Bohr's atom model is the modification of Rutherford's atom model by the application of

Options

A. Newtons theory
B. Huygen's theory
C. Maxwell's theory
D. Planck's quantum theory

Answer

**Step-by-Step Solution:**

1. **Understanding Rutherford's Model:**
- Rutherford's model proposed that an atom consists of a dense nucleus surrounded by electrons, similar to planets orbiting the sun. However, it had limitations, particularly regarding electron stability and energy dissipation.

2. **Introduction of Bohr's Model:**
- Niels Bohr modified Rutherford's model by introducing the concept of quantized orbits for electrons. He proposed that electrons can only occupy certain stable orbits without radiating energy.

3. **Stationary Orbits:**
- Bohr referred to these stable orbits as stationary orbits. In these orbits, electrons do not lose energy, which was a significant deviation from Rutherford's model, where electrons were expected to spiral into the nucleus due to energy loss.

4. **Conservation of Angular Momentum:**
- Bohr applied the principle of conservation of angular momentum to explain the stability of these orbits. He stated that the angular momentum of an electron in a stationary orbit is quantized and can be expressed as:
\[ mvr = n\frac{h}{2\pi} \]
- Here, \(m\) is the mass of the electron, \(v\) is its velocity, \(r\) is the radius of the orbit, \(n\) is a positive integer (quantum number), and \(h\) is Planck's constant.

5. **Energy Levels and Photon Emission:**
- Bohr's model also introduced the concept of energy levels. When an electron transitions between these energy levels, it absorbs or emits energy in the form of photons. This explained the spectral lines observed in hydrogen and other elements.

6. **Conclusion:**
- Thus, Bohr's atom model is a modification of Rutherford's atom model by the application of quantized orbits and the conservation of angular momentum, which allowed for stable electron configurations without energy dissipation.

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