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".
In the ground state configuration, electrons are in their lowest energy levels within an atom. In an excited state configuration, electrons have absorbed energy and moved to higher energy levels, creating an unstable state that is temporary before returning to the ground state.
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.
The colors seen in flame tests result from the release of energy. When a substance is atomized and exposed to a flame, electrons in the atoms are excited to higher energy levels. As the electrons return to their normal energy levels, they release energy in the form of light, creating the characteristic colors of flame tests.
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.
When an atom gains or loses energy, electrons jump between energy levels. Electrons absorb energy to move to higher energy levels (excitation) and release energy as they move back down to lower energy levels (emission). This jump in energy levels is responsible for the emission or absorption of light, which can be used to identify atoms and molecules.
In the ground state configuration, electrons are in their lowest energy levels within an atom. In an excited state configuration, electrons have absorbed energy and moved to higher energy levels, creating an unstable state that is temporary before returning to the ground state.
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.
An atom is in its ground state when its electrons are in their lowest energy levels. When atoms absorb energy, their electrons can jump to higher energy levels, creating an excited state. The excited state is temporary and the electrons will eventually return to their ground state, releasing the absorbed energy as light or heat.
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.
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.
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.
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.
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.
Metal ions radiate energy as light when they undergo a process called luminescence. This occurs when the metal ions are excited to higher energy levels and then return to their ground state, releasing energy in the form of light. The specific color of light emitted depends on the specific properties of the metal ion.
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.
The colors seen in flame tests result from the release of energy. When a substance is atomized and exposed to a flame, electrons in the atoms are excited to higher energy levels. As the electrons return to their normal energy levels, they release energy in the form of light, creating the characteristic colors of flame tests.
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.