Studied by 4 people
Covers: Chapter 9 - Gasses & Chapter 10 - Liquids and Solids
Gas Pressure
The force exerted on a given area (P=F/A)
The relationship between pressure and temperature
Proportional ( P1/T1 = P2/T2)
The relationship between temperature \n and volume
Proportional (T1/V1 = T2/V2)
The relationship between pressure and volume
Inversely Proportional (P1 x V1 = P2 x V2)
The relationship between volume and amount (moles) of gas
Proportional ( V1/N1 = V2/N2)
What makes a gas behave ideally?
Low pressure and high temperature
Ideal Gas Law
PV=nRT
How the partial pressure of a gas in a mixture is related to the total pressure of the \n mixture.
Add all of the partial pressures together to get the total pressure of the mixture.
Mole Fraction
Number of moles of a component / Total moles
Diffusion
Prosses by which molecules disperse in space in response to differences in concentration
Effusion
The escape of a gas molecule through a tiny hole such as a pinhole in a balloon into a vacuum
How molar mass impact molecular speeds of gases.
The average speed of a molecule is inversely proportional to the square root of their masses
How temperature impact molecular speeds of gases.
The average kinetic energy of the gas molecule is proportional to temperature
The factors that make a gas behave non-ideally.
Low pressure and high temperature
Van der Waals Equation
Used on gasses that do not behave ideally
The two correction factors on the Van der Waals Equation
Molecule attraction and volume of molecules
Intermolecular Forces
Forces BETWEEN atoms/ molecules
Intramolecular Forces
Forces that hold an atom together in a molecule
Dispersion Forces
force that is present in all substances (caused by induced/ instantaneous dipoles)
Dipole-Dipole Forces
The force that is found in permanently polar molecules
Hydrogen Bonds (NOT REAL BONDS)
Forces that are found in liquids when Hydrogen is bonded to either Nitrogen, Oxygen, or Fluorine
Strength of intermolecular forces from least to greatest
Dispersion < Dipole-Dipole < Hydrogen Bonds
How polarizability impacts the strength of intermolecular forces
As polarizability increases, the IMFs also become stronger.
How polarizability impacts boiling point
As polarizability increases, so do boiling points.
How to rank polarizability of atoms/compounds
Smaller atoms are less polarizable than larger ones
Viscosity
A measure of a liquids resistance to flow
Relationship of viscosity and IMFs
Proportional, the stronger the IMFs the more viscus the liquid
Relationship of viscosity and Temperature
Inversely proportional, the higher the temperature the lower the viscosity.
How the strength of intermolecular forces impacts surface tension.
Proportional, as the stronger the IMFs the more surface temperature it has.
Vaporization
Liquid to Gas (endothermic)
Fusion
Solid to liquid (endothermic)
Sublimation
Solid to gas (endothermic)
Condensation
Gas to liquid (Exothermic)
Freezing
Liquid to solid (Exothermic)
Deposition
Gas to solid (Exothermic)
Boiling point
the temperature at which the vapor pressure of a liquid equals the external pressure surrounding the liquid.
Normal Boiling point
Boiling point when surrounding pressure is equal to 1 atm
Change in temperature equation
q= amount x Specific heat x Change in temperature
Change in temperature (phase change)
q= Amount x theta H of phase change
A
Gas
B
Liquid
C
Solid
D
Triple Point
E
Critical Point
Note 
Flashcard (24)