Shivani Lal Period 3 Semester 2

Solutions

IMFs

Gases

Charles law: T1/V1 = T2/ V2

Boyle's Law: P1V1=P2V2

Gay-Lussacs law: P1/T1 = P2/T2

Combined gas Law: P1V2/T1 = P2V2/T2

Ideal gas law: pv=nrt

r = 0.082 in atm, 8.31 in kPa

ideal conditions: high temperature, low pressure

Molarity = mol solute/Liters of solution

Molality = mol solute / kg solution

To make a solution, the solute-solute interactions and solvent-solvent interactions must be overcome in endothermic processes

New attractions then form between the solute and solvent particles in an exothermic process

The overall heat of solution is the sum of all the endothermic and exothermic processes needed to form the solution

If the total energy cost for breaking the particles in the pure solute and pure solvent is greater than the energy released in making the new attractions, the overall process will be endothermic

London Dispersion - temporary dipole in the molecules due to unequal electron distribution

Dipole-dipole attractions - permanent polarity in the molecules due to their structure

Hydrogen bonds - especially strong dipole-dipole attraction results when hydrogen is attracted to an extremely electronegative atom, N O F

London Forces << Dipole-dipole << hydrogen bonds << network covalent bonds

Weaker intermolecular forces lead to higher vapor pressure while stronger IMFs lead to lower vapor pressure

Magnitude of the london dispersion forces increases with molar mass

The higher the vapor pressure, the more volatile the liquid

Particles of matter are always in motion

Kinetic Molecular theory:

Collisions of particles with container walls cause pressure exerted by gas

Particles exert no forces on each other

Volume of individual particles is 0

Average kinetic energy is dependent on the Kelvin temperature of a gas

Psolution = Xsolvent * Psolvent