* Energy Levels: Electrons in an atom can only occupy specific energy levels, like steps on a ladder. These levels are quantized, meaning they have discrete values.
* Excited State: When an electron absorbs energy (e.g., from heat, light, or an electrical current), it jumps to a higher energy level. This is called an "excited state."
* Returning to Ground State: The excited state is unstable. The electron wants to return to its lowest energy level (ground state).
* Photon Emission: To return, the electron releases the excess energy as a photon of light. The specific energy of the photon corresponds to the energy difference between the two energy levels.
Here's a simple analogy: Imagine a ball rolling down a staircase. As it falls from a higher step to a lower step, it releases energy in the form of sound. Similarly, an electron "falling" from a higher energy level to a lower one releases energy as light.
The color of the light emitted depends on the energy difference between the levels. Higher energy differences result in shorter wavelengths (blue, violet) and lower differences result in longer wavelengths (red, orange).
