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A hydrogen atom with an electron in its ground state interacts with a photon of light with a wavelength of 1.22 × 10^?6m. Could the electron make a transition from the ground state to a higher energy level? If it does make a transition, indicate which one. If no transition can occur, explain.

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Nestor Rutherford
Nestor RutherfordLv2
5 Aug 2019

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Related questions

3e) If an electron in the ground state of hydrogen absorbed a photon of light that has an energy of 1000 kJ, will the electron make an energy transition? Explain why or why not.

3f) Identify the energy of a photon in kJ that would result in the transition of an electron from the ground state to the n=5 energy level?

3g) If an electron makes a transition from any energy level n³3 and drops to the energy level n=2, identify its hydrogen emission series and its electromagnetic range.

Hydrogen Emission Series Name

Electromagnetic Range Name

3h) Why are the Lyman and Paschen Series in the hydrogen emission spectrum not observable with visual senses or the spectroscope?

3i) Why does it appear that there is a continuous band of color in the emission spectrum of multi-electron atoms such as mercury.

Need help with whole question!! A & B please!

In the Balmer series of the hydrogen atom, an electron makes a transition from some higher state to the n = 2 shell. Suppose the initial state of the electron is n = 4. (A) Calculate the energy of the emitted photon for this transition. _____ eV. (B) Find the wavelength of the photon. To save time and effort, remember that a photon's wavelength is &lambda = hc/E = (1240 eV-nm)/E. _____ nm.

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