Although the Bohr model was very successful in accounting for the line spectrum

Question

Although the Bohr model was very successful in accounting for the line spectrum of hydrogen, from what limitations did it suffer? (you can choose more than one)

a. It failed to predict the line spectrum for multi-electron atoms.

b. It incorrectly proposed that electrons could reside between orbitals.

c. It only accurately predicted the visible series of lines in the line spectra of atoms, but not the ultraviolet or infrared series.

d. It incorrectly proposed that electrons move in fixed, defined orbits.

e. It did not explain the quantized nature of the orbital energy levels in an atom.

*I think it is A forsure but still wondering if it is also B and C.

a. It failed to predict the line spectrum for multi-electron atoms.

b. It incorrectly proposed that electrons could reside between orbitals.

c. It only accurately predicted the visible series of lines in the line spectra of atoms, but not the ultraviolet or infrared series.

d. It incorrectly proposed that electrons move in fixed, defined orbits.

e. It did not explain the quantized nature of the orbital energy levels in an atom.

Explanation / Answer

a. It failed to predict the line spectrum for multi-electron atoms.

Bohr's theory successfuly explain one electron contains hydrogen spectrum. It does not explain more than electron containing atoms and anion spectrum.

Bohr's does not explain fine spectrum.

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