Photoelectron spectroscopy applies the principle of the photoelectric effect to study orbital energies of atoms and molecules. High-energy radiation (usually UV or X-ray) is absorbed by a sample and an electron is ejected. The orbital energy can be calculated from the known energy of the radiation and the measured energy of the electron lost. The following energy differences were determined for several electron transitions: ΔE2 →1 = 4.098 ×10−17 J ΔE3 →1 = 4.854 × 10−17 J ΔE5 → 1 = 5.242 ×10−17 J ΔE4 → 2 = 1.024 ×10−17 J Calculate the energy change and the wavelength of a photon emitted in the following transitions. Enter your answers in scientific notation. Use 6.626 ×10−34 J·s for Planck's constant. (a) Level 3 to 2: ______J ______m (b) Level 4 to 1: _____J _____ m (c) Level 5 to 4: _____J _____m
Photoelectron spectroscopy applies the principle of the photoelectric effect to study orbital energies of atoms and molecules. High-energy radiation (usually UV or X-ray) is absorbed by a sample and an electron is ejected. The orbital energy can be calculated from the known energy of the radiation and the measured energy of the electron lost. The following energy differences were determined for several electron transitions: ΔE2 →1 = 4.098 ×10−17 J ΔE3 →1 = 4.854 × 10−17 J ΔE5 → 1 = 5.242 ×10−17 J ΔE4 → 2 = 1.024 ×10−17 J Calculate the energy change and the wavelength of a photon emitted in the following transitions. Enter your answers in scientific notation. Use 6.626 ×10−34 J·s for Planck's constant. (a) Level 3 to 2: ______J ______m (b) Level 4 to 1: _____J _____ m (c) Level 5 to 4: _____J _____m
General Chemistry - Standalone book (MindTap Course List)
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Chapter7: Quantum Theory Of The Atom
Section: Chapter Questions
Problem 7.34QP: The following shapes each represent an orbital of an atom in a hypothetical universe. The small...
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Photoelectron spectroscopy applies the principle of the
ΔE2 →1 = 4.098 ×10−17 J
ΔE3 →1 = 4.854 × 10−17 J
ΔE5 → 1 = 5.242 ×10−17 J
ΔE5 → 1 = 5.242 ×10−17 J
ΔE4 → 2 = 1.024 ×10−17 J
Calculate the energy change and the wavelength of a photon emitted in the following transitions. Enter your answers in scientific notation. Use 6.626 ×10−34 J·s for Planck's constant.
(a) Level 3 to 2:
______J
______m
(b) Level 4 to 1:
_____J
_____ m
(c) Level 5 to 4:
_____J
Calculate the energy change and the wavelength of a photon emitted in the following transitions. Enter your answers in scientific notation. Use 6.626 ×10−34 J·s for Planck's constant.
(a) Level 3 to 2:
______J
______m
(b) Level 4 to 1:
_____J
_____ m
(c) Level 5 to 4:
_____J
_____m
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