Return to lower energy levels To be in the ground state all electrons must be in their lowest energy state; all excited atoms must lose energy. The lost energy appears in the form of light. Hope this helped :)
is excited with electricity causing it to move up a shell into (for example) n=3 shell. when excited the atom is unstable and will come back down to a n=2 shell and the energy left over is emitted and the emission is in the form of photons of different wavelengths, and if using electricity not heat will result in a bright line spectra
When you heat each element is will emit its own color and depending on the color it emmits that where is will be on the bright line spectrum.
*****************2nd Opinion***************
1. Heating a gaseous element can cause electrons to jump in energy (quantum jumps).
2. Almost immediately, the electrons lose that energy.
3. The lost energy shows up in the form of light, which is emitted from the atom.
4. Only certain energy jumps or falls are allowed by nature, so
5. Only certain frequencies (colors) are produced.
6. Those few colors make up the line spectrum of that element.
Electrons emitting quanta/energy.
Tty
its named after the bright indigo line in its spectrum
A few bright lines against a dark background.
Caesium metal is gives a bright blue solution when dissolved in liquid ammonia. The dissolving is believed to cause the production of caesium ions and a free electron. a similar blue colr is produced by sodium, potassium and rubidium. In aqueous alkali solutions caesium ion is colorless and therefore unless the anion is colored the solution is colorless.
it is a silvery color, but can also be a white color
Neon has a bright, white glow when it has been lit. Plutonium also has a bright glow, due to its reaction with oxygen.
Emission Spectrum
This would consist of several series of lines corresponding to the energies of electron transitions. They are bright lines for an emission spectrum and dark for absorbtion.
Emission spectra are bright-line spectra, absorption spectra are dark-line spectra. That is: an emission spectrum is a series of bright lines on a dark background. An absorption spectrum is a series of dark lines on a normal spectrum (rainbow) background.
There are several kinds of spectra. Bright line spectrum, or emission spectrum, is when light emitted by a gas has an electrical discharge going through it, and it produces a spectrum of just a few isolated parallel lines.
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
a Edit: The question is very mixed up, but I think I get the idea. It's obviously an emission spectrum. Because it is a high density gas the spectrum should be CONTINUOUS.
It requires a certain amount of energy to raise an electron from a specific level to another specific level; the same amount of energy is released again if it falls back down. One - the electron moving up an energy level - corresponds to the absorption of energy; the other - the electron falling down - corresponds to the emission of energy.
It differs by that white light spectrum is continuous and consists of light of all wavelengths. Emission spectrum is not continuous. It consists of bright lines at specific wavelengths, with complete darkness between them.
An emission or absorption line in a spectrum that arises when an electron moves between two energy levels in an atom. A jump to a higher level requires an input of energy, and produces a dark absorption line. A drop to a lower level releases energy, producing a bright emission line.
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.
The spectrum that she will be observing is called an emission spectrum, in which electrons are excited to a higher energy state and then drop back down to the ground state, during which the electrons will emit photons of specific wavelengths, which will be observed as bright lines of color on what appears to be a black background.
The colors of light given off when an element loses energy