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Ch.7 - Quantum MechanicsWorksheetSee all chapters

# Bohr Model

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Sections
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

In the Bohr Model, electrons can move up and down to different orbitals or shells based on absorbing or releasing of energy.

###### Bohr Model

Concept #1: Bohr Model

Example #1: Calculate the energy of an electron found in the second shell of the hydrogen atom.

Concept #2: Absorption and Emission

Practice: Which of the electron transitions represents absorption with the greatest frequency?

Practice: Which of the following transitions (in a hydrogen atom) represent emission of the shortest wavelength?

Practice: If the energy of an electron within the boron atom was calculated as –6.0556 x 10-18 J, at what energy level would it reside?