Question

(a) For \(n=4\), what are the possible values of \(l\) (b) For \(I=2\), what are the possible values of \(m_{l} ?(c)\) If \(m_{l}\) is 2 , what are the possible values for \(l ?\)

Short answer

For n = 4, the possible values of l are 0, 1, 2, and 3. For l = 2, the possible values of m_l are -2, -1, 0, 1, and 2. If m_l = 2, the possible values of l are 2 and 3.

Step-by-step solution

Find the possible values of l for n = 4

The angular momentum quantum number (l) can have integer values from 0 to n-1. Here, n = 4, so to find the possible values of l, we will use this formula: l = 0, 1, 2, ..., n-1 For n = 4: l = 0, 1, 2, 3 So, the possible values of l for n = 4 are 0, 1, 2, and 3.

Find the possible values of m_l for l = 2

The magnetic quantum number (m_l) can take integer values from -l to +l, including 0. Here, l = 2, so to find the possible values of m_l, we will use this range: m_l = -l, -(l-1), ..., 0, ..., +(l-1), +l For l = 2: m_l = -2, -1, 0, 1, 2 So, the possible values of m_l for l = 2 are -2, -1, 0, 1, and 2.

Find the possible values of l for m_l = 2

As m_l can take integer values from -l to +l, including 0, we are given m_l = 2 and have to find the possible values of l. We will use the range of possible m_l values to determine the possible l values: m_l = -l, -(l-1), ..., 0, ..., +(l-1), +l Since m_l = 2, we can denote it as follows: 2 = -l, -(l-1), ..., 0, ..., +(l-1), +l The only possible values of l that satisfy this condition are: l = 2 (as +2 lies in the range -2, -1, 0, 1, 2) l = 3 (as +2 lies in the range -3, -2, -1, 0, 1, 2, 3) So, the possible values of l for m_l = 2 are 2 and 3.

Key concepts

Angular Momentum Quantum Number (l)

In quantum mechanics, the angular momentum quantum number, typically denoted as \( l \), plays a crucial role in defining the shape of atomic orbitals. It is one of the four quantum numbers used to describe the unique quantum state of an electron. The value of \( l \) indicates the subshell or sublevel in which an electron resides, which corresponds to the shape of the orbital.
The value of \( l \) can range from 0 to \( n-1 \), where \( n \) is the principal quantum number representing the main energy level or shell. Different values of \( l \) correspond to different types of orbitals:

• \( l = 0 \): s orbital
• \( l = 1 \): p orbital
• \( l = 2 \): d orbital
• \( l = 3 \): f orbital

For example, if \( n = 4 \), the possible values of \( l \) are 0, 1, 2, and 3. This indicates that in the fourth energy level, there are s, p, d, and f orbitals available for electrons.

Magnetic Quantum Number (m_l)

The magnetic quantum number, denoted by \( m_l \), provides information about the orientation of an atomic orbital within a subshell. It is also one of the four quantum numbers that fully describe the quantum state of an electron.
The range of \( m_l \) values depends on the angular momentum quantum number \( l \). For a given \( l \), \( m_l \) can take on integer values from \(-l\) to \(+l\), inclusive. This means that each type of orbital corresponding to a single \( l \) value can have multiple orientations in space:

• If \( l = 0 \), \( m_l = 0 \) (only one orientation for an s orbital).
• If \( l = 1 \), \( m_l = -1, 0, 1 \) (three possible orientations for a p orbital).
• If \( l = 2 \), \( m_l = -2, -1, 0, 1, 2 \) (five possible orientations for a d orbital).
• If \( l = 3 \), \( m_l = -3, -2, -1, 0, 1, 2, 3 \) (seven possible orientations for an f orbital).

So, for example, if \( l = 2 \), \( m_l \) can be \(-2, -1, 0, 1, \) or \( 2 \), which signifies that the d orbitals have five possible spatial orientations.

Atomic Orbitals

Atomic orbitals are regions in an atom where there is a high probability of finding electrons. These orbitals are solutions to the Schrödinger equation, which describes how these probabilities are distributed around the nucleus.
The shape and orientation of atomic orbitals depend on the quantum numbers \( n, l, \) and \( m_l \). Each type of orbital (s, p, d, f) has a distinct shape. S orbitals are spherical, p orbitals are dumbbell-shaped, d orbitals have more complex, cloverleaf shapes, and f orbitals are even more intricate.
The angular momentum quantum number \( l \) determines the shape, and the magnetic quantum number \( m_l \) describes the orientation:

• S orbitals (\( l = 0 \)) are spherical and not directional.
• P orbitals (\( l = 1 \)) exhibit a directional shape, with three possible orientations along the x, y, or z axes indicated by \( m_l \).
• D orbitals (\( l = 2 \)) have five orientations, offering more complex shapes.
• F orbitals (\( l = 3 \)) have seven orientations, being even more intricate.

These orbitals are critical in understanding chemical bonding and electron configurations in atoms. They form the foundation for predicting how atoms will interact and bond with each other.