What are the possible values of n, l, and ml for an electron in a 5p orbital? (LO 5.12)

Verified step by step guidance

1. insert step 1> Identify the principal quantum number (n) for a 5p orbital. The number before the letter (p) indicates the principal quantum number, so n = 5.
2. insert step 2> Determine the azimuthal quantum number (l) for a p orbital. The azimuthal quantum number (l) is associated with the shape of the orbital: s = 0, p = 1, d = 2, f = 3. For a p orbital, l = 1.
3. insert step 3> Identify the possible values of the magnetic quantum number (m_l). The magnetic quantum number (m_l) can range from -l to +l, including zero. For l = 1, m_l can be -1, 0, or +1.
4. insert step 4> Summarize the possible values of n, l, and m_l for an electron in a 5p orbital.
5. insert step 5> Conclude that for an electron in a 5p orbital, n = 5, l = 1, and m_l can be -1, 0, or +1.

Key Concepts

Quantum Numbers

Quantum numbers are a set of numerical values that describe the unique quantum state of an electron in an atom. There are four quantum numbers: the principal quantum number (n), the azimuthal quantum number (l), the magnetic quantum number (ml), and the spin quantum number (ms). Each of these numbers provides specific information about the electron's energy level, shape, orientation, and spin.

Principal Quantum Number (n)

The principal quantum number (n) indicates the main energy level or shell of an electron in an atom. It can take positive integer values (1, 2, 3, ...), with higher values corresponding to electrons that are further from the nucleus and have higher energy. For a 5p orbital, n is equal to 5.

Azimuthal Quantum Number (l)

The azimuthal quantum number (l) defines the shape of the orbital and can take integer values from 0 to (n-1). For p orbitals, l is always equal to 1. Therefore, for a 5p orbital, l is 1, indicating that the electron is in a p-type orbital, which has a characteristic dumbbell shape.