AP Chemistry Chapter 3 Exam

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53 Terms

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INTRAmolecular Forces

Forces that happen WITHIN a molecule

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INTERmolecular Forces

Forces interaction BETWEEN molecules

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Dipole-Dipole Interactions

Occurs between two polar molecules

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Polar

The more ____ the stronger the interaction

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Dipole-Induced Dipoles

When polar molecules can cause nonpolar molecules to have “temporary dipoles” or to “temporarily become polar”

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London Dispersion Forces

When temporary dipoles approach another molecules, electrons disperse and create another temporary dipole
(the weakest intermolecular force)

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Hydrogen Bonding

The strongest intermolecular force, occurs between hydrogen and highly electronegative atoms (N, O, F)

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Nitrogen, Oxygen, Fluorine (NOF)

The 3 atoms that hydrogen bonding works with

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Ion-Dipole Interaction

Interactions even stronger than hydrogen bonding

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Melting/boiling point, vapor pressure, volatitlity, surface tension, viscosity, heat of vaporization

Properties that can be explained by Intermolecular forces

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Melting/boiling point, surface tension, viscosity, heat of vaporization

Properties that INCREASE as IMF INCREASE (direct relationship)

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Vapor pressure, Volatility (ease of evaporating)

Properties that DECREASE as IMF INCREASES

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Ionic, Molecular, Metallic, Covalent Network

The 4 types of solids

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Ionic Solids

Solids formed by a metal and a nonmetal

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High melting/boiling point, brittle, poor conductors of electricity in solid but good in liquid

Properties of Ionic solids

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Molecular Solids

Solids formed by 2 or more nonmetals

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Neutral, form lattice structures, low melting/boiling point, poor conductors of electricity in all states

Properties of molecular solids

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Covalent Network Solids

Solids formed by carbon and semimetals

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High melting/boiling point and hardness, poor conductors of electricity

Properties of Covalent Network Solids

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Metallic Solids

Solids formed by metallic elements (only metals)

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Great conductors of electricity and heat, malleable and ductile, melting points varyS

Properties of Metallic Solids

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Crystalline Solids

Solids in which particles are arranged in a regular, repeating pattern

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Amorphous Solids

Solids in which particles that are randomly arranged

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PV=NRT

Ideal Gas Law

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P1V1=P2V2

Boyle’s Law

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Decreases

As volume increases, pressure _____

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Increases

As moles increase, pressure _______

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Increases

As pressure increases, temperature _________

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Increases

As temperature increases, volume ________

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Pressure is low and temperature is high

Gases are most ideal when….

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Ptotal= Pa + Pb + Pc + ….

Dalton’s Law of Partial Pressure

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-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

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Temperature

Measure of average kinetic energy

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KE= ½ MV²

Kinetic Energy Equation

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Squeeze togetheer

In a Maxwell-Botlzmann graph, when it moves to the left it must _______

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Smash down

In a Maxwell-Botlzmann graph, when it moves to the right it must _______

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M/L

Molarity Equation

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M1V1=M2V2

Dilution Equation

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Column chromatography

The best form of chromatography

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Solute

The stationary phase is the ______

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Solvent

The mobile phase is the _______

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Distillation

A process that involves using vapor and separating substances by boiling point

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Polar & Ionic

Polar dissolves ________

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Nonpolar

Nonpolar dissolves ______

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Spectroscopy

The study of matter’s interactions with electromagnetic radiation

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Molecular rotation

Microwave radiation is associated with ______

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Molecular vibration

Infrared Radiation is associated with ________

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Molecular transitions

Ultraviolet/Visible radiation is associated with ______

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A = Ebc

Beer lambert law Equation

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Absorbance

The “A” in Beer-Lambert Law stands for _____

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Molar absorptivity

The “E” in Beer-Lambert Law stands for _______

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Path length

The “b” in Beer-Lambert Law stands for ______

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Concentration

The “c” in Beer-Lambert Law stands for ______