What is the possible energies that electrons in an atom have?

Answer 1

Possible energy levels of an electron in an atom is quantized. That is, there are only discrete energy levels that an electron can have, and nothing in between. These energy levels are given by E(n) = -hcR(Z^2/n^2) = -13.6 eV (Z^2/n^2) where Z is the atomic number and n is the energy level.

Answer 2

There are countless energy levels, which we sometimes call Fermi energy levels, that an electron can exist in. But let's get the rest of the story. For a given atom of a given element, there are "set" energy levels for each electron in that atom. The nature of the atom itself sets them. These are the orbitals and suborbitals for that atom. And if we look at, say, the 1s1 orbital for hydrogen, it will be at a different energy than the 1s1 orbital for a helium atom, or carbon atom, etc. All are 1s1 orbitals, but all distinct energy levels associated with them. We're talking about energy levels for existing electrons in a given atom of a given element. There are other energy levels in which the electron can exist. If we add energy to a given atom, we can ionize it by causing an electron to "jump out" to a higher Fermi energy level. That new level, too, is "set" by the characteristics of the atom. The level has no electron residing in it, but it is an allowable energy level according to the quantum mechanical characteristics of that given atom, and an electron can be given energy to go there. But it's not free of the atom. There are still higher energy levels to which an electron can ge lifted. These are all "fixed" by the nature of the given atom. Once we get this thing going, two, three or more electrons can play the game, each jumping to a specific energy level and then falling back. There are a ton of different energy levels possible for a given atom, and the more electrons it has, the more possible energy levels it will have. That's a lot of levels. By the way, what happens when an electron is lifted to one of these energy levels and falls back? Let's look. The electron will "fall back" into its original orbit, and it will give up a quantum of energy to do this. Note: an electron will be lifted to a given energy level only by absorbing a specific quantum of energy - the quantity necessary to put it exactly out at that higher level. Anyway, that quantum of energy that is released will be released as electromagnetic energy, like light. A very specific color of light. That's what we're doing in a fluorescent tube, but on a massive scale with several different kinds of atoms and lots and lots of different energy levels. That's what is happening to give us a whole bunch of colors of light to create a broad spectrum of light. With enough colors, we can make the light appear generally white, which is a combination of all colors. Let's go on, but note that you've just had your introductory lesson to spectroscopy. See how we sneaked it up on you? So we've got tons and tons of possible energy levels for electrons to hang out in. Lots and lots of different ones. They will vary according to each element, and will be dictated by its very nature. Oh, and all bets are off if the element is chemically bonded. That throws a whole new set of possible energy levels into the mix. See how complicated it got in a short span? That's what chemistry and physics is all about, though. And by looking at stuff a little bit at a time, you can take the puzzle pieces and put them together to give you the whole picture in a surprisingly short time. It isn't that hard with a little effort. Good luck.

Answer 3

The question cannot be answered as you have put it. Is it the electron at the origin, and you want the potential everywhere in space, V=k*e/r (e = -1.602*10^-19C).

Or is it the potential energy of an electron orbiting a nucleus? (answer depends on specifics)

Answer 4

Energy levels