Why Do Different Elements Have Unique Spectral Lines?

[learning_phys]

why do different spectral lines appear for the excitation of different elements? I know that electrons jump to lower energy levels gives off photons of distinct frequencies but why characterizes them to be a certain frequency for each element? why doesn't an electron in a high orbital (say n=2) give off the same energy when they jump to the n=1 energy level for all elements? why is there a difference in frequency depending on the element?

 

[Dick]

There is a Z in the formula for the energy of a given level, like n=1 an n=2. Z is the number of protons in the nucleus. So the frequency depends on the element.

 

[baba89]

The unique spectral lines observed for each element are a result of the specific arrangement and energy levels of electrons within its atomic structure. When an electron is excited to a higher energy level, it absorbs energy and moves further away from the nucleus. This energy is then released as the electron returns to its original, lower energy level. This release of energy takes the form of a photon, which has a specific frequency and wavelength determined by the energy difference between the two levels.

The energy levels of electrons in an atom are determined by the atomic number and the number of protons in the nucleus. This means that different elements have different energy levels and thus, different frequencies of emitted photons. For example, hydrogen has one proton and one electron, giving it a unique set of energy levels and corresponding spectral lines. On the other hand, helium has two protons and two electrons, resulting in a different set of energy levels and spectral lines.

Additionally, the arrangement of electrons in an atom also plays a role in the unique spectral lines observed for each element. The arrangement of electrons in different energy levels is determined by the number of electrons and their distribution in the atom's electron shells. This can vary greatly between elements, leading to differences in energy levels and spectral lines.

In summary, the unique spectral lines observed for each element are a result of the specific energy levels and electron arrangements within its atomic structure. This is why different elements have distinct and characteristic spectral lines when excited.