electrical current? | because of the delocalization of electrons (electrons are free to move about the metal structure)
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| what are the 3 kinds of cubic unit cells? | primitive cubic, body-centered cubic, and face-centered cubic
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| which solids are hard and brittle and have high melting point? | ionic solids
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