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50 Cards in this Set
- Front
- Back
solids can be changed to gases by adding energy |
sublimation |
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solids can be changed to liquids by adding energy |
melting |
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liquids can be changed to gases by adding energy |
vaporization |
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liquids can be frozen to solids by removing energy |
freezing |
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gases can be condensed to liquids by removing energy |
condensation |
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gases can be condensed to solids by removing energy |
deposition |
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pressure and volume are inversely proportional |
boyles law |
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volume and temperature are directly proportional |
charles law |
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as the number of moles increases, the volume will increase as well |
avogadros law |
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temperature and pressure are directly proportional |
gay-lussac law |
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when do gases deviate from ideal behavior? |
low temperature and high pressure |
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the mvmt of a gas into a vacuum |
effusion |
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the gradual mixing of two or more gases |
diffusion |
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short-range attractive forces operating between the particles that make up the units of a liquid or solid substance |
intermolecular forces |
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attractive forces between two oppositely charged ions |
ion-ion |
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attractive forces between an ion and a permanent dipole in a polar compound |
ion-dipole |
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attractive interactions between polar molecules |
dipole-dipole |
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very weak and very short-range attractive forces between temp dipoles |
london dispersion |
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a dipole-dipole interaction between molecules containing hydrogen directly bonded to N, O, or F |
hydrogen bonding |
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what intermolecular forces does HF have? |
dipole-dipole, dispersion, and hydrogen bonding |
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what intermolecular forces does HCl have? |
dispersion and dipole-dipole |
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diffuse freely into one another and form a homogenous solution (alcohol and water) |
miscible |
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do not diffuse freely into one another and do not form a homogenous solution (oil and water) |
immiscible |
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a measure of the ability of a liquid to evaporate quickly |
volatility |
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the stronger the intermolecular forces, the ______ the viscosity |
higher |
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forces that bind molecules to each other |
cohesive forces |
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forces that bind molecules to a surface |
adhesive forces |
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adesive forces > cohesive forces |
U-shaped (concave) |
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cohesive forces > adhesive forces |
curved downwords (convex) |
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capillary rise implies that….. |
adhesive forces are greater than cohesive forces |
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capillary fall implies that |
cohesive forces are greater than adhesive forces |
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the pressure exerted by a vapor in equilibrium with its liquid or solid phase |
vapor pressure |
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temp at which the vapor pressure of the liquid equals the applied pressure |
boiling point |
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what are the ways to get a liquid to boil? |
increase temp and decrease pressure |
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solids composed of structural units bounded by specific (regular) geometric patterns; characterized by sharp melting points |
crystalline solid |
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substances that do not display geometric regularity in the solid; do not have sharp melting points, but melt over a wide range of temps |
amorphous solids |
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atoms at the corners of a simple cube |
primitive cubic |
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atoms at the corners of a cube plus one in the center of the body of the cube |
body-centered cubic |
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atoms at the corners of a cube plus one atom in the center of each face of the cube |
face-centered cubic |
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discrete molecules that occupy positions in unit cells; attraction forces weak; usually soft and low melting points |
molecular solids |
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positive and negative ions arranged in a definite crystal structure; strong attraction; hard; high melting points |
ionic solids |
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individual atoms are covalently bonded to several other atoms; usually hard and high melting point |
covalent solids |
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positively charged nuclei imbedded in a sea of electrons; hardness varies but usually have high melting points |
metallic solids |
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what type of solid is CO2? |
molecular |
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what type of solid is ice? |
molecular |
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what type of solid is NaCl? |
ionic |
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what type of solid is a diamond? |
covalent |
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what type of solid is sand? |
covalent |
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what type of solid is potassium? |
metallic |
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what type of solid is aluminum? |
metallic |