In the Bohr model of the atom, electrons are assumed to orbit the nucleus in discrete energy levels or orbits. When an electron undergoes a transition between these orbits, certain phenomena occur.
According to the Bohr model, electrons can only exist in specific quantized energy levels. The energy of an electron in a particular orbit is given by the formula:
E = (-13.6 eV) * (Z^2 / n^2),
where E is the energy, Z is the atomic number (number of protons in the nucleus), and n is the principal quantum number representing the orbit.
When an electron transitions between orbits, it either absorbs or emits energy in the form of electromagnetic radiation. There are two types of transitions:
Absorption: When an electron absorbs energy from an external source, it can move to a higher energy level. This absorption of energy causes the electron to jump from a lower orbit (with lower energy) to a higher orbit (with higher energy). The absorbed energy corresponds to the energy difference between the two orbits according to the formula mentioned earlier. This absorbed energy can come in the form of photons with specific wavelengths or frequencies.
Emission: When an electron returns to a lower energy level from a higher energy level, it releases energy in the form of electromagnetic radiation. This emitted energy corresponds to the energy difference between the two orbits. The emitted radiation can have specific wavelengths or frequencies determined by the energy difference.
These transitions between orbits are often observed as spectral lines in the electromagnetic spectrum. Each spectral line corresponds to a specific energy transition, and different elements have unique sets of spectral lines due to their specific electron configurations.
It's worth noting that the Bohr model is a simplified representation of atomic structure and has limitations. It doesn't fully account for the wave-like nature of electrons and the complexities of quantum mechanics. However, it provides a useful framework for understanding the basic principles of energy transitions in atoms.