Intermolecular Forces - AP Chemistry Unit 3

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Intramolecular Forces

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40 Terms

1

Intramolecular Forces

Forces within a molecule, such as covalent bonds.

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2

Intermolecular Forces (IMFs)

Forces between molecules, which are much weaker than intramolecular forces.

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3

Polarizability

The ability of a molecule to form instantaneous temporary dipoles; larger electron clouds lead to higher polarizability.

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4

London Dispersion Forces (LDFs)

The weakest type of IMF that exists between all molecules with electrons, more notable in non-polar covalent molecules.

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5

Dipole-Dipole Forces

Forces that exist between polar molecules due to an uneven distribution of charge.

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6

Hydrogen Bonding

A stronger type of dipole-dipole attraction that occurs when hydrogen is bonded to nitrogen, oxygen, or fluorine.

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7

Ion-Dipole Forces

Forces that occur when ions are attracted to the oppositely charged dipoles of a polar molecule.

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8

Molecular Solids

Solids formed from molecules, held together by IMFs, with low melting points and not electrically conductive.

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9

Covalent Network Solids

Solids formed from atoms held together by covalent bonds, having the highest melting points.

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10

Ionic Solids

Solids formed from cations and anions held together by lattice energy, which are soluble in water.

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11

Metallic Solids

Solids formed from metals, held together by a sea of electrons, and always electrically conductive.

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12

Viscosity

The resistance to flow in liquids; related to the ease with which individual molecules can flow.

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13

Surface Tension

A measurement of inward forces that must be overcome to break the surface of a liquid.

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14

Capillary Action

The tendency of liquids to climb narrow tubes driven by adhesion and cohesion.

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15

Meniscus

The curvature that exists at the surface of a liquid due to surface tension.

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16

Vapor Pressure

The pressure that develops in the gas phase when a liquid is placed in a closed container.

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17

Volatility

The ability of a substance to turn into a gas; related to vapor pressure.

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18

Homogeneous Mixture

A mixture in which one substance is dissolved in another, such as seawater.

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19

Dilution Equation

M1V1 = M2V2; used for calculating concentrations when mixing solutions.

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20

Beer's Law

A = abc; describes the relationship between absorbance and concentration in solutions.

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21

Distillation

The process of separating substances based on differences in boiling points.

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22

Filtration

The process of separating solids from liquids using a porous membrane.

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23

Chromatography

A technique for separating components of a mixture based on their relative polarities.

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24

Ideal Gas Law

The equation PV = nRT that relates pressure, volume, temperature, and amount of gas.

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25

Boyle’s Law

P1V1 = P2V2; describes the relationship between pressure and volume.

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26

Charles’ Law

V1/T1 = V2/T2; describes the relationship between volume and temperature.

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27

Gay-Lussac’s Law

P1/T1 = P2/T2; describes the relationship between pressure and temperature.

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28

Dalton’s Law of Partial Pressures

States that the total pressure is equal to the sum of the partial pressures of individual gases.

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29

Graham’s Law of Diffusion

States that heavier gases diffuse slower than lighter gases.

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30

Kinetic Molecular Theory

A model that explains the behavior of ideal gases and their properties.

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31

Maxwell-Boltzmann Diagrams

Probability distributions that describe the speed or energy of gas particles.

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32

Triple Point

The condition at which solid, liquid, and gas phases exist in equilibrium.

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33

Aqueous Solution

A solution in which water is the solvent.

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34

Molarity (M)

A measure of concentration calculated as moles of solute divided by liters of solution.

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35

Factors Affecting Vapor Pressure

Including IMFs, temperature, and molar mass; increased temperature usually increases vapor pressure.

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36

IMFs and Physical Properties

As IMFs increase, molecules stick together more, affecting boiling points and melting points.

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37

Allotropes

Different forms of an element in the same physical state, such as graphite and diamond.

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38

Kinetic Energy and Temperature

As temperature increases, so does the kinetic energy of particles.

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39

Pressure and Volume Relationship

The presence of extra gases does not change the volume of a rigid container.

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40

Real vs. Ideal Gases

Real gases have volume and intermolecular forces; ideal gases do not.

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