Uploaded October 2018 | Updated September 2026, 14 hours ago
This video explains how to determine the photon wavelength needed to ionize a hydrogen atom. Ionization is described as the complete loss of an electron from an atomic or molecular species.
The most common transitions are (1) the Lyman series in which electrons transition to the ground state (n = 1). This series emits light in the ultraviolet; (2) the Balmer series in which electrons transition to first excited state (n = 2). This series emits light in the visible portion of the spectrum; (3) the Paschen series in which electrons transition to second excited state (n = 3). This series emits light in the infrared portion of the spectrum.
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This video explains how to determine the photon wavelength needed to ionize a hydrogen atom. Ionization is described as the complete loss of an electron from an atomic or molecular species.
The most common transitions are (1) the Lyman series in which electrons transition to the ground state (n = 1). This series emits light in the ultraviolet; (2) the Balmer series in which electrons transition to first excited state (n = 2). This series emits light in the visible portion of the spectrum; (3) the Paschen series in which electrons transition to second excited state (n = 3). This series emits light in the infrared portion of the spectrum.
Link for sharing this video: youtu.be/zRZP96cximk
Support my channel by doing all of the following:
(1) Subscribe, get all my physics, chemistry and math videos
(2) Give me a thumbs up for this video
(3) Leave me a positive comment
(4) Sharing is Caring, share this video with all of your friends
