Studied by 9 people
INTRAmolecular Forces
Forces that happen WITHIN a molecule
INTERmolecular Forces
Forces interaction BETWEEN molecules
Dipole-Dipole Interactions
Occurs between two polar molecules
Polar
The more ____ the stronger the interaction
Dipole-Induced Dipoles
When polar molecules can cause nonpolar molecules to have “temporary dipoles” or to “temporarily become polar”
London Dispersion Forces
When temporary dipoles approach another molecules, electrons disperse and create another temporary dipole
(the weakest intermolecular force)
Hydrogen Bonding
The strongest intermolecular force, occurs between hydrogen and highly electronegative atoms (N, O, F)
Nitrogen, Oxygen, Fluorine (NOF)
The 3 atoms that hydrogen bonding works with
Ion-Dipole Interaction
Interactions even stronger than hydrogen bonding
Melting/boiling point, vapor pressure, volatitlity, surface tension, viscosity, heat of vaporization
Properties that can be explained by Intermolecular forces
Melting/boiling point, surface tension, viscosity, heat of vaporization
Properties that INCREASE as IMF INCREASE (direct relationship)
Vapor pressure, Volatility (ease of evaporating)
Properties that DECREASE as IMF INCREASES
Ionic, Molecular, Metallic, Covalent Network
The 4 types of solids
Ionic Solids
Solids formed by a metal and a nonmetal
High melting/boiling point, brittle, poor conductors of electricity in solid but good in liquid
Properties of Ionic solids
Molecular Solids
Solids formed by 2 or more nonmetals
Neutral, form lattice structures, low melting/boiling point, poor conductors of electricity in all states
Properties of molecular solids
Covalent Network Solids
Solids formed by carbon and semimetals
High melting/boiling point and hardness, poor conductors of electricity
Properties of Covalent Network Solids
Metallic Solids
Solids formed by metallic elements (only metals)
Great conductors of electricity and heat, malleable and ductile, melting points varyS
Properties of Metallic Solids
Crystalline Solids
Solids in which particles are arranged in a regular, repeating pattern
Amorphous Solids
Solids in which particles that are randomly arranged
PV=NRT
Ideal Gas Law
P1V1=P2V2
Boyle’s Law
Decreases
As volume increases, pressure _____
Increases
As moles increase, pressure _______
Increases
As pressure increases, temperature _________
Increases
As temperature increases, volume ________
Pressure is low and temperature is high
Gases are most ideal when….
Ptotal= Pa + Pb + Pc + ….
Dalton’s Law of Partial Pressure
-All particles are in continous, random motion
-Between collisions articles have constant velocity and direction
-After collisions particles have new velocity and direction
-Elastic collisions
Kinetic Molecular Theory
Temperature
Measure of average kinetic energy
KE= ½ MV²
Kinetic Energy Equation
Squeeze togetheer
In a Maxwell-Botlzmann graph, when it moves to the left it must _______
Smash down
In a Maxwell-Botlzmann graph, when it moves to the right it must _______
M/L
Molarity Equation
M1V1=M2V2
Dilution Equation
Column chromatography
The best form of chromatography
Solute
The stationary phase is the ______
Solvent
The mobile phase is the _______
Distillation
A process that involves using vapor and separating substances by boiling point
Polar & Ionic
Polar dissolves ________
Nonpolar
Nonpolar dissolves ______
Spectroscopy
The study of matter’s interactions with electromagnetic radiation
Molecular rotation
Microwave radiation is associated with ______
Molecular vibration
Infrared Radiation is associated with ________
Molecular transitions
Ultraviolet/Visible radiation is associated with ______
A = Ebc
Beer lambert law Equation
Absorbance
The “A” in Beer-Lambert Law stands for _____
Molar absorptivity
The “E” in Beer-Lambert Law stands for _______
Path length
The “b” in Beer-Lambert Law stands for ______
Concentration
The “c” in Beer-Lambert Law stands for ______
