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Ch.7 - Quantum MechanicsWorksheetSee all chapters
All Chapters
Ch.1 - Intro to General Chemistry
Ch.2 - Atoms & Elements
Ch.3 - Chemical Reactions
BONUS: Lab Techniques and Procedures
BONUS: Mathematical Operations and Functions
Ch.4 - Chemical Quantities & Aqueous Reactions
Ch.5 - Gases
Ch.6 - Thermochemistry
Ch.7 - Quantum Mechanics
Ch.8 - Periodic Properties of the Elements
Ch.9 - Bonding & Molecular Structure
Ch.10 - Molecular Shapes & Valence Bond Theory
Ch.11 - Liquids, Solids & Intermolecular Forces
Ch.12 - Solutions
Ch.13 - Chemical Kinetics
Ch.14 - Chemical Equilibrium
Ch.15 - Acid and Base Equilibrium
Ch.16 - Aqueous Equilibrium
Ch.17 - Chemical Thermodynamics
Ch.18 - Electrochemistry
Ch.19 - Nuclear Chemistry
Ch.20 - Organic Chemistry
Ch.22 - Chemistry of the Nonmetals
Ch.23 - Transition Metals and Coordination Compounds
Wavelength and Frequency
Speed of Light
The Energy of Light
Electromagnetic Spectrum
Photoelectric Effect
De Broglie Wavelength
Heisenberg Uncertainty Principle
Bohr Model
Emission Spectrum
Bohr Equation
Introduction to Quantum Mechanics
Quantum Numbers: Principal Quantum Number
Quantum Numbers: Angular Momentum Quantum Number
Quantum Numbers: Magnetic Quantum Number
Quantum Numbers: Spin Quantum Number
Quantum Numbers: Number of Electrons
Quantum Numbers: Nodes

The Energy of Light involves the use of a new variable Planck's Constant.

Light as Particles

Concept #1: The Energy of Light

Concept #2: Photon Energy Formulas

Example #1: Calculate the energy of a photon with a wavelength of 293.7 m.

Concept #3: Moles and Energy

Example #2: Calculate the energy for a mole of photons with a frequency of 4.29 x 1015 s-1.

Practice: Calculate the energy (in nJ) of a photon emitted by a mercury lamp with a frequency of 6.88 x 1014 Hz.

Practice: A light ray has a wavelength that is 835 µm contains 6.32 x 10-3 J of energy. How many photons does this light ray have?

Practice: How much energy (in kJ) do 4.50 moles of photons contain at a wavelength of 705 nm?