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Chemistry Chap 6 Gas

QuestionAnswer
melting define heating of solid that involves thermal energy absorbed by the particles of the solid - solid to liquid
vaporization define energy absorbed by liquid particles making them move faster - liquid to gas
boiling point define temperature at which the pressure of the escaping vapor is the same as outside pressure - liquid to gas
sublimation define solid to gas
deposition define gas to solid
what are some characteristics of ionic bonds have higher melting and boiling points due to strong ionic bonds, form a conductive solution when dissolved, form hard crystals
what are some characteristics of molecular bonds have a lower melting and boiling point due to weaker bonds, form a nonconductive solution when dissolved, form soft "crystals"
chemical bonds are also known as intramolecular bonding
do ionic compounds have intermolecular bonds no
do molecular compounds have intermolecular bonds yes
define dispersion forces momentary, weak attractive forces between molecule
how do nonpolar substances exist in liquid and solid states dispersion forces
what are the only kind of forces present in nonpolar molecules dispersion
what types of molecules can dispersion forces be present in can be present in ionic, covalent, and non-polar bonds
define dipole-dipole forces occur between 2 polar molecules, weaker than ionic bonds but stronger than dispersion forces
define hydrogen bonds NOT REAL BONDS - hydrogen bonds to a seperate molecule
hydrogen bonds are weaker/stronger than covalent (intramolecular) bonds weaker
what elements are hydrogen bonds seen in H, N, O, F
what are all the intermolecular bonds from strongest to weakest hydrogen bonds, dipole-dipole forces, dispersion forces
how do solutions form when substances have similar strengths of force (likes dissolve likes)
how does salt dissolve in water allows the ions to have an alternative to ionic interaction in the crystal (form ion-dipole interactions)
what is law #1 of kinetic-molecular theory particles/molecules of a gas are in rapid, constant motion and move in straight lines
what is law #2 of kinetic-molecular theory particles of a gas are tiny compared with the distances between them
what is law #3 of kinetic-molecular theory there is very little interaction between gas molecules
what is law #4 of kinetic-molecular theory particles of gas collide with one another, energy is exchanged and conserved in these collisions
what is law #5 of kinetic-molecular theory temperature is a measure of the average kinetic energy of the gas particles
what are the 5 laws of kinetic-molecular theory see notes
what is Boyle's law for a given amount of gas at a constant temperature, the volume of the gas varies inversely with its pressure (pressure and volume)
what is the formula for Boyle's law PV=k (constant) - P1P2=V1V2
what is Charles' law the volume of a fixed amount of gas at a constant pressure is directly proportional to its absolute temperature (temperature and volume)
what is the formula for Charles' law V/T=K - V1/T1=V2/T2
what is Gay-Lussac's law pressure of a fixed amount of gas at a constant volume is directly proportional to its absolute temperature
what is the formula for Gay-Lussac's law p/t = k
what is Avagadro's law amount of gas is directly related to the gas volume when the temperature and pressure are constant
define molar volume volume occupied by 1 mole of gas
what is STP Standard Temperature and Pressure - pressure at 1 atm and temperature at 0 degrees Celcius
what is standard molar volume under STP 22.4 L
how to find the density of a gas at STP density of gas = molar mass of a gas/molar volume
what is the combined gas law PV/T=k
when is the combined gas law used when 2 variables of the 4 are held constant
what is the ideal gas law PV=nRT - R is 0.0821L*atm/mol*K at STP
when is the ideal gas law used incorporates possibility of all 4 variables changing
Created by: user-1965832
 

 



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