Explain the relationship between quantized energy, electrons, and the atomic emission spectrum.?

Answer 1

Atomic emission spectra are the unique spectra of light (usually bands of different colors) that an element produces when energy is passed through it.

Each element has a unique spacing of its electron orbitals. This spacing is revealed by passing electricity through a given element. It's electrons absorb energy and go from the ground state to some excited state. As the electrons, tumble down toward the ground state, they release energy.

But here's the kicker...

The electron will only release the EXACT amount of energy required to go from one orbital...no more no less. This is where the idea of electrons accepting or releasing a quanta of energy. That is why the atomic emission spectra only gives very specific bands of variously colored light...each band represents the quanta of energy necessarily released by an excited state electron as it moves to a lower orbital.

Thus the atomic emission spectra reveal the unique energy differences of orbitals of a given element.

Hope that makes sense....

Answer 2

The emission spectrum of an element is produced when its electrons move from higher levels to lower levels. Since only certain energy levels are permitted the electrons can only release specific "quantities" or "quanta" of energy. (Its like you are walking down the stairs. Your foot can only land on the existing stair steps, not in between steps)

The energy given off between levels determines the frequency and wavelength of light emitted, so the "spectrum" is very specific for an element or compound.

Answer 3

Emission strains are the frequencies of sunshine that an electron emits while it drops from an excited state to a decrease one. each atom has a distinctive set. See the reference for the hydrogen emissions of electrons falling from bigger skill stages to the n=2 point.