The electron shell closest to the nucleus, also known as the first shell (n=1) or the K shell, has the lowest energy.
This is because electrons in this shell experience the strongest electrostatic attraction to the positively charged nucleus. The closer an electron is to the nucleus, the lower its potential energy. As you move to electron shells further from the nucleus (n=2, n=3, etc.), the electrons have higher energy levels.
Here's a breakdown of the relationship between electron shells and energy:
- Shell Number (n): Represents the energy level. Higher 'n' means higher energy.
- Shell Name: (K, L, M, N, etc.). K shell corresponds to n=1, L shell to n=2, and so on.
- Energy Level: The energy of an electron increases as it moves to shells further from the nucleus.
| Shell Number (n) | Shell Name | Relative Energy Level |
|---|---|---|
| 1 | K | Lowest |
| 2 | L | Higher |
| 3 | M | Even Higher |
| 4 | N | Still Higher |
In summary, the K shell (n=1), being the closest to the nucleus, has the lowest energy level for electrons.
