What does a bright line spectrum display?

A bright line spectrum, also known as an emission spectrum, displays colors produced when electrons transition from higher energy levels to lower energy levels within an atom. When an electron in an atom absorbs energy, it can get excited to a higher energy state. Eventually, the electron will return to its lower energy state, and as it does so, it releases energy in the form of light. The specific wavelengths (or colors) of light emitted depend on the differences in energy levels of the electrons, which are unique to each element. This results in distinct lines of color that correspond to specific energy transitions.

The bright line spectrum is characteristic of the element that produces it, revealing information about the electronic structure and energy levels of the atom. Thus, this spectrum serves as a unique fingerprint for elements, allowing for applications such as identifying the composition of stars and other celestial bodies.

In contrast, the other options refer to phenomena that do not specifically describe the mechanism of light emission due to electron transitions in atoms. Fusion reactions produce a broad continuous spectrum and chemical reactions may involve numerous compounds and changes that do not relate directly to electron transitions. The gaseous state of elements is involved in producing spectra, but it's the transitions of electrons within those gaseous atoms that lead to the bright