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Why do electrons emit light when they fall down to their ground state?
Wiki User
∙ 9y ago
There's a difference in energy between the excited state and the ground state. The energy has to go somewhere. It's generally emitted as electromagnetic radiation ... "light".
Wiki User
∙ 9y ago
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What is difference between a ground state electrons configuration and an excited state configuration?
In the ground state all the (only one for Hydrogen)) electrons is in the lowest stable orbit. If the electron gains energy (usually from a photon) it will orbit in a higher energy state (called excited).
What causes the colored flame for each element on the subatomic level?
The heat of the flame gives off energy to the ions. This results in electrons jumping out of their ground state and into their excited state. From a lower subatomic level to a higher one. When the electrons fall back down, the give off a color.
Do the colors of flame tests result from taking in energy or releasing energy?
Both. Electrons absorb energy and move to a higher energy state, which is unstable, and they fall back down to their ground state immediately, releasing energy as they do.
In which case will the woman see a just a spectrum that is almost entirely black except for few bright emission lines?
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.
Why is a lithium nitrate flame and a lithium chloride flame the same color?
Lithium nitrate and lithium chloride flame tests produce the same color because it is the lithium electrons that are raised to a higher energy level and then drop back down to their ground state. Any ionic compound containing lithium will give the same results. Flame tests are used to show the color and spectrum of the element as its electrons are raised to a higher energy level and then fall back to their ground state.
What is difference between a ground state electrons configuration and an excited state configuration?
In the ground state all the (only one for Hydrogen)) electrons is in the lowest stable orbit. If the electron gains energy (usually from a photon) it will orbit in a higher energy state (called excited).
Why is no color emitted from the solid before it is placed into the flame?
Its electrons have not been excited to higher energy levels until after the solid is placed in the flame. The heat causes electrons to be excited and when they fall back down to their ground state, they emit light at a specific wavelength, giving off a specific color of visible light.
What is reproduced when electrons fall from the exited state?
Every electron that falls from an excited state back down to the ground state releases a "photon," which is a bundle of energy in the form of light. Albert Einstein came up with this term, and a whole bunch of photons all released at once can make a visible light. This is how glow sticks and neon lights basically work.
When you put an element in a flame you see different colors of light given off How why?
The heat of the flame provides thermal energy which can excite the electrons in the atom to higher energy levels. When the electrons 'relax' down to their ground state the excess energy is given out as radiation. For it to be coloured, the radiation must fall in the visible spectrum.
Ground state vs excited state?
A ground state is an outer orbital electron of an element that is at its lowest possible energy level. The electron in an excited state has a higher energy level than a ground state electron. The average distance from the nucleus is greater in the excited state than in the ground state.
What is the definition of excited state electron?
An atom will go into an excited state when the electrons are given extra energy. Then after the electrons have been excited it will eventually go back to ground state producing a light as it returns to its normal state.
What causes the colored flame for each element on the subatomic level?
The heat of the flame gives off energy to the ions. This results in electrons jumping out of their ground state and into their excited state. From a lower subatomic level to a higher one. When the electrons fall back down, the give off a color.
What must happen to the electron in order for an atom to emit light?
The atom must be subjected to a form of energy which propels the electron(s) to a higher energy level. When the electrons return to their resting state they emit one photon of light at a certain wavelength that our eyes interpret as a color.
Why does sodium make fire yellow?
Energy from the fire temporarily promotes some of the electrons in atoms to higher energy levels. When they fall back down to the ground state, and this emits light of characteristic frequencies ... in the case of sodium, two of the most prominent lines are in the yellow-orange region of the spectrum.
Why do the metal ions radiate energy as light?
Metal ions radiate energy as light because of the electrons. The electrons that are moving around the nucleus move in spaces called orbitals. When an electron is zapped with energy (usually electricity) the electrons absorb that energy and jump to a higher energy level than at which they were. As the electrons lose this energy, they fall back to their ground state or their "normal non-excited state" and they emit or release the same amount of energy that they absorbed or the equivalent to the amount they absorbed in the same amount of levels that they dropped down. The energy that is emitted is what we know as light, but they also emit UV and infrared radiation.
Do the colors of flame tests result from taking in energy or releasing energy?
Both. Electrons absorb energy and move to a higher energy state, which is unstable, and they fall back down to their ground state immediately, releasing energy as they do.
How do the Aurora Brealis colours form?
Gases get excited by charged solar particles, their electrons rise to higher energy levels, when the electrons drop down to a lower level they emit characteristic colored light. Oxygen emissions give green or brownish-red colors, depending on the amount of energy absorbed. Nitrogen emissions give blue or red; blue if the atom regains an electron after it has been ionized, red if returning to ground state from an excited state.
