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 The exact position and momentum of an electron cannot be determined simultaneously is: a) the Pauli exclusion principle b) Lewis's rule d) Hund's rule e) the Heisenberg uncertainty principle

Explanation / Answer

Bhor atom model

1. The electron in an atoms revolve around the nucleus only in a certain circular orbits. It neither lost nor gain the energy

2. The energy of an electron can't change continuously. That is the electron has to jump not to flow from one energy lever to another.

3 angular momentum of electron is quantised

It's fail to explain atomic spectra of many electron atoms. Because it incorrectly predicted that it can absorb or emit of any engery. Not considering Pauli's priciple

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