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.
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.
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.
The photons released by an electron as the electrons makes the transition from a higher energy level to a lower energy level.
A gas under low pressure does not produce a continuous spectrum.
The electron transitions from a high energy state to a lower energy state is the cause of lines apparition in an emission spectrum.
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.
It sounds like you're describing an emission spectrum. An emission spectrum will contain bright lines at specific colors, each of which is characteristic of a particular chemical element.
Red, blue, green, and violet are found in the emission spectrum of hydrogen.
The difference in energy states for the electrons is different in sodium and neon, so they produce different wavelengths (the emission spectrum of each element is different) or colors.
No. They're called the visible spectrum, the range of wavelengths us humans can see.
If there were colors, that part of the spectrum would not be invisible.
It sounds like you're describing an emission spectrum. An emission spectrum will contain bright lines at specific colors, each of which is characteristic of a particular chemical element.
No. Atomic emission spectrum is non-contiuous and it is named as line spectrum.
Dark-line spectrum is a "photo-negative" of emission spectrum. It is the gaps that appear in precisely the same location as corresponding bright lines. produced by a cool gas with a hot solid and you
There are no bright lines and no dark lines in the spectrum, incandescent light has a continuous spectrum with all visible colors present
Red, blue, green, and violet are found in the emission spectrum of hydrogen.
The colors of light given off when an element loses energy
The difference between continuous spectrum and the atomic emission espectrum of an element is that in emission spectrum, only certain specific frequencies of light are emitted while in a continuous spectrum, a continuous range of colors are seen in the visible light.
Computer uses can find the color bright green in the spectrum of colors known in printing as RYGB (red, yellow, green, blue). All colors, including bright green, are contained in this spectrum.
it is a set of lines corresponding to photon emission wavelengths.
Colors are able to form by water droplets that can break sunlight into several colors of the spectrum. Colors can also form by light absorption, emission spectra and reflection.
The name of the range of colors emitted by a heated (energized, excited, etc...) atom is called an emission spectrum.
A broad spectrum of all colors would be observed.