Rutherford's atomic model was unstable because

Options

A. nuclei will break down
B. electrons do not remain in orbit
C. orbiting electrons radiate energy
D. electrons are repelled by the nucleus

Explanation

**Step-by-Step Solution:**

1. **Understanding Rutherford's Atomic Model**:
- Rutherford proposed a model of the atom where a small, dense nucleus is surrounded by electrons that revolve around it, similar to planets orbiting the sun.

2. **Identifying the Instability**:
- The instability of Rutherford's atomic model arises from the behavior of electrons in orbit around the nucleus.

3. **Electrons in Orbit**:
- In classical physics, an electron moving in a circular orbit is considered to be accelerating due to its change in direction. According to Maxwell's equations, an accelerating charge emits radiation.

4. **Radiation of Energy**:
- As the electrons orbit the nucleus, they would continuously lose energy in the form of electromagnetic radiation. This loss of energy would cause the electrons to spiral inward towards the nucleus.

5. **Consequences of Energy Loss**:
- If the electrons lose energy, they would eventually collapse into the nucleus, leading to an unstable atomic structure. This is a significant flaw in Rutherford's model.

6. **Conclusion**:
- Therefore, Rutherford's atomic model was deemed unstable because it could not account for the continuous radiation of energy by orbiting electrons, leading to their eventual collapse into the nucleus.