Quantum Number Rules 1 of 26 Correct 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. Part B The principal quantum number n corresponds to the shell in which the electron is located. Thus n What are the possible values of m for an electron in a d orbital? can therefore be any integer. For example, an electron in the 2p subshell has a principal Express your answer numerically with sequential values separated by commas. 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,d as 2 , and f as 3 . For example, an electron in the 2p subshell has =1. As a rule, can have integer values ranging from 0 to n1. The magnetic quantum number m corresponds to the orbital in which the electron is located. Part C Learning Goal: To learn the restrictions on each quantum Which of the following set of quantum numbers (ordered n,,m,ms ) are possible for an electron in an atom? number. Check all that apply. Quantum numbers can be thought of as labels for an electron. Every electron in an atom has a View Available Hint(s) 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,d as 2 , and f as 3 . For example, an electron in the 2p subshell has =1. As a rule, can have integer values ranging from 0 to n1. The magnetic quantum number m corresponds 4,3,4,1/2 5,3,4,1/2 to the orbital in which the electron is located