AP Chemistry Unit 3

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27 Terms

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London Dispersion Forces

  • Weakest

  • Found in all molecules

  • More electrons = more polarizable = stronger LDF

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Dipole-Dipole Forces

  • Moderate Strength

  • Found in Polar Molecules Only

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Hydrogen Bonds

  • Strongest

  • O-H, N-H, F-H

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Ionic Solids

  • High Melting Point

  • Brittle

  • Conduct Electricity when dissolved in water

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Covalent Network Solids

  • Highest melting point

  • Extremely high hardness

  • Strongest covalent forces

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Molecular Solids

  • Low melting points

  • Weak IMFs

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Metallic Solids

  • Sea of Electrons

  • Excellent conductor

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Ideal Gas Law

PV = nRT

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Pressure Gas Equations

Pgas = Xgas * Ptotal
Ptotal = Pgas1 + Pgas2 + …

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Pressure vs Volume

Exponentially Decreases

<p>Exponentially Decreases</p>
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Volume vs Temperature

Linearly Increases

<p>Linearly Increases</p>
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Pressure vs Temperature

Linearly Increases

<p>Linearly Increases</p>
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Volume vs Number of Moles

Linearly Increases

<p>Linearly Increases</p>
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Boltzmann Distribution Curve

At high temperatures, more molecules have greater velocity and, thus, greater kinetic energy

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Ideal conditions for real gases

  • High Temperature

  • Low Pressure

  • Very small molecule sometimes

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Heterogeneous Mixtures

Different sections are visible to the naked eye

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Homogeneous Mixture

  • Called solutions

  • Uniform composition throughout

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Molarity

M = Moles/Liters

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Like Dissolves Like

Polar Molecules dissolve in Polar Solvents

nonPolar Molecules dissolve in nonPolar Solvents

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UV or visible light

Causes electrons to transition to different energy levels

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Infrared Radiation

Causes molecules to vibrate

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Microwave Radiation

Causes molecules to rotate

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Wavelength & Frequency

c = λν
c = speed of light (2.998 × 10^8 m/s)

λ = wavelength in meters

v = Frequency in waves cycles per second

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Energy of a Photon

E = hv

E= Energy of a photon

h = Plancks Constant (6.626 × 10^34 Js)
v = Frequency in waves cycles per second

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Beer-Lambert Law

A = εbc
A = Abosrbance
ε = molar absorptivity
b = Path length of cuvette (Usually 1cm)
c = Concentration of the solution

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High Outliers

Caused by contamination from solution of higher concentration

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Low Outlier

Caused by Contamination from water or a solution of lower concentration