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# Bohr model energy levels

Calculating electron energy for levels n=1 to 3. Drawing a shell model diagram and an energy diagram for hydrogen, and then using the diagrams to calculate the energy required to excite an electron between different energy levels.  Created by Jay.

## Want to join the conversation?

• It's all in the definition.
The energy is defined as zero when the electron is an infinite distance from the nucleus. As the electron comes closer, the energy decreases, so the energy of the system becomes negative.
Even for an H atom in an excited state, the energy is negative, but it is less negative than for an atom in the ground state.
• What physical process do you have to do to give energy for a transition? Do you apply voltage to a material to make electrons "jump" to a different orbit? I am having a hard time visualizing this process.
• another common way to give energy is by using the energy of photons from light. Sort of like the photoelectric effect, but instead of having such a high energy photon that it would kick the electron out, it simply excites it to a higher energy level.
• I have two interrelated questions.
1 - If Bohr's model isn't correct (as stated in many of these videos), why is it that we keep referring to it?
2 - If electrons don't go around the nucleus in definite orbits, what's the current explanation regarding the electrons' movement? How can the Bohr "laws" still apply?
***
• Bohr's Model may be wrong but it is still "correct" for many uses/calculations, it's kinda like newtons equation for gravity Einstein may have made it better, but for most cases Newton's math works out fine
• if electron is attracted towards nucleus, why instead of jumping around it doesn't stick to it?
• The Heisenberg Uncertainty Principle says that we cannot know both the position and momentum of a particle. If an electron rests on the nucleus, then its position would be highly defined and its momentum would have to be undefined. So, it cannot completely shed its kinetic energy and must move, yet it will want to minimize its total energy, resulting in the probability wave function of the orbital.
• What will happen if electron get more than 13.6 eV energy photon? Will it absorb or?
• It will escape the potential well of the nucleus and the atom becomes ionized.
• What exactly are electron volts? How are they defined?
• They're the general unit used to define energy in electrons.
• what is a energy level?
• Think of energy levels as the different floors of a very tall building. Atoms have electrons located in on each of these floors. The higher floor the electron is on, the more energy it will have because it will be further away from the center of the atom.
• On each energy level, there is a limit as to how many electrons can be on the level, right. Is there a pattern to the limit of electrons on each energy level? When electrons jump levels the atom produces energy, right, is that energy electricity? How does the number of electrons placed on the energy levels affect the characteristics of the material, I think it causes the material to be more unstable, is that right?
• What about atoms with more than one electron? Are they pulled away one at a time or can you pull several at once with enough energy?
• My textbook book uses a different equation for calculating the energy of electrons on different levels: En=-Rh(Rydberg constant)x1/n^2. What are the differences of this one and the one Jay uses in his explanation?
• Rydberg Constant Value,R∞ = 10973731.568508(65) m-1
Rydberg Constant Value,R∞ = 1.097 x 10^7 m^-1
in 1/METRE
Rydberg Constant in Joules,1Ry = 2.17 10^-18J
*IN JOULES

I think the value in Joules is used here as we're considering Energy, so basically the same
If I'm wrong do let me know,
Hope this helps!
Onward!
(1 vote)