Consider the following sets of quantum numbers:
n l m s
(a) 3 0 0 + 12
(b) 2 2 1 + 12
(c) 4 3 -2 - 12
(d) 1 0 -1 - 12
(e) 3 2 3 + 12
Which of the following sets of quantum number is not possible?
Consider the following sets of quantum numbers:
n l m s
(a) 3 0 0 + 12
(b) 2 2 1 + 12
(c) 4 3 -2 - 12
(d) 1 0 -1 - 12
(e) 3 2 3 + 12
Which of the following sets of quantum number is not possible?
The correct option is D b, d and e
Choice (b), (d) and (e) are incorrect. Remember that value of ‘l’ ranges from (0) to (n – 1) and values of ‘m’ range from (–l) to (+l).
The three coordinates that come from Schrodinger's wave equations are the principal (n), angular (l), and magnetic (m) quantum numbers. These quantum numbers describe the size, shape, and orientation in space of the orbitals on an atom.
The principal quantum number (n) describes the size of the orbital whereas the angular quantum number (l) describes the shape of the orbital. Orbitals have shapes that are best described as spherical (l = 0), polar (l = 1), or cloverleaf (l = 2). They can even take on more complex shapes as the value of the angular quantum number becomes larger. There is only one way in which a sphere (l = 0) can be oriented in space - spherical. Orbitals that have polar (l = 1) or cloverleaf (l = 2) shapes, however, can point in different directions or orientations. Hence, we need a third quantum number, known as the magnetic quantum number (m), to describe the orientation in space of a particular orbital.
Rules Governing the Allowed Combinations of Quantum Numbers:
The three quantum numbers (n, l, and m) that describe an orbital are integers: 0, 1, 2, 3, and so on.
The principal quantum number (n) cannot be zero. The allowed values of n are therefore 1, 2, 3, 4, and so on.
The angular quantum number (l) can be any integer between 0 and n - 1. If n = 3, for example, l can be either 0, 1, or 2.
The magnetic quantum number (m) can be any integer between -l and +l. If l = 2, m can be either -2, -1, 0, +1, or +2.
Simply, we have to weed out options where l≥n and/or m>n. Spin, like mass and charge, is a fundamental property of quantum entities. It can take either - 12 or + 12
b, d and e
Choice (b), (d) and (e) are incorrect. Remember that value of ‘l’ ranges from (0) to (n – 1) and values of ‘m’ range from (–l) to (+l).
The three coordinates that come from Schrodinger's wave equations are the principal (n), angular (l), and magnetic (m) quantum numbers. These quantum numbers describe the size, shape, and orientation in space of the orbitals on an atom.
The principal quantum number (n) describes the size of the orbital whereas the angular quantum number (l) describes the shape of the orbital. Orbitals have shapes that are best described as spherical (l = 0), polar (l = 1), or cloverleaf (l = 2). They can even take on more complex shapes as the value of the angular quantum number becomes larger. There is only one way in which a sphere (l = 0) can be oriented in space - spherical. Orbitals that have polar (l = 1) or cloverleaf (l = 2) shapes, however, can point in different directions or orientations. Hence, we need a third quantum number, known as the magnetic quantum number (m), to describe the orientation in space of a particular orbital.
Rules Governing the Allowed Combinations of Quantum Numbers:
The three quantum numbers (n, l, and m) that describe an orbital are integers: 0, 1, 2, 3, and so on.
The principal quantum number (n) cannot be zero. The allowed values of n are therefore 1, 2, 3, 4, and so on.
The angular quantum number (l) can be any integer between 0 and n - 1. If n = 3, for example, l can be either 0, 1, or 2.
The magnetic quantum number (m) can be any integer between -l and +l. If l = 2, m can be either -2, -1, 0, +1, or +2.
Simply, we have to weed out options where l≥n and/or m>n. Spin, like mass and charge, is a fundamental property of quantum entities. It can take either - 12 or + 12
