Ephoton=h(Planck's constant) v (frequency of the radiation)
ground state
The 2s and 2p sublevels in the second principal energy level are completely occupied in the ground state of a sodium atom.
By placing atoms of a metal into a flame, electrons can be induced to absorb energy and jump to an excited energy state, a quantum jump. They then return to their ground state by emitting a photon of light (the law of conservation of energy indicates that the photon emitted will contain the same amount of energy as that absorbed in the quantum jump). The amount of energy in the photon determines its color; red for the lowest energy visible light, increasing energy through the rainbow of orange yellow green blue indigo, and finally violet for the highest energy visible light. Photons outside the visible spectrum may also be emitted, but we cannot see them.
The groundstate for Sodium (11-Na) is: 1S2 , 2S2, 2P6, 3S1 If you count the ^powers you notice it'll sum to 11, when Sodium is excited the outermost electron (3S1) will be excited from the 3S shell to the next shell up which is the 3P shell. The "core" electron configuration doesn't change so the first excited state is simply: 1S2 , 2S2, 2P6, 3P1 For the next excited state the electron that is now in the 3P shell will transition to the 4S shell before the 3D shell
The ground state electron configuration for sodium is 1s2 2s2 2p6 3s1
When sodium ions are heated, electrons move from the ground state to the excited state, and because they are unstable in the excited state, they immediately return to lower energy levels in the ground state. As they do this, energy is released in the form of light. In the case of sodium, it produces orange light.
ground state
Its electrons are excited to a higher energy state in the flame, and then they immediately release that energy, which is visible as yellow light.
excited electrons returning to the ground state.
It depends upon the gas involved in the plasma. For example, neon plasma is a bright red-orange, sodium is a bright yellow, mercury produces a cool-blue, and nitrogen produces a pink. The color of the plasma depends on the particular element's "emission spectrum." When you excite a gas with a high-voltage, the valence electrons become excited and jump up to a higher state. When they de-excite, they drop back down to their ground state and emit a photon. The energy of this photon is equal to the energy difference between the ground state and the excited state.
The 2s and 2p sublevels in the second principal energy level are completely occupied in the ground state of a sodium atom.
when something is in the ground^No. That is totally incorrect.Basically, a ground state electron is when the atom/element is not being surged through with heat or electricity. Basically, it's the atom's normal electron configuration. So NA [Sodium]'s ground state would be shown as : 1s2, 2s2, 2p6, 3s1.The opposite is when it's in it's excited state. You can remember tell when an atom is in it's excited state when in the electron configuration, there is a huge jump, like 1s2,2s2,2p5, 3s2. This might have happened due to being exposed to heat and or electricity.In other words, ground state=normal, excited is, well, excited. XD
Sodium Chloride is a crystal lattice and it is an ionic compound. It is a salt used in the ocean and when you burn the sodium chloride, the electrons on the compound gets excited and starts "jumping" from one energy level to another. This causes color change.
1s2 2s2 2p6
By placing atoms of a metal into a flame, electrons can be induced to absorb energy and jump to an excited energy state, a quantum jump. They then return to their ground state by emitting a photon of light (the law of conservation of energy indicates that the photon emitted will contain the same amount of energy as that absorbed in the quantum jump). The amount of energy in the photon determines its color; red for the lowest energy visible light, increasing energy through the rainbow of orange yellow green blue indigo, and finally violet for the highest energy visible light. Photons outside the visible spectrum may also be emitted, but we cannot see them.
sodium
The groundstate for Sodium (11-Na) is: 1S2 , 2S2, 2P6, 3S1 If you count the ^powers you notice it'll sum to 11, when Sodium is excited the outermost electron (3S1) will be excited from the 3S shell to the next shell up which is the 3P shell. The "core" electron configuration doesn't change so the first excited state is simply: 1S2 , 2S2, 2P6, 3P1 For the next excited state the electron that is now in the 3P shell will transition to the 4S shell before the 3D shell