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? It failed to predict the line spectrum for multi-electron atoms. It incorrectly proposed that electrons could reside between orbitals 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 on atom. Match the principal and angular momentum quantum numbers below with their appropriate orbital notation.

Explanation / Answer

Limitations Of Bohr Atomic model:

1)It is applicable for H-like atoms only(H,He+,Li+2,Be+3).

2)It is not applicable for multi electron atoms

3)It does not explain fine spectrum

4)It does not explain Zeeman stark effect.

(Zeeman effect:The splitting of spectral lines into no of closely spaced lines in presence of magnetic field

Stark effect:The splitting of spectral lines into no of closely spaced lines in presence of electrtic field )

Related Questions

Navigate

• Browse (All)
• Browse A
• Subjects

---

---

Integrity-first tutoring: explanations and feedback only — we do not complete graded work. Learn more.