Concept explainers
A hydrogen atom in the ground stale absorbs a photon whose wavelength is 95.0 nm. The resulting excited atom then emits a photon of 1282 nm. What are the regions of the
Interpretation:
The principal quantum number of level from the emission of excited atom has to be calculated.
Concept introduction:
Bohr developed a rule for quantization of energy that could be applicable to the electron of an atom in motion. By using this he derived a formula for energy levels of electron in H-atom.
Relation between frequency and wavelength is,
C is the speed of light.
h is Planck’s constant (
E is energy of light particle.
Answer to Problem 7.106QP
The principal quantum number of level from the emission of excited Hydrogen atom is three.
Explanation of Solution
To calculate: The principal quantum number of level from the emission of excited Hydrogen atom.
The level to which
The energy of the UV radiation is calculated as follows,
Absorption occurs and the change in energy is positive.
The excited level of hydrogen atom is five. This excited level by emitting
The energy of the IR radiation is calculated as follows,
Emission occurs and the change in energy is negative.
By using the formula for energy levels of electron in H-atom, the principal quantum number of level from the emission of excited atom was calculated.
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Chapter 7 Solutions
OWLv2 for Ebbing/Gammon's General Chemistry, 11th Edition, [Instant Access], 1 term (6 months)
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