Question

Although the Bohr model was very successful in accounting for the line spectrum of hydrogen, from what limitations did it suffer? It failed to predict the line spectrum for multi-electron atoms. It incorrectly proposed that electrons could reside between orbital's. It only accurately predicted the visible series of lines in the line spectra of atoms, but not the ultraviolet or infrared series. It incorrectly proposed that electrons move in fixed, defined orbits. It did not explain the quantized nature of the orbital energy levels in an atom. Match the principal and angular-momentum quantum numbers below with their appropriate orbital notation. n = 2, t = 0 1s n = 2, t = 1. 2s n = 1, t = 02p n = 3, t = 2 3d n = 2, t = 2 n and i combination not possible

Answer 1

1. limitations of Bohr theory: ans: A

It does not explain the spectra of multi- electron atoms. Bohr theory does not explain the fine spectra of even the hydrogen atom.

It does not explain the splitting of spectral lines into a group of finer lines under the influence of magnetic feild and electric field.

2. For 1s orbital , n=1,l=0

2s orbiatl n=2, l=0

2p orbiatl , n=2, l=1

3d orbiatl , n=3,l=2

n=1, l=1 combination not possible because l= (n-1)