The Bohr Model, proposed by Niels Bohr in 1913, revolutionized our understanding of atomic structure. This model describes the arrangement of electrons in an atom as occupying specific energy levels or electron orbits. According to Bohr, electrons can only exist in discrete energy levels, rather than occupying any arbitrary distance from the nucleus.

To better understand this concept, let's consider the example of hydrogen, the simplest atom. In the Bohr Model, hydrogen consists of a single proton in its nucleus and a single electron orbiting around it. This electron can exist in different energy levels, which are quantized and represented by integers (n). The lowest energy level, closest to the nucleus, is denoted as n = 1. As n increases, the energy level and the distance of the electron from the nucleus also increase.

When an electron transitions from a higher energy level to a lower energy level, it releases energy in the form of light. This emitted light can be observed as specific colors or wavelengths, creating a line spectrum unique to each element. Similarly, when an electron absorbs energy, it jumps from a lower energy level to a higher energy level.