According to Bohr's model of an elements

Options

A. `mvr = mh//2pi`
B. `mvr = 2pi//nh`
C. `mvr=n^(2)h^(2)//2pi^(2)`
D. `mvr^(2)=(nh)/pi`

Explanation

**Step-by-Step Solution:**

1. **Understanding Bohr's Model**: Bohr's model describes the behavior of electrons in an atom. It proposes that electrons move in specific orbits around the nucleus, and these orbits are quantized.

2. **Quantization of Angular Momentum**: According to Bohr, the angular momentum (L) of an electron in a given orbit is quantized. This means that the angular momentum can only take on certain discrete values.

3. **Angular Momentum Formula**: The formula for the angular momentum of an electron in orbit is given by:
\[ L = mvr = n \frac{h}{2\pi} \]
where:
- \(L\) is the angular momentum,
- \(m\) is the mass of the electron,
- \(v\) is the velocity of the electron,
- \(r\) is the radius of the orbit,
- \(n\) is a positive integer (1, 2, 3, ...), known as the principal quantum number,
- \(h\) is Planck's constant.

4. **Integral Multiples**: The equation indicates that the angular momentum of the electron can only be an integral multiple of \(\frac{h}{2\pi}\). This means that the electron can only occupy certain allowed orbits where its angular momentum is quantized.

5. **Conclusion**: Therefore, according to Bohr's model, the correct statement is that the angular momentum of the electron is quantized and can be expressed as \(mvr = n \frac{h}{2\pi}\).

**Final Answer**: The angular momentum of the electron in Bohr's model is quantized and given by the formula \(mvr = n \frac{h}{2\pi}\).

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