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The atomic number of an element is a fundamental property that defines the number of protons in the nucleus of an atom. This unique identifier determines the element's identity and its position in the periodic table. For example, helium has an atomic number of 2, meaning it has 2 protons, while carbon has an atomic number of 6, giving it 6 protons.
The atomic number not only influences an element's chemical behavior but also its electron configuration. Since each element has a distinct atomic number, it also has a unique set of energy levels and emission spectra.

Electron configuration describes how electrons are distributed in an atom's orbitals. Different elements have distinct electron configurations based on their atomic numbers.
For instance, helium, with an atomic number of 2, has the electron configuration 1s², meaning both of its electrons occupy the first energy level in the s-orbital. Carbon, with an atomic number of 6, has an electron configuration of 1s² 2s² 2p², where the electrons fill the first and second energy levels in a specific order.
Electron configurations affect how atoms interact with light and, therefore, their emission spectra. The unique arrangement of electrons in different elements results in specific energy levels and transitions, leading to distinct lines in their emission spectra.

Energy levels in atoms are like the rungs of a ladder that electrons can 'climb' or 'descend'. When an electron absorbs energy, it moves to a higher energy level. When it releases energy, it falls back to a lower level, emitting light in the process.
Each element has a unique set of energy levels dictated by its electron configuration. This creates a characteristic pattern in its emission spectrum.
For example, the energy levels in helium and carbon are different due to their distinct electron configurations. Helium's simple 1s² setup results in a different pattern of energy emissions compared to carbon's more complex 1s² 2s² 2p² configuration.
Understanding these energy transitions is key to explaining why each element has a unique emission spectrum.