The Bohr model of the atom fails to explain the observed emission spectrum for a

Question

The Bohr model of the atom fails to explain the observed emission spectrum for atoms of elements with more than one electron (i.e. other than H, He^+, Li^2+, etc.) because: a) it incorrectly predicted that electrons should emit or absorb photons of any energy b) it only allows electrons to occupy certain discrete energy levels around the nucleus c) it incorrectly treats electrons as particles circling the nucleus and not as probability distributions d) it incorrectly treats the electron energy levels as continuous and not quantized e) it incorrectly assumed that electrons could not be "excited" into higher energy levels

Explanation / Answer

C) It incorrectly treats electrons as particles circling the nucles and not as propability distributions. Thus it violating Heisenberg uncertainity principle

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