
#1
Feb2912, 06:53 PM

P: 54

If there is a cloud of electrons around an atom than why can't there be orbitals between 1 and 2 or between 2 and 3. I know the probability of an electron being between certain nodes decreases as they approach them but why as the probabilities go away from the perfect orbital do they not become fractional orbitals? (just starting to learn this stuff)




#2
Feb2912, 07:28 PM

P: 194

If you solve the angular part of the Schrödinger equation in the Coulomb potential (or for any spherically symmetric potential), you'll find that in order to satisfy boundary conditions at [itex]\theta=0[/itex] and [itex]\theta=\pi[/itex] and [itex]\phi=0[/itex] and [itex]\phi=2\pi[/itex], you need to have "integer orbitals" (in your language).




#3
Feb2912, 07:49 PM

Sci Advisor
P: 2,194

Simply because there are no (fractional) integers! The orbitals are labeled by their radial quantum number, n, which is an integer. So while an electron in the n=1 orbital has a finite probability of being found at the most probable radius for an electron in the n=2 orbital, and vice versa, they are distinct quantum states.



Register to reply 
Related Discussions  
Motion of electrons in orbitals and shape of orbitals  Chemistry  5  
Angular momentum  integer or halfinteger  Quantum Physics  2  
Proof Question: Prove integer + 1/2 is not an integer  Calculus & Beyond Homework  4  
constructing orthogonal orbitals from atomic orbitals  Atomic, Solid State, Comp. Physics  8  
Atomic Orbitals vs. Molecular Orbitals and Hybridization  Chemistry  1 