Quantum Number Rules
Quantum numbers can be thought of as labels for an electron. Every electron in an atom has a unique set of four quantum numbers.
The principal quantum number n corresponds to the shell in which the electron is located. Thus n can therefore be any integer. For example, an electron in the 2p subshell has a principal quantum number of n=2 because 2p is in the second shell.
The azimuthal or angular momentum quantum number ℓ corresponds to the subshell in which the electron is located. s subshells are coded as 0, p subshells as 1, d as 2, and f as 3. For example, an electron in the 2p subshell has ℓ=1. As a rule, ℓ can have integer values ranging from 0 to n−1.
The magnetic quantum number mℓcorresponds to the orbital in which the electron is located. Instead of 2px, 2py, and 2pz, the three 2p orbitals can be labeled −1, 0, and 1, but not necessarily respectively. As a rule, mℓcan have integer values ranging from −ℓ to +ℓ.
The spin quantum number ms corresponds to the spin of the electron in the orbital. A value of 1/2 means an “up” spin, whereas −1/2means a “down” spin.
What is the only possible value of mℓ for an electron in an s orbital?
What are the possible values of mℓ for an electron in a d orbital?
Posted on October 10, 2013, in Question and tagged angular momentum quantum number, Chemistry, electron, integer values, principal quantum number, Quantum Number Rules, quantum numbers, question, science, What are the possible values of mℓ for an electron in a d orbital?, What is the only possible value of mℓ for an electron in an s orbital?. Bookmark the permalink. Leave a comment.