How do electrons create the colors in a bright line emission spectrum?

Answer 1

When the electron falls from an higher energy level to lower energy level, photons are liberated. The energy is found to be the difference between the two levels which determines the color of the emission spectrum depending on wavelength.

Answer 2

When a compound is incandescent the electons in the atoms are excited into higher energy levels. When these electrons return to lower energy levels photons (light) are emitted. The frequency of the light is related to the energy gap between the upper and lower levels by the equation E = hv where E= energy, h = planks constant and v = frequency of emitted light.

Answer 3

As electron has option to get changed from different levels of energy to different levels there comes chances for getting different lines. Practically speaking there are billions and billions of hydrogen atoms as well as molecules. So probability is always there for emission of different lines. If prob is more then that line is seen distinctly and if low probable then such line cannot be seen so easily.

Answer 4

The photons released by an electron as the electrons makes the transition from a higher energy level to a lower energy level.

Answer 5

A gas under low pressure does not produce a continuous spectrum.

Answer 6

The electron transitions from a high energy state to a lower energy state is the cause of lines apparition in an emission spectrum.

Answer 7

There is one energy difference (one line) for the transition of energy level 2 to energy level 1, another for level 3 to level 1, another for level 3 to level 2, etc.