Electron Energy in Atoms: What is it?

In summary, the energy levels of electrons in atoms are determined by the principle quantum number n, which dictates the dominant energy state, and the various degenerate orbitals within each n. The energy of each orbital can be calculated using the Bohr formula, which takes into account the mass of the electron, Planck's constant, and the charge and permittivity of free space. The energy levels can be further affected by spin-orbit coupling, external fields, and other factors.
  • #1
darkar
187
0
What energy do electrons poses in atoms?
 
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  • #2
What atom? What orbital level? Be more specific.

For instance, the energy level of an electron in a hydrogen atom in orbital level n is

[tex]E_n = -(me^4)/((4*pi*e_o)^2(2h_b*n^2))[/tex]

Gah, pardon the terrible laytex. That should give you an idea though. Just do a search on the web for a prettier written formula.
 
  • #3
Like Locrian pointed out an electron has different possible enery-values, each corresponding to the orbital they are on. Each capital level is denoted by a quantumnumber n that has the "values" 1,2,3,.. corresponding to the K,L,M,N,...levels. Per level there are n possible sublevels denoted as s(0),p(1),d(2),f(3)-levels (these are the orbitals, or the probability value of the angular solutions of the Schrödinger-equation.). Per orbital there are 2n+1 possible "sub-sub"levels. for example d has number 2, so there are 5 different d-orbitals that contain maximum two electrons of the same energy when no EM-field is applied on the atom. These 5 d-robitals each correspond to a different energy...

Per sub-sub-level there is also the magnetic quantumnumber that has two values for spin 1/2-particles. Each energy-level is split in two when an extern magnetic field is applied over the atom, due to the two possible values of this quantumnumber. This effect is called the Zeemann-effect.


regards
marlon
 
  • #4
Er... I'm going to nitpick here a bit since I see a few problems...

1. We all agree that the original question was VAGUE.

2. I have no idea what formula Locrian is quoting.

3. At the SIMPLEST level, if we adopt the Bohr model (which we all know is not correct, but is damn accurate for H atom, so-so for slightly heavier atoms, and completely whacky for very heavy atoms), then one can find the "energy" of the electronic state from usual sources.

http://hyperphysics.phy-astr.gsu.edu/hbase/hyde.html

4. We need to be clear about one thing here. The principle quantum number, n, typically dictates the dominant energy state of the atom. The various orbitals (the s,p,d, etc) that are within each n are DEGENERATE states. By that we mean they have the identical energy state within each n. It is only when the degeneracy is REMOVED, either via spin-orbit coupling, application of external fields, etc., that they will have separate energy states.

Zz.
 
  • #5
I think with the correct addendum of Zz, the question is solved...


regards
marlon
 
  • #6
ZapperZ said:
2. I have no idea what formula Locrian is quoting.

Well, if you plug in all the constants and convert them to units of eV, you get something like -13.5eV/n^2 ... maybe that's more familiar?
 
  • #7
Other than that, electrons always move in the electron cloud right? Can you say that they have kinetic energy?
 
  • #8
I have no idea what formula Locrian is quoting

He probably meant: [tex]E_n=-\left[\frac{m}{2\hbar^2} \left(\frac{e^2}{4\pi \epsilon_0} \right) ^2 \right]\frac{1}{n^2}=\frac{E_1}{n^2}=\frac{-13.6eV}{n^2}[/tex]

Wich is the famous "Bohr formula"
 

Related to Electron Energy in Atoms: What is it?

1. What is electron energy in atoms?

Electron energy in atoms refers to the energy level or state of an electron within an atom. It is the amount of energy that an electron possesses as it orbits the nucleus of an atom.

2. How is electron energy in atoms measured?

Electron energy in atoms is typically measured in units of electron volts (eV) or kilojoules per mole (kJ/mol). These units represent the amount of energy needed to move one electron through an electric potential difference of one volt or one kilojoule per mole of electrons, respectively.

3. What factors affect the electron energy in atoms?

The electron energy in atoms is affected by the distance of the electron from the nucleus, the number of protons in the nucleus, and the presence of other electrons. The further an electron is from the nucleus, the higher its energy level will be. Additionally, as the number of protons in the nucleus increases, the energy levels of electrons also increase. The presence of other electrons can also affect the energy levels of electrons through repulsion or attraction forces.

4. How does electron energy in atoms relate to chemical reactions?

The energy levels of electrons in atoms play a crucial role in chemical reactions. When atoms interact to form compounds, the electrons in their outermost energy levels (valence electrons) are involved in the bonding process. The energy levels of these valence electrons determine how easily they can be shared or transferred between atoms, which ultimately determines the stability and reactivity of the resulting compound.

5. How do changes in electron energy affect the properties of elements?

Changes in electron energy can greatly impact the properties of elements. For example, when an electron is excited to a higher energy level, it can lead to the emission of light, which is the basis for flame tests used to identify elements. Additionally, the arrangement of electrons in different energy levels can affect the reactivity and chemical behavior of elements, leading to differences in properties such as melting and boiling points, conductivity, and color.

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