Matter Week Flashcards
Liquid -> gas
Vaporization
Boiling
Gas -> liquid
Condensing
Gas -> solid
Deposition
Solid -> gas
Sublimation
Less energy = ? Stability
Less energy = more stability
“In atomic world”
AXE meaning
A = central atom X = stick on group E = lone pairs
4 Principle Interactions of Intermolecular Forces
- dipole dipole interactions
- hydrogen bonding
- London forces
- ion-dipole interactions
Dipole-Dipole Interaction
Attraction b/w opposite partial charges of 2 polar mlcs
H-Cl - - - - H-Cl
Hydrogen Bonding
Special type of dipole-dipole interaction
(Generally stronger than d-d interactions)
H to O F or N
Ion-Dipole Attraction
B/w an ion & polar mlc
Allows ion to dissolve in water
Surfactant parts
Mlc head polar
No polar tail
Polar heads get in between H2O mlcs & disrupt hydrogen bonding
Force of the collisions of gas mlcs averaged over area of container of liquid mlcs
Vapor Pressure of liquid
Dynamic Equilibrium , water level stay the same
Vaporization & condensation rates equal
Temp Increase = ? Vapor Pressure
Temp Increase = VP increases
Heat of vaporization (/\H vap)
Energy needed to liberate 1 mol of Liquid @ boiling point into gas phase
Mol fraction = vol fraction = pressure fraction
🤓
Mol fraction of med =
vapor P of med / total P
Dalton’s Law
More intermolecular forces = ? Boiling point
> im forces = > boiling point
Temp which vapor pressure = ambient pressure (1 atm)
Boiling Point
Temp that = Average molecular KE sufficient to overcome intermolecular forces that hold mlcs in liquid state
AX2E1
Ax2E2
Bent
AX2E0
Linear
AX3E0
Trigonal planar
AX3E1
Pyramidal
AX4
Tetrahedral
Increasing solute concentration = ? Boiling point
> solute concentration =
> Boiling Point
Increasing solute concentration =
? Freezing Point
> solute concentration =
< Freezing Point
Increasing solute concentration =
? Osmotic Pressure
> solute =
> Osmotic P
Increasing solute concentration =
? Vapor Pressure
> solute =
< Vapor P
Vapor Pressure of liquid
Caused by most energetic mlcs near surface of liquid escaping to gas phase
Exothermic
Feel warm
Solvation energy greater than lattice energy
Relates Vol to Pressure for gas
> V = ?P
Boyle’s Law
V1 P1 = V2 P2
> V = < P
Relates Vol to Temp
> T = ? V
Charles Law
V1/T1 = V2/T2
> T = >V
Relates Vol to moles of gas
> n = ? V
Avogadro’s Law
V1/n1 = V2/n2
> n = > V
SMV
Standard molar volume
22.7L/mol
Relative humidity
Partial Pressure / vapor Pressure
Molar enthalpy of fusion ( /\ H )
Heat necessary to convert one mole of a SOLID -> LIQUID @ it’s normal melting point
Molar enthalpy of vaporization ( /\ H)
Heat required to convert 1 mole LIQUID to GAS @ normal boiling point
