6.2 The Bohr Model

Quantized orbits for hydrogen's single electron and the Rydberg equation giving the energy of light emitted or absorbed in a jump between levels.

Chemistry 2e, 6.2 The Bohr Model

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7 exercises

6.2 Exercise 2

What does it mean to say that the energy of the electrons in an atom is quantized?

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6.2 Exercise 4

The electron volt (eV) is a convenient unit of energy for expressing atomic-scale energies. It is the amount of energy that an electron gains when subjected to a potential of 1 volt; 1 eV = 1.602 $\times$ 10^–19 J. Using the Bohr model, determine the energy, in electron volts, of the photon produced when an electron in a hydrogen atom moves from the orbit with n = 5 to the orbit with n = 2. Show your calc…

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6.2 Exercise 6

Using the Bohr model, determine the lowest possible energy for the electron in the He⁺ ion.

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6.2 Exercise 8

Using the Bohr model, determine the energy of an electron with n = 8 in a hydrogen atom.

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6.2 Exercise 10

What is the radius, in angstroms, of the orbital of an electron with n = 8 in a hydrogen atom?

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6.2 Exercise 12

Using the Bohr model, determine the energy in joules of the photon produced when an electron in a Li²⁺ ion moves from the orbit with n = 2 to the orbit with n = 1.

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6.2 Exercise 14

How are the Bohr model and the Rutherford model of the atom similar? How are they different?

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