Question

Explain how line spectra are used to identify elements and what they indicate about atoms. Please help!!

Answer 1

watch this vid https://www.youtube.com/watch?v=GhAn8xZQ-d8

Answer 2

Its about valence electrons I believe

Answer 3

A spectral line is like a fingerprint that can be used to identify the atoms, elements or molecules present. The presence of spectral lines is explained by quantum mechanics in terms of the energy levels of atoms, ions and molecules. These energy levels depend on the numbers of protons, electrons and neutrons in an atom, and the limited set of configurations in which these elemental particles can exist (the set of quantum numbers). Atoms prefer to be in their ground state, where all of the electrons are located as close to the nucleus as possible. Absorption lines occur when an atom, element or molecule absorbs a photon with an energy equal to the difference between two energy levels. This causes an electron to be promoted into a higher energy level, and the atom, element or molecule is said to be in an excited state. Emission lines occur when the electrons of an excited atom, element or molecule move between energy levels, returning towards the ground state. The spectral lines of a specific element or molecule at rest in a laboratory always occur at the same wavelengths. For this reason, we are able to identify which element or molecule is causing the spectral lines.