AP Chemistry Chapter 3 Exam

INTRAmolecular Forces

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 ______