Learning Goal: To learn the restrictions on each quantum

Last updated: 8/2/2022

Learning Goal: To learn the restrictions on each quantum number. 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 & corresponds to the subshell in which the electron is located. s subshells are coded as 0, p subshells as 1, das 2, and fas 3. For example, an electron in the 2p subshell has = 1. As a rule, l can have integer values ranging from 0 to n - 1. The magnetic quantum number me corresponds to the orbital in which the electron is located. Instead of 2pz, 2py, and 2pz, the three 2p orbitals can be labeled -1, 0, and 1, but not necessarily respectively. As a rule, me can have integer values ranging from -l to +l. The spin quantum number m, 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. ▼ What is the only possible value of my for an electron in an s orbital? Express your answer numerically. ► View Available Hint(s) 0 Previous Answers Part B ✓ Correct Since the allowed values for my range from - to +l, once you know the value for you know the values for l me. Review I Constants I Periodic Table What are the possible values of me for an electron in a d orbital? Express your answer numerically with sequential values separated by commas. ► View Available Hint(s)