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Part A What is the only possible value of mę 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) Submit

Part A What is the only possible value of mę 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) Submit

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
Chapter5: Quantum Mechanics And Atomic Structure
Section: Chapter Questions
Problem 28P: Quantum mechanics predicts that the energy of the ground state of the H atom is 13.6eV . Insight...
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Review TConstants |PerIodic Tabie Learning Goal: To learn the restrictions on each quantum number. Part A Quantum numbers can be thought of as labels for an electron. Every electron in an atom has a unique set of four quantum numbers. What is the only possible value of m, for an electron in an s orbital? The principal quantum numbern 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. Express your answer numerically. • View Available Hint(s) 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 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 Submit The magnetic quantum number mų 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. Part B 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 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) Submit
Transcribed Image Text:Review TConstants |PerIodic Tabie Learning Goal: To learn the restrictions on each quantum number. Part A Quantum numbers can be thought of as labels for an electron. Every electron in an atom has a unique set of four quantum numbers. What is the only possible value of m, for an electron in an s orbital? The principal quantum numbern 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. Express your answer numerically. • View Available Hint(s) 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 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 Submit The magnetic quantum number mų 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. Part B 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 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) Submit
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