difference between electron shell vs orbital

Electron shell - An electron shell may be thought of as an orbit followed by electrons around an atom nucleus. Because each shell can contain only a fixed number of electrons, each shell is .....

Electron shell - An electron shell may be thought of as an orbit followed by electrons around an atom nucleus. Because each shell can contain only a fixed number of electrons, each shell is associated .....

Molecular orbital - ... completely full energy shells ... for core orbitals. This however is incorrect as these experiments measure the ionization energy, the difference in energy between the molecule and .....

Atomic orbital - Because of the difference from classical mechanical ... correspond to transitions (quantum leaps) between ... For instance, the n = 1 shell has only orbitals with , and the n = 2 .....

  How does the wavelength of a matter wave relate to the orbits of the B..   described by quantum (meta)physics as the 'jumps' or 'leaps' made by electrons between 'orbits' (fixed quantum energetic levels) of an atom. The conventional depiction of an atom shows the nucleus surrounded by perfect concentric orbits for electrons. This original model was developed by Niels Bohr. He determined that the electrons actually possess a negative charge and each of the rings or orbits represented a different energy level, often called 'layers' or 'shells'. The electrons of ...

  what are the differences between the 2s orbital and the 1s orbital of ..   equals one. L equals zero. And the superscript two is an indication of electron occupancy. In plain English, this says that there are two electrons in the 1s orbital. And then we can continue. This is two electrons in the 2s orbital, and there are two electrons in the 2p orbital. Another way of displaying this is in a box notation. Here is 1s, if you like, k shell. Here is 2s, l shell. And then there is 2p. And we know from over here that 2p has the possibility of three different m numbers. ...

Question : When electrons are moving in shells around the nucleus, then what are the s,p,d and f orbitals? And why are these not in circular shapes?

Answer : spd and f are letters that describe the orbital angular momentum of the electron. In units of h-bar, s is zero, p is one, d is two, f is three, g is four, etc Now as a whole, all of these are spherical. But for each value, l, of angular momentum, there are 2l+1 states that describe the z-component of angular momentum. They run from -l to l. Now although all the 2l+1 states put together are spherically symmetric, they each are not spherical--except in the case of the s orbitals, where l=0, so there's only one state, and it's spherically symmetric.

Question : tell me the defination for both atomic and ionic radii the distance between the center of the nucleus and outer most shell which has an electron is called atomic radii. the distance between the center of the nucleus and outer most shell which has an electron cloud is called ionic radii. is this is correct or not???

Answer : atomic radii is the radios of the atom when it's in neutral. ionic radii is the radios of the atom when it losses or gains electron ( become an ion) so for the very same element the number of electrons in atom differs than the number of electrons of the ion which might cause a change in the number of orbitals and the radios. hope this helps

Question : the oder from lower to high energy orbital is this 1s, 2s, 2p, 3s, 3p, 4s, 3d ..... so i'm wondering, when you start to write the shell notation which one do you start filling FIRST the 4s or 3d? because 3d has a higher energy level that 4s, however 3d is nearer to the nucleus than 4s For those of you who think its the same thing, its not because this could mean the difference between a 3d^9, 4s^2 and 3d^10, 4s^1 (^ are the superscript) representing amount of electrons) THERE SHOULD BE SOME KI..

Answer : der Aufbau (in German it means to 'build up') is the principle that describes the order that electron orbitals are filled. The shapes of the s, p, d, and f orbitals are strikingly different. While the s orbital is spherical, the others are not. So the energy levels of the orbitals and the order they are filled is not simply in order of some radius from the nucleus of the atom. Edwin Schroedinger wrote some intersting solid trigonometry differencial equations to describe the shapes of those orbitals back in the 1930s. the 4s orbital is filled before the 3d because it has a lower energy level. By the way, most texts don't mention it but the order that the electron orbitals are filled is NOT always the same order that the electrons are lost when cations are formed. What this means is that transitional metals typically lose electrons from their s orbitals to form cations BEFORE they lose electrons from their d orbitals, even though the d orbital electrons were loaded in after the ..