Due to Heisenberg's uncertainty principle one can never know the position of an electron to an arbitrary precision. We can only use quantum mechanical probability densities to estimate it's position. Or we can measure it's location, but that only tells us where it was and can not tell us where it is or how fast it is moving.
One of the first things one must understand about our Universe -- and experiments have found this aspect of quantum mechanics to be true -- is that you can NOT determine the location of an electron within an atom. All you can do is determine the probability that an electron will, over time, be at a specified place. It is NOT the case that we lack the instrumentation or the cleverness to measure this, it is NOT the case that the electrons "knows" where it is but we are unable to pry that information from it -- the location of the electron in an atom is FUNDAMENTALLY unknowable.
Your question is quite reasonable in a Universe that does not obey QM. But, in our Universe, the question is as reasonable as asking, "What's the best way to determine the height at which an elephant has levitated itself above the ground?"
The answer is probability.
they use probability
According to the modern theory of quantum mechanics the electrons have a vibrating wave character and hence uncertain positions.Sometimes,they are close to the nucleus and sometimes away from it.Thus we can say that the paths of motion of electrons around the nucleus are not definite
Heisenberg and Schrodinger developed the electron cloud model using quantum mechanical probability functions to determine the the regions, or clouds, in which electrons would most likely be found outside of the nucleus.
In theory, the number of electrons with each quantum number is not limited. However, for any given "main quantum number" (n), the number of electrons having the other quantum numbers is limited - but it depends on the value of "n". For more information, the Wikipedia article on "quantum number" seems to give a good overview.
Actually it is quite simple. If you are familier with the basics of the quantum theory you can see that the number of orbitals for any given principle quantum number is n^2. Since one orbital can carry a maximum of 2 electrons, the total number of electrons for a principle quantum number is 2 x n^2 = 2n^2 If you are unfamilier with quantum theory. It can be simplified like so - we know that electrons are present in three dimensional energy levels (orbitals). Each of these energy levels have may many sub orbitals. for example for the 1st energy level the number of sub orbitals is n^2 (n square) that is 1 x 1 = 1. then the total number of electrons for this energy level is 2n^2 = 2 x 1^2 = 2.
Because I'm good at black ops 2
use the quantum theory
Location and momentum. You can determine either, but not both.
I think you are referring to the 3 quantum numbers, n, l m; principal azimuthal and magnetic. Together with the spin quantum number they "define" an electron- but I would hesitate to call this the electrons location- Heisenbergs uncertainty principle gets in the way of a simultaneous knowledge of energy and location.
According to the modern theory of quantum mechanics the electrons have a vibrating wave character and hence uncertain positions.Sometimes,they are close to the nucleus and sometimes away from it.Thus we can say that the paths of motion of electrons around the nucleus are not definite
Heisenberg and Schrodinger developed the electron cloud model using quantum mechanical probability functions to determine the the regions, or clouds, in which electrons would most likely be found outside of the nucleus.
An electron configuration shows the distribution of electrons among the subshells. Each number shows the principal quantum number, or shell, the subshell and finally the orbital of the electron.
Joseph John Thomson, Max Planck
Classical free electron theory could not explain many physical properties. In 1928, Sommerfeld developed a new theory applying quantum mechanical concepts and Fermi-Dirac statistics to the free electrons in the metal. This theory is called quantum free electron theory.
In theory, the number of electrons with each quantum number is not limited. However, for any given "main quantum number" (n), the number of electrons having the other quantum numbers is limited - but it depends on the value of "n". For more information, the Wikipedia article on "quantum number" seems to give a good overview.
I think you are referring to the 3 quantum numbers, n, l m; principal azimuthal and magnetic. Together with the spin quantum number they "define" an electron- but I would hesitate to call this the electrons location- Heisenbergs uncertainty principle gets in the way of a simultaneous knowledge of energy and location.
John Lewis Heilbron has written: 'A history of the problem of atomic structure from the discovery of the electron to the beginning of quantum mechanics' -- subject(s): Quantum theory, Electrons, Atomic theory
Electrons can be described as waves and the laws of quantum mechanics determine them and their location probabilistically or statistically. Applying these laws, electrons are distributed in orbitals around the nucleus of the atom according to how much energy they have with higher energies being more distant from the nucleus. The different orbitals have different shapes. The equations say that there are "nodes" where the probability is zero and again these nodes differ for the different orbitals and energies. One of the mind blowing things about quantum mechanics is that electrons can only be at certain discrete energies and orbitals and therefore must be able to go from one to the other without ever passing in between. As the great Richard Feynmann said, if you think you understand quantum mechanics, then you don't really understand quantum mechanics. But the math works and the theory is the most precise and proven theory in the history of science.