Week 2 Flashcards
Solid—> gas
Sublimation
Gas—> solid
Deposition
Solid—> liquid
Melting
Liquid—> solid
Freezing
Liquid —> gas
Evaporation
Gas—> liquid
Condensation
EN
Atoms with higher electro negativity will get shared electrons more; the result is a polar covalent bond. Partial - on high EN and partial + on lower en
Intermolecular forces in order strong-weakest
1) Force between permanent dipole and ion
2) force between permanent dipole (hydrogen bonding is much stronger)
3) force b/w permanent dipole and induced dipole
4) London force (force between induced dipole)
Solvent
Thing doing dissolving
Solute
What is being dissolved
Ampphipathic
Attraction to both polar and non polar
Bent shape
AX2E
Trigonal planar
AX3
Tetrahedral
AX4
Linear
AX2
PYRAMIDAL
AX3E
Vapor pressure
Pressure of vapor in contact with the matters liquid
Relative humidity =
Pp H2O/vapor pressure h2o
Heat of vaporization
Energy necessary to overcome all intermolecular forces so that molecules can escape into gas phase. Heat needed to boil
Heat of fusion
Necessary energy to convert 1 mole of solid into liquid at normal melting point. Heat needed to melt
Q-
Exothermic- feels hot
Q+
Endothermic- feels cold
Higher intermolecule force does what to vapor pressure?
Decreases
Boiling point
Vapor pressure equal to pressure it is exposed to
Which one is greater, heat of fusion of vaporization?
Heat of vaporization
Specific heat
Amt energy necessary to heat 1g 1degree C
Which concentration is not temp dependent?
Molality
Osmolarity is
Sum of all molarities. 1 M Nacl is 2 osm
Increased pressure does what to solubility
Increases
Increased temperature does what to solubility liquid solid and gas?
Temp increases solubility of liquid and solid but decreases in solubility of gases
Colligative properties
1) Vapor pressure decreases with increasing solute concentration
2) boiling point increases with increasing solute concentration
3) freezing point decreases with increasing solute concentration
4) osmotic pressure increases with increasing solute concentration
Raoult’s law
Vapor pressure of solute depends on concentration
Boyle’s law
PV with temp constant. Indirect. Press something, it gets smaller
Charle’s law
Volume/temp. Directly, volume up, temp up
Gay-Lussac’s law
Pressure/temperature, temp up, pressure up direct.
Avogadro’s law
Volume/mole. Direct. Mole up, volume up
Dalton’s Law
Sum of all pressures of each gas is the total pressure of the system.
Xi
Mole freaction mi/mtotal
Dew point
Point at which air cannot hold any more water
Assumptions of kinetic molecular theory of gas
1) gas molecules are small compared to volume of gas, so we can ignore the size of the molecule
2) gas molecules are in constant, random motion
3) gas molecules show range of kinetic energies, but average kinetic energy depends on temp
4) gas molecules are not attracted or repulsed from each other, so all collisions are elastic
Boltzmann’s constant
R/avogradro’s number.
KE of particle
1/2 mv2= 3/2 RT. M=molecular weight
Graham’s law of effusion
Smaller particles move faster and heating them up moves them faster
Real gas rules
Cannot completely ignore size of particles, especially at high pressures. At very low temperature, particles also begin to be more attracted to eachother
Van der Waals
Used when high pressure or low temp. Takes into account attraction.
