Bohr's model of the atom is a system consisting of a small, dense nucleus surrounded by orbiting electrons. How does Bohr's model explain spectral emission lines? Bohr developed a formula (shown below) that predicted the wavelength of a photon given off when an electron moves from one orbit to another orbit. His formula worked well to explain spectral emission lines in the hydrogen atom. Calculate the wavelength of light that would be emitted for the orbital transition of n = 2 to n = 1. Submit an answer to four significant figures tial R= 1.09678 x 107 m

Bohr's model of the atom is a system consisting of a small, dense nucleus surrounded by orbiting electrons. How does Bohr's model explain spectral emission lines? Bohr developed a formula (shown below) that predicted the wavelength of a photon given off when an electron moves from one orbit to another orbit. His formula worked well to explain spectral emission lines in the hydrogen atom. Calculate the wavelength of light that would be emitted for the orbital transition of n = 2 to n = 1. Submit an answer to four significant figures tial R= 1.09678 x 107 m

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

Section: Chapter Questions

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

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9. An electron in the hydrogen atom relaxes to the n =2 orbit and 434 nm light is emitted. What was the initial orbit of the electron? A: 5 Me g ou counoe
The Balmer series provided the clue to the structure of the hydrogen atom, the simplest atom with only one electron. From that we learned about the structure of all atoms, even those more complex than uranium with its 92 electrons, the heaviest of the natural elements. This series ends on the lowest energy state with n=2 and starts with any state above it. The first line of the Balmer series arises when the atom changes from a state with n=3 to one with n=2. The second line comes from the change from n=4 to n=2, and so on. 3. Suppose that you could measure accurately the wavelengths of the first two lines of the Balmer series. How could you use those measurements to predict the wavelength of the first line of the Paschen series, the ones ending on n=3? This is the method by which we measure the energy levels of atoms experimentally.
An energy of 353 kJ/mol is required to cause a magnesium atom on the metal's surface to lose an electron. Calculate the lowest frequency of light that can ionize a magnesium atom.
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2. What is the wavelength of light emitted when an electron in a hydrogen atom transitions from the n=5 to the n= 3 level?
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The electron in an (unbound) hydrogen atom (H(g)) is excited from the ground state to the n=3 state.Which of the following statements are true and which are false. 1. it takes less energy to ionize the electron from n=3 than it does from the ground state.2. The wavelength of the light emitted when the electron returns to the ground state from n=3 is the same as the wavelength of light absorbed to go from n=1 to n=3.3. the electron is farther from the nucleus on average in the n=3 state than in the ground state.4. The first excited state corresponds to n=3.5. The wavelength of light emitted when the electron drops from n=3 to n=2 is shorter than the wavelength of light emitted if the electron falls from n=3 to n=1.
The energy E of the electron in a hydrogen atom can be calculated from the Bohr formula: R. E In this equation R, 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 emission line spectrum of hydrogen caused by the transition of the electron from an orbital with n=5 to an orbital with n 2. Round your answer to 3 signiticant digits. Tim