Quantum numbers can be thought of as labels for an electron. Every electron in a
ID: 961287 • Letter: Q
Question
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 ncan 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, psubshells 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. Instead of 2px, 2py, and 2pz, the three 2p orbitals can be labeled 1, 0, and 1, but not necessarily respectively. As a rule, m can have integer values ranging from to +.
The spin quantum number ms corresponds to the spin of the electron in the orbital. A value of 1/2means an "up" spin, whereas 1/2 means a "down" spin.
Which of the following set of quantum numbers (ordered n, , m, ms) are possible for an electron in an atom? 3, 2, 1, -15, 3, 4, 1/23, 3, 1, -1/23, 1, 0, -1/24, 2, -1, -1/24, 3, -2, 1/23, 1, -2, -1/2-2, 1, 0, -1/2
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 ncan 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, psubshells 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. Instead of 2px, 2py, and 2pz, the three 2p orbitals can be labeled 1, 0, and 1, but not necessarily respectively. As a rule, m can have integer values ranging from to +.
The spin quantum number ms corresponds to the spin of the electron in the orbital. A value of 1/2means an "up" spin, whereas 1/2 means a "down" spin.
Which of the following set of quantum numbers (ordered n, , m, ms) are possible for an electron in an atom? 3, 2, 1, -15, 3, 4, 1/23, 3, 1, -1/23, 1, 0, -1/24, 2, -1, -1/24, 3, -2, 1/23, 1, -2, -1/2-2, 1, 0, -1/2
Explanation / Answer
Which of the following set of quantum numbers (ordered n, , m, ms) are possible for an electron in an atom? 3, 2, 1, -1;5, 3, 4, 1/2;3, 3, 1, -1/2;3, 1, 0, -1/2;4, 2, -1, -1/2;4, 3, -2, 1/2;3, 1, -2, -1/2;-2, 1, 0, -1/2
A) Possible set of quantum numbers
3, 1, 0, -1/2
4, 2, -1, -1/2
4, 3, -2, 1/2