According to Bohr, electrons revolve:
- AOption (a)
in fixed circular orbits called shells
- BOption (b)
inside the nucleus of an atom
- COption (c)
only when energy is absorbed
- DOption (d)
in elliptical orbits randomly
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Correct answer
in fixed circular orbits called shells
Why this answer is correct
The correct answer is in fixed circular orbits called shells.
Key Points
- In 1913, Niels Bohr proposed a model for the atom that modified Rutherford’s earlier model to explain why atoms are stable and why they emit specific frequencies of light.
- According to Bohr’s theory, electrons revolve around the nucleus in certain discrete orbits. These orbits are circular and have a fixed radius and fixed energy associated with them.
- These discrete orbits are known as stationary states, energy levels, or shells. Hence, statement 1 is correct.
- Bohr postulated that while an electron is revolving in these fixed orbits, it does not radiate energy, which prevents it from spiraling into the nucleus.
- Electrons do not exist inside the nucleus; the nucleus is composed of protons and neutrons, while electrons occupy the space around it. Hence, statement 2 is incorrect.
- Electrons revolve continuously in these orbits; they absorb energy only to jump to a higher energy level (excitation) and emit energy when falling to a lower level. They do not require constant absorption of energy just to maintain their revolution. Hence, statement 3 is incorrect.
- Bohr's model specifically described circular orbits. The concept of elliptical orbits was later introduced by Arnold Sommerfeld to explain the fine structure of spectral lines. Hence, statement 4 is incorrect.
Additional Information
- Designation of Shells: The energy levels or shells are represented by the letters K, L, M, N or by the principal quantum number n = 1, 2, 3, 4. The K-shell (n=1) is the one closest to the nucleus and possesses the lowest energy.
- Bohr-Bury Scheme: This scheme determines the distribution of electrons in different shells. The maximum number of electrons that can be accommodated in any shell is given by the formula 2n². For instance, the M-shell (n=3) can hold a maximum of 18 electrons.
- Stability of the Atom: Bohr’s model solved the primary flaw of Rutherford’s atomic model, which suggested that accelerating electrons should continuously lose energy and eventually collapse into the nucleus. Bohr’s stationary orbit concept ensured atomic stability.
- Quantization of Energy: A fundamental aspect of Bohr's model is that the angular momentum of an electron is quantized. It can only be an integral multiple of h/2π, where h is Planck’s constant.
Important Points
- Hydrogen Spectrum: Bohr’s model was highly successful in explaining the line spectra of the hydrogen atom and hydrogen-like ions (such as He+ or Li2+). It predicted the wavelengths of light emitted during electron transitions between shells.
- Valence Electrons: The electrons present in the outermost shell of an atom are called valence electrons. These electrons determine the chemical properties and valency of the element.
- Limitations of the Bohr Model: While a major milestone, the model could not explain the Zeeman effect (splitting of spectral lines in a magnetic field) or the Stark effect (splitting in an electric field). It also failed to account for the wave-particle duality of matter and the Heisenberg Uncertainty Principle.