Energy of electron vs. Energy Level
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Energy of electron vs. Energy Level
If an atom undergoes a transition from say 1s to 2p, does the energy of the electron also increase? I know the energy state increases for sure since it’s going from the s-orbital to the p-orbital, but does that also mean the energy of th ELECTRON also increases? Can someone please explain why or why not?
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Re: Energy of electron vs. Energy Level
I believe the energy of the electron increases, because when the e- is so far from the nucleus that it's unattached, energy level is 0, and as the e- comes closer and closer to the nucleus, its energy becomes more and more negative, losing energy. Therefore, the farther away it moves from the nucleus/the higher the energy state, the higher (less negative) the energy of the e-
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Re: Energy of electron vs. Energy Level
For an electron to transition to a higher energy level, say 1s to 2p, it must be excited by absorbing energy, from say a photon of light, so the energy of the electron does increase. The 1 in 1s and 2 in 2s indicate the principle quantum numbers, n, which represent the energy and size of the orbital. Therefore, in a transition from 1s to 2p, n is increasing from 1 to 2 and the energy is increasing. The s and p indicate the angular momentum, l, which represents the sub-shell of the n orbital that determines the shape of the orbital.
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