Who says it isn't?burgjeff said:Why isn't the Orbital angular momentum quantum number in the nuclear shell model restricted by the principal quantum number like it is in the atomic shell model?
No it doesn't. Neither does it correspond to energy in the atomic shell model.Also, does the principal quantum number even correspond to energy in the shell model?
burgjeff, Atomic states correspond to energy levels in a Coulomb potential, the energy E ~ 1/n2, where n is the principal quantum number.burgjeff said:Why isn't the Orbital angular momentum quantum number in the nuclear shell model restricted by the principal quantum number like it is in the atomic shell model? Also, does the principal quantum number even correspond to energy in the shell model?
The orbital quantum number, denoted by the letter l, is a quantum number that describes the shape of an electron's orbital in an atom. It determines the subshell in which the electron is located, and it can have values ranging from 0 to n-1, where n is the principal quantum number.
The higher the orbital quantum number, the higher the energy of the electron. This is because electrons with higher values of l are found farther away from the nucleus and experience less attraction, resulting in higher energy levels.
There are n possible values for the orbital quantum number, where n is the principal quantum number. For example, if n = 3, the possible values for l would be 0, 1, and 2.
The orbital quantum number is related to the angular momentum of an electron by the equation L = √(l(l+1)ħ, where ħ is the reduced Planck's constant. This means that the higher the orbital quantum number, the greater the angular momentum of the electron.
The orbital quantum number determines the number of orbitals in a subshell. The number of orbitals in a subshell is equal to 2l+1. For example, a subshell with l=2 would have 2(2)+1 = 5 orbitals, which can hold a maximum of 10 electrons (2 electrons per orbital).