30 thoughts on “The Bohr Model of the atom and Atomic Emission Spectra: Atomic Structure tutorial | Crash Chemistry

  1. most excellent. informative regarding emission spectra itself and I have not found any decent explanation of the connection between emission spectra and what Neils Bohr did. Thank you so much for your clear explanation here.

  2. I had a problem with this video. When you initially show the electron moving around the nucleus of the Bohr atom, you show various orbits having increasing energies as the electron gets farther from the nucleus. But, the orbital radii you indicate aren't what I remember them being. I think that the electron in the n=2 orbit is supposed to have a radius that is n^2 or 4 times what it is for the n=1 orbit. The electron in the n=4 orbit should then have an orbital radius that is 4^2 or 16 times what it is for the n=1 orbit. I assume that you did this on purpose so that you could show how the differences between total energies for electrons in consecutive orbits gets smaller and smaller as the electrons get farther and farther from the nucleus. I think you should state in the beginning of the video that the orbit radii you indicate are not to scale for this purpose.

    Also, you summarize by stating that electrons do not orbit the nucleus. If that is the case, then how can one rationalize the Zeeman Effect which would seem to require electron motion in order for an externally applied magnetic field to alter the orbits of the moving electrons and thereby slightly alter their energy levels so as to distort the atomic spectra of the elements.

  3. Thanks for the clarity. Lot's of good information, well explained. It gave me a "aha!" moment, trying to understand the transition from earlier models of the atom to the quantum mechanical model.

  4. Great! In class I had totally missed how Bohr was connected to emission spectra. This is a perfect explanation.

  5. Excellent and beautiful video.
    I suggest you see some interesting videos on SALEH THEORY-com about behaviors of photon.

  6. This video should be viewed by all students of the school. In fact this video summarizes all the works of ancient science. thank you again

  7. Great video as many have said. I have a question which may show my ignorance. If hydrogen has just one electron jumping from one level to the next, eg n3 to n2 how can it produce different colours in its emission spectra. Surely that would require several electrons jumping around. Can anyone explain this for me?
    Adrian

Leave a Reply

Your email address will not be published. Required fields are marked *