Part A. What is the only possible value of ml for an electron in an s orbital?
Express your answer numerically.
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 nn corresponds to the shell in which the electron is located. Thus nn 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\ell can have integer values ranging from 0 to n − 1.
The magnetic quantum number ml corresponds 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, ml can have integer values ranging from −l to +l.
The spin quantum number msm_s corresponds to the spin of the electron in the orbital. A value of 1/2 means an "up" spin, whereas −1/2 means a "down" spin.
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