https://padlet.com/ayahsamara27/99wrex6wjna5 Made with magic en-us 2018-03-28 15:35:38 UTC 2026-01-08 19:06:03 UTC hello@padlet.com ayahsamara27 https://padlet.com/ayahsamara27/99wrex6wjna5/wish/246954432

Molecules can have more than one type of Intermolecular force

• All molecules have Dispersion forces but they may also have hydrogen bonding or dipole-dipole

Hydrogen-bonding is a dipole-dipole interaction between molecules that contain an H-F, H-O, or H-N bond 

• Hydrogen bonding doesn't exist between a single water molecule but between multiple molecules 

Vapor pressure decreases when the strength of the Intermolecular increases; they are inversely proportional  

higher boiling point = lower vapor pressure = stronger IMF 

lower boiling point = higher vapor pressure = weaker IMF

Effusion an diffusion depend on the molar mass of the gas involved but rates are not equal

Graham's Law of Effusion: rate of effusion of gas is inversely proportional to the square root of the molar mass of the particles 

In regards to Kinetic Molecular real gases deviate from ideal gases because their particles exert interactive forces and gas particles do occupy space and interact

]]> 2018-03-28 15:38:49 UTC https://padlet.com/ayahsamara27/99wrex6wjna5/wish/246954432 ayahsamara27 https://padlet.com/ayahsamara27/99wrex6wjna5/wish/246954808 Gas Pressure: created by the force exerted by gas molecules colliding with the surfaces of objects

Pressure: the force exerted on a given area

Diffusion: process by which molecules disperse in space in response to differences in concentration

Effusion: the escape of gas molecules through a tiny hole into a vacuum (evacuated space)

Graham's Law of Effusion: the rate of effusion of a gas is inversely proportional to the square root of the molar mass of the particles

Vapor Pressure: pressure exerted by the vapor in equilibrium with a liquid in a closed container at a given temperature

Boiling Point: (of a liquid) the temperature at which its equilibrium vapor pressure is equal to the pressure exerted on the liquid by its gaseous surroundings

Ionic Solids: composed of positive and negative ions held together by electrostatic attractions

Metallic Solids: uniform distribution of atomic nuclei with a "sea" of delocalized electrons

Covalent Network Solids: atoms are held together by a network of covalent bonds

Molecular Solids: composed of neutral molecules

Electrolytes: substances that yield ions in solution ]]> 2018-03-28 15:39:39 UTC https://padlet.com/ayahsamara27/99wrex6wjna5/wish/246954808 ayahsamara27 https://padlet.com/ayahsamara27/99wrex6wjna5/wish/246954866 Kinetic Molecular Theory- 
1. Gases are composed of molecules in random motion 
2. Molecules are negligibly small
3. Pressure results from collisions between particles and the walls
4. Gas molecules exert no attractive or repulsive forces and lose no energy
5. Average kinetic energy is directly proportional to temperature
Gas Laws- show relationships between temperature, volume, and pressure, and moles of gas
Ideal gases in lab conditions vs. real gases not at STP- Real gases behave ideal at high temp. and low pressure
Velocity of Particles- dependent on mass of atoms smaller moves faster and temp. higher is faster
Partial Pressures- each gas exerts a different pressure which combined make up total pressure
Effusion and Graham's Law- escaping of gas through a small hole used to find rates of effusion
Phase diagrams- show temperature points where substances change phases
IMFs- forces that hold molecules together, most substances have at least 1, change boiling point, freezing point, melting point, and vapor pressure based on strength
Polarizability- how easy it is to change a molecules charge distribution, depends on size and shape of molecule
Like dissolves like
Colligative properties- depend on number of solute molecules vapor pressure lowering, boiling point elevation, freezing point depression, and osmotic pressure
Van Hoff factor- ratio of solute particles in solution to # of fun dissolved, changes osmotic pressure and temperature change]]> 2018-03-28 15:39:45 UTC https://padlet.com/ayahsamara27/99wrex6wjna5/wish/246954866 drew_hollett19 https://padlet.com/ayahsamara27/99wrex6wjna5/wish/246954963 P = F / A
Gay-Lussac's Law: P₁/T = P₂/T₂
^{P: pressure (atm), T: temperature (K)}
Charles Law:   V₁/T₁ = V₂/T₂
^{V: volume (L), T: temperature(K)}
Boyle's Law:   P₁V₁ = P₂V₂
^{P: pressure (atm), V: volume(L)}
Avagadro's Law:  V₁/n₁ = V₂/n₂
^{V: volume(L), n: # of moles}
Ideal Gas Law:  PV = nRT
^{P: pressure(atm)
V: volume(L)
n: # of moles
R: gas constant (.0821)
T: temperature(K)}
Density: 
D=m/v
D = PM/RT
^{D: density(g/L)
M: molar mass (g/mol)
P: pressure(atm)}
Molar Mass:   M = mRT/PV
Partial Pressures:
P_total = P₁ + P₂ + P₃ + . . .
Graham's Law:
rate of effusion of A / rate of effusion of B
(M_B^1/2 / M_A^1/2)
Kinetic Energy: KE = 1/2mv^{2
KE: kinetic energy (J)
v: velocity (m/s)
m: mass (kg)}
Molarity:
M=mol solute / L solution
Molality:
m = mol solute / kg solvent
Mole Fraction:
X = mol A / total moles
Raoult's Law:
P_A = X_AP^o_A
Boiling Point Elevation:
T_b = K_b(m)
^{T_{b: temperature (}o_C)}
Freezing Point Depression:
T_f  = K_f(m)




]]> 2018-03-28 15:39:57 UTC https://padlet.com/ayahsamara27/99wrex6wjna5/wish/246954963 addisonrevans https://padlet.com/ayahsamara27/99wrex6wjna5/wish/246978750 https://docs.google.com/document/d/1Vl7NA5hYc0a2xXluOk3gk6HfVX0g6xL5OzMUXSsXNvE/edit?usp=sharing]]> 2018-03-28 16:30:03 UTC https://padlet.com/ayahsamara27/99wrex6wjna5/wish/246978750