The following are possible energy values for the electron orbiting the nucleus in Bohr’s model for the hydrogen atom. n = 1: E1 = -21.79 x 10–19 J; n = 2: E2 = - 5.45 x 10–19 J; n = 3: E3 = - 2.42 x 10–19 J; n = 4: E4 = - 1.36 x 10–19 J;If an electron jumps from the orbit n = 4 to orbit n = 2, and a quantum of energy is emitted in the form of light, what is the wavelength of the emitted light in nm? (A) 365 nm (B) 486 nm (C) 1095 nm (D) 1460 nm

Name: The following are possible energy values for the electron orbiting the
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Description: The following are possible energy values for the electron orbiting the nucleus in Bohr’s model for the hydrogen atom. n = 1: E1 = -21.79 x 10–19 J; n = 2: E2 = - 5.45 x 10–19 J; n = 3: E3 = - 2.42 x 10–19 J; n = 4: E4 = - 1.36

Given: Electron transition is from n=4 to n=2, E4 =- 1.36 x10-19JE2 = - 5.45 x 10-19J

Answered: The following are possible energy…

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

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Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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The following are possible energy values for the electron orbiting the nucleus in Bohr’s model for the hydrogen atom.

n = 1: E₁ = -21.79 x 10^–19 J;

n = 2: E₂ = - 5.45 x 10^–19 J;

n = 3: E₃ = - 2.42 x 10^–19 J;

n = 4: E₄ = - 1.36 x 10^–19 J;

If an electron jumps from the orbit n = 4 to orbit n = 2, and a quantum of energy is emitted in the form of light, what is the wavelength of the emitted light in nm?

(A) 365 nm

(B) 486 nm

(D) 1460 nm

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