Dick said:Uh, how did you get a negative ground state energy using that formula?
hhhmortal said:Not too sure. I think that formula would just give you the energy of the level, but doesn't the electron in that level require that amount of energy to be ionised, hence the negative sign.
Dick said:You are right about that. And in fact, I think your answer is right. On the other hand the formula you gave for E is wrong. Why do you try and write down a clear derivation of your result?
hhhmortal said:I'm not too sure, I think I just used that equation then I canceled out certain terms and multiplied it by ћω. This is wrong, but I can't find the right way of doing it.
A hydrogen atom is the simplest and most abundant atom in the universe. It consists of one proton in the nucleus and one electron orbiting around it.
Energy state transitions refer to the movement of an electron between different energy levels in a hydrogen atom. This occurs when the electron absorbs or emits energy in the form of photons.
The energy state transitions determine the spectral lines of hydrogen, which are used to identify its presence in stars and other objects. They also affect the reactivity and chemical properties of the atom.
The energy levels in a hydrogen atom are quantized, meaning that only certain values are allowed. This has important implications in understanding the behavior of atoms and molecules, as well as in modern physics and quantum mechanics.
Energy state transitions in a hydrogen atom result in the emission or absorption of photons, which can be detected as spectral lines in the electromagnetic spectrum. These lines are unique to each element and can be used to identify the presence of hydrogen in various environments.