Question

In the Bohr model of hydrogen atom, the angular momentum of the electron is:

• A. Quantized as multiples of \( h \)
• B. Continuous
• C. Quantized as multiples of \( \frac{h}{2\pi} \)
• D. Equal to zero

Hint:

In Bohr's model, angular momentum is quantized:
\[ L = n \cdot \frac{h}{2\pi} = n\hbar \] This was key in explaining the discrete energy levels in atoms.

Answer 1

The Correct Option is C

Per Bohr's quantization rule, an electron's angular momentum in a hydrogen atom is restricted to discrete values. This implies the electron is limited to specific energy levels.
Bohr's postulate states:
\[ L = n \cdot \frac{h}{2\pi} \quad \text{where } n = 1, 2, 3, \dots \] Consequently, the angular momentum is not arbitrary; it is an integer multiple of \( \frac{h}{2\pi} \), not \( h \).
Reasons for excluding other possibilities:
- (A) Quantized as multiples of \( h \): incorrect; the correct form is \( \frac{h}{2\pi} \).
- (B) Continuous: Bohr’s model fundamentally asserts quantization.
- (D) Equal to zero: inaccurate; the ground state exhibits non-zero angular momentum.