Bohr Model of the Hydrogen Atom, Electron Transitions, Atomic Energy Levels, Lyman & Balmer Series

This chemistry video tutorial focuses on the bohr model of the hydrogen atom. It explains how to calculate the amount of electron transition energy that is released or absorbed whenever an electron jumps from one atomic energy level to another. The electron transition energy formula / equation helps you to calculate the energy levels of electrons in the hydrogen atom only. This video also explains what is meant by the lyman, balmer and paschen series. The lyman series is associated with UV radiation. The balmer series is associated with the visible light emission spectrum and the paschen series is related to the infrared region of the electromagnetic spectrum. The bracket series and pfund series are part of the IR spectrum as well. This video contains plenty of examples and multiple choice practice problems.
Speed of Light, Frequency, Wavelength:
• Speed of Light, Freque...
Photon Energy:
• How To Calculate The E...
The Photoelectric Effect:
• Photoelectric Effect, ...
De Broglie Wavelength:
• De Broglie Wavelength ...
The Bohr Model of Hydrogen:
• Bohr Model of the Hydr...
Heisenberg's Uncertainty Principle:
• Heisenberg's Uncertain...
________________________________
Intro to Quantum Numbers:
• Quantum Numbers
Orbitals & Atomic Energy Levels:
• Orbitals, Atomic Energ...
Maximum Number of Electrons:
• How To Determine The M...
Intro to Electron Configuration:
• Electron Configuration...
Electron Configuration Exceptions:
• Electron Configuration...
Noble Gas Notation:
• Electron Configuration...
Electron Configuration of Ions:
• Electron Configuration...
_______________________________
Orbital Diagrams:
• Orbital Diagrams and E...
Paired & Unpaired Electrons:
• How To Determine The N...
Aufbau's Principle & Hund's Rule:
• Aufbau's Principle, Hu...
Paramagnetic & Diamagnetic Elements:
• Paramagnetic & Diamagn...
Valence Electrons & Periodic Table:
• Valence Electrons and ...
Effective Nuclear Charge:
• How To Calculate The E...
_________________________________
Slater's Rule:
• How To Use Slater's Ru...
How To Identify The Element:
• Electron Configuration...
Quantum Numbers - Mega Review:
• Quantum Numbers - n, l...
Quantum Numbers - Practice Test:
• Orbitals, Quantum Numb...
Final Exams and Video Playlists:
www.video-tuto...
Full-Length Videos and Worksheets:
/ collections

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Your equation was made by Rydberg and you have to use the wavelenght and Rydberg constant for wavelenghts. His equation is Bohr's equation and you use energy and Rydberg's constant for energy. It does the same thing.

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Hello bro Thanks for everything you are doing here ....but with the question u calculated for energy I don't hv no idea of where -2.178 came about , any help?

[@jamesalucas2643]

The 2.178 is the Rydberg’s constant (RH)the reason why it is negative is because the formula for the energy jump-back is E= -RH [1/nf2 - 1/nI2]

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[@ilianettemontanez-cintron4572]

According to my MCAT Kaplan text, the equation requires the final value be subtracted from initial (the opposite of what was done here) and that a positive E corresponds to emission while a negative E corresponds to absorption. Is that incorrect? The solution for E would then be +4 x10^-19J.

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There is a formular and it says that you must substract final from initial. Kaplan might be wrong.

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• If it's an absorption process; the energy of the system would be increased, thus the Energy (E) should be positive, it means that the Final state (nF) - which is the higher energy level - should be bigger than the Initial state (nI) - which is the lower energy level -. If: Energy (E) > 0 Then: Final state (nF) > Initial state (nI) E = -2.178×10^-18 [(1/nF²) - (1/nI²)] E = -2.178×10^-18 [(lesser) - (bigger)] E = -2.178×10^-18 [-value] = +value • If it's an emission process; the energy of the system would be decreased, thus the Energy (E) should be negative, it means that the Initial state (nI) - which is the higher energy level - should be bigger than the Final state (nF) - which is the lower energy level - . If: Energy (E) < 0 Then: Final state (nF) < Initial state (nI) E = -2.178×10^-18 [(1/nF²) - (1/nI²)] E = -2.178×10^-18 [(bigger) - (lesser)] E = -2.178×10^-18 [+value] = -value Advice: it's all about the reciprocal value of the Initial & Final states, it confuses you, try to concentrate, and apply some simple values of the Initial & Final states - like (1) and (2), and vice versa - depending on the process, it will help you understand. Remember: 1. In Emission: the Final state is always lower than the Initial state. Because the electron is falling down. 2. In Absorption: the Final state is always higher than the Initial state. Because the electron is jumping up.

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hi! (i’m honestly so bad at chemistry so sorry if the following questions make no sense or r super simple) great content btw I solved my problem now, but I’ve also got some questions for commenters or you. With both my own chemistry work and this video, it both says hydrogen atom. The second example you gave also didn’t explicitly say hydrogen, but the same formulas were applied, so for these chemistry problems should I automatically assume its hydrogen? And is hydrogen the only one I need to know for highschool chem? Also, why hydrogen? Is it for simplicity?

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