A photon with an energy of 10.2 eV has a wavelength of 1.21 x 10-7 m, in the ultraviolet part of the spectrum. So when an electron wants to jump from n = 1 to n = 2, it must absorb a photon of ultraviolet light.

Electrons do not stay in excited states for very long – they soon return to their ground states, emitting a photon with the same energy as the one that was absorbed.

Let me explain further, as electron gets closer to an atom the electrostatic & other quantum mechanical forces between the electron starts pulling it, and as electron gets closer the electron is essentially more confined and since Heisenberg’s uncertainty principle governs that the electrons momentum has to become …

The energy difference between the n = 4 and n = 3 orbitals is larger than the energy difference between the n = 3 and n = 2 orbitals.

An element produces bright and dark lines with the same wavelengths. For example, hydrogen has three prominent lines with wavelengths of 434 nm, 486 nm, and 656 nm; these appear dark if the hydrogen is absorbing light, and bright if it is emitting light, but the same three wavelengths are seen in either case.

What colors of light are absorbed by helium gas? primarily the yellow,blue,blue-green and red but also violet and blue are somewhat absorbed. In 1913, Niels Bohr proposed that the unique spectral lines created by different elements were related to the way electrons were arranged around the nucleus.

The different colors of light all travel at roughly the same speed in air. In glass, however, this is not true. Blue light gets slowed down by glass more than red light. As a result of their different speeds in the glass, the red and blue light get bent at different angles when they go into the prism.

violet light