| Term | Definition |
|---|
| density relates to the level of | attraction |
| compressibility relates to the level of | intermolecular distance |
| ideal gas | a model of the way that particles of a gas behave at the microscopic level |
| what are the 4 characteristics of a gas that we can measure? | temperature, volume, pressure, mass in moles |
| pressure | force per unit area |
| gas pressure is a result of | force exerted by the collision of particles with the walls of the container |
| what 2 units of pressure will we pretty much be working with? | atm and torr |
| 1atm = ____ mmHg | 760 |
| 1atm = ____ torr | 760 |
| 1mmHg = ____ torr | 1 |
| density of water | 1 g/mL |
| density of organic solvents | .8 g/mL |
| as temperature goes up, particle speed | goes up |
| diffusion states that gas particles will move from ____ to ____ concentration | high, low |
| true/false: gas diffusion is mass dependent | true |
| boyle's law in terms of symbols | PV = k |
| when working with gas equations, temperature must always be converted to | kelvin |
| kelvin = | C + 273.15 |
| celcius = | K - 273.15 |
| charle's law in terms of symboles | V/T = K |
| if all 3 variables are changing, use the | combined gas law |
| combined gas law in terms of symbols | P(initial)V(initial)/T(initial) = P(final)V(final)/T(final) |
| avogadro's law in terms of symbols | V/n = K |
| molar volume | the volume occupied by one mole of any gas |
| stp | standard temperature and pressure |
| standard temperature | 273K (0 C) |
| standard pressure | 1atm |
| at stp, the molar volume of any gas is | 22.4L |
| the ideal gas law | PV = nRT |
| dalton's law in symbols | p(t) = p1 + p2 + p3 + ... |
| is there actually such a thing as an ideal gas? | no |
| why do nonpolar gases behave more ideally than polar gases? | attractive forces are present in polar gases |
| viscosity | a measure of a liquid's resistance to flow |
| viscosity is a function of both ________ and _______ | attractive forces between molecules, molecular geometry |
| as temperature increases, viscosity _____ | decreases |
| surface tension | a measure of the attractive forces exerted among molecules at the surface of a liquid |
| how do surface particles act due to surface tension? | they try to get closer to the particles below them |
| net attractive forces on surface molecules _____________ | pulls them downward |
| surfactant | a substance added which decreases the surface tension |
| is it possible to keep all molecules in the liquid phase? | no |
| kinetic theory | liquid molecules are in continuous motion, with their average kinetic energy directly proportional to the kelvin temperature |
| evaporation is an __________ reaction | endothermic |
| condensation is an ___________ reaction | exothermic |
| evaporation | the process of conversion of liquid to gas at a temperature too low to boil |
| condensation | conversion of a gas to the liquid state |
| a system is said to be at equilibrium when | the rate of evaporation equals the rate of condensation |
| vapor pressure of a liquid | the pressure exerted by the vapor at equilibrium |
| boiling point in terms of vapor pressure | the temperature at which the vapor pressure of the liquid becomes equal to the atmospheric pressure |
| normal boiling point | temperature at which the vapor pressure of the liquid is equal to 1atm |
| what happens when you go to a mountain where the atmospheric pressure is lower than 1atm? | the boiling point lowers |
| boiling point depends on the | intermolecular forces |
| dipole-dipole interactions | attractive forces between polar molecules as the positive end of one part lines up with the negative of the other |
| another name for london forces | dispersion forces |
| london forces | as electrons are in continuous motion, a nonpolar moelcule could have an instantaneous dipole; they line up for a moment and are not that strong |
| hydrogen bonding is a special type of | dipole-dipole attraction |
| hydrogen bonding | a very strong intermolecular attraction that causes higher than expected b.p. and m.p. |
| requirement for hydrogen bonding: | molecules have hydrogen directly bonded to O, N, F (electronegative elements) |
| is hydrogen bonding stronger or weaker than van der waals forces? | stronger |
| are solids compressible? | no |
| the melting point of a solid depends on the | strength of attractive force between particles |
| the two formations of a solid | crystalline and amorphous |
| crystalline solid has | a regular repeating structure |
| amorphous solid has | no organized structure |
| the disparity between gas volume and liquid volume is | huge |
| the disparity between liquid volume and solid volume is | small |
| the four types of crystalline solids | ionic, covalent, molecular, metallic |
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