Chapter 3: Limitations of Bohr's Theory

Question 1

Limitation 1

Answer 1

Bohr’s theory worked perfectly to explain the emission line spectrum of hydrogen. However when his theory was applied to atoms with more than one electron, it failed to account for many lines in the emission spectra of these atoms.

Question 2

Limitation 2

Answer 2

Bohr’s theory did not take into account the fact that the electron had a wave motion. Therefore the picture of an electron travelling in a precise path at a precise distance from the nucleus cannot be true.

Question 3

Limitation 3

Answer 3

Heisenberg’s Uncertainty principle is in conflict with Bohr’s theory. We can only refer to the probability of finding an electron in a region of space.

Question 4

Limitation 4

Answer 4

Bohr’s theory could not explain the splitting of certain lines in the emission spectra and did not take into account the presence of sublevels.