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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 l = 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 2px, 2py, and 2p%, 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. ▼ Part A What is the only possible value of me for an electron in an s orbital? Express your answer numerically. ► View Available Hint(s) Submit Part B 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)

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 l = 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 2px, 2py, and 2p%, 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. ▼ Part A What is the only possible value of me for an electron in an s orbital? Express your answer numerically. ► View Available Hint(s) Submit Part B 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)

Principles of Modern Chemistry
Principles of Modern Chemistry
8th Edition
ISBN:9781305079113
Author:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler
Publisher:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler
Chapter4: Introduction To Quantum Mechanics
Section: Chapter Questions
Problem 39P: Chapter 3 introduced the concept of a double bond between carbon atoms, represented by C=C , with a...
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Part C Which of the following set of quantum numbers (ordered n, l, me) are possible for an electron in an atom? Check all that apply. View Available Hint(s) 2, 4, 1 5, 3, 4 4, 2, -2 2, 1, 0 2, 1, -2 ☐ -1, 0, 0 5, 3, 0
Transcribed Image Text:Part C Which of the following set of quantum numbers (ordered n, l, me) are possible for an electron in an atom? Check all that apply. View Available Hint(s) 2, 4, 1 5, 3, 4 4, 2, -2 2, 1, 0 2, 1, -2 ☐ -1, 0, 0 5, 3, 0
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 l = 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 2px, 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. Part A What is the only possible value of me for an electron in an s orbital? Express your answer numerically. ► View Available Hint(s) Submit Part B 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)
Transcribed Image Text: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 l = 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 2px, 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. Part A What is the only possible value of me for an electron in an s orbital? Express your answer numerically. ► View Available Hint(s) Submit Part B 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)
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