In the Bohr model, what happens when an electron makes a transition between orbits?

Atoms are the basic units of matter and consist of a dense nucleus surrounded by a cloud of electrons. The electrons in an atom are not just scattered around the nucleus; they occupy specific regions known as energy levels or shells. These energy levels are like the rungs of a ladder, with each successive level further away from the nucleus holding electrons at progressively higher energies.

In the context of the Bohr model, these energy levels are quantized, which means that an electron cannot exist between the set levels; it must be on one of the rungs. Think of it as being allowed to stand on the first or second step of the ladder but not on the air in between. The energy of each level is represented by the formula: \( E_n = -\frac{R_H}{n^2} \) where \( R_H \) is the Rydberg constant and \( n \) is the principal quantum number, which indicates the energy level's number.

Electron excitation is a process that occurs when an electron inside an atom absorbs energy and jumps from a lower to a higher energy level. This is similar to a person using energy to jump to a higher step on a ladder. In the atom, this energy can come from various sources, such as light (photons) or collisions with other particles.

When an electron is excited, it absorbs a photon with just the right amount of energy to make the transition. This energy must match the difference between the electron's current energy level and the one it is jumping to, obeying the law of conservation of energy. The mathematical form of this energy difference is expressed as \( \Delta E = E_{final} - E_{initial} \) where \( E_{final} \) and \( E_{initial} \) are the energies of the electron in the final and initial levels, respectively. This process is crucial for many phenomena in physics and chemistry, including spectroscopy and the functioning of lasers.

When discussing photons in the context of the Bohr model, we're essentially talking about packets of light energy that electrons can either emit or absorb. These transitions between energy levels within atoms are responsible for the phenomenon of photon emission and absorption.

During photon emission, an electron drops from a higher energy level to a lower one, releasing energy in the form of a photon. The energy of this photon is precisely equal to the energy difference between the two levels. On the other hand, photon absorption happens when an electron gains energy by absorbing a photon, allowing it to move up to a higher energy level. This is what generates the diverse colors we witness in fireworks or neon signs, where each color represents a specific photon energy, thus linking to a unique transition between energy levels. These processes are fundamental to our understanding of atomic behavior and are integral in technologies such as photovoltaic cells and various forms of spectroscopy.