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42 solutions

Bohr and Balmer Equations

Q. An electron in the n = 7 level of the hydrogen atom relaxes to a lower energy level, emitting light of 397 nm. What is the value of n for the level to which the electron relaxed?

Solved • Dec 2, 2019

Bohr and Balmer Equations

Q. The energy E of the electron in a hydrogen atom can be calculated from the Bohr formula: =E−Ryn2 In this equation Ry stands for the Rydberg energy, and n stands for the principal quantum number of the orbital that holds the electron. (You can find the value of the Rydberg energy using the Data button on the ALEKS toolbar.) Calculate the wavelength of the line in the absorption line spectrum of hydrogen caused by the transition of the electron from an orbital with =n7 to an orbital with =n10. Rou

Solved • Nov 26, 2019

Bohr and Balmer Equations

Q. a gamma-ray of wavelength 1.00 x10^-8 cm has enough energy to remove an electron from a hydrogen atom. True or False?

Solved • Nov 25, 2019

Bohr and Balmer Equations

Q. 19. It is the amount of energy that an electron gains when subjected to a potential of 1 volt; 1 eV = 1.602 × 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 calculations.

Solved • Nov 13, 2019

Bohr and Balmer Equations

Q. Use the Rydberg equation to calculate the wavelength (in Å) of the photon absorbed when a hydrogen atom undergoes a transition from n = 3 to n = 4.

Solved • Oct 26, 2019

Bohr and Balmer Equations

Q. An electron in the n = 5 level of an H atom emits a photon of wavelength 4052.28 nm. To what energy level does the electron move?

Solved • Oct 24, 2019

Bohr and Balmer Equations

Q. Use the Rydberg equation to calculate the wavelength (in Å) of the photon absorbed when a hydrogen atom undergoes a transition from n = 2 to n = 3.

Solved • Oct 24, 2019