Spectroscopy

[macca69831]

Two Questions:

1. When exposed to a high-voltage power supply, neon emits green light. Does this mean that the electrons in neon emit energy of only one wavelength? Discuss.

2. The flame test requires only one crystal of the salt in question. Potassium salts have a lilac flame. If a crystal of what is believed to be pure KCl is introduced into a flame, and both lilac and yellow colours are observed, what could be two possible explanations?

[superflya]

1) it should be of the same wavelength. as the electrons absorb a quantum of energy to 'jump up' to a specifically higher energy level they will have to emit that same amount upon returning to their ground level as they are unstable.

2) it could be contaminated with sodium which produces a yellow flame.

[naved_s9994]

1) it should be of the same wavelength. as the electrons absorb a quantum of energy to 'jump up' to a specifically higher energy level they will have to emit that same amount upon returning to their ground level as they are unstable.

2) it could be contaminated with sodium which produces a yellow flame.

it's preety correct. Really the only thing I would add is , that for the reason stated in 2) by super.. Flame tests are INaccurate!!

[fady_22]

1) it should be of the same wavelength. as the electrons absorb a quantum of energy to 'jump up' to a specifically higher energy level they will have to emit that same amount upon returning to their ground level as they are unstable.

2) it could be contaminated with sodium which produces a yellow flame.

I don't know about 1): electrons from one shell could be "jumping to" a number of other shells, producing light of a specific wavelength, depending on what shell they jumped to, when they return to ground state. That is why you get a number of lines on an emission spectrum and not one. So couldn't it be emitting light of a number of wavelengths?
The colour that we observe could be a mixture of colours.

[superflya]

1) it should be of the same wavelength. as the electrons absorb a quantum of energy to 'jump up' to a specifically higher energy level they will have to emit that same amount upon returning to their ground level as they are unstable.

2) it could be contaminated with sodium which produces a yellow flame.

I don't know about 1): electrons from one shell could be "jumping to" a number of other shells, producing light of a specific wavelength, depending on what shell they jumped to, when they return to ground state. That is why you get a number of lines on an emission spectrum and not one. So couldn't it be emitting light of a number of wavelengths?
The colour that we observe could be a mixture of colours.

i think ur correct fady

EDIT: 1000TH