Give the values for n, l, and 𝑚𝑙 for a. each orbital in the 2p subshell

Verified step by step guidance

1. <em>n</em> is the principal quantum number, which indicates the energy level of the electron. For the 2<em>p</em> subshell, <em>n</em> = 2.
2. The azimuthal quantum number, <em>l</em>, defines the shape of the orbital. For <em>p</em> orbitals, <em>l</em> = 1.
3. The magnetic quantum number, <em>m_l</em>, describes the orientation of the orbital in space. It can take values from -<em>l</em> to +<em>l</em>, including zero.
4. For the 2<em>p</em> subshell, where <em>l</em> = 1, the possible values for <em>m_l</em> are -1, 0, and +1.
5. Thus, the 2<em>p</em> subshell has three orbitals, each with the following quantum numbers: (2, 1, -1), (2, 1, 0), and (2, 1, +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. They include the principal quantum number (n), azimuthal quantum number (l), and magnetic quantum number (ml), which together provide information about the energy level, shape, and orientation of an orbital.

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 higher energy levels and greater distances from the nucleus. For the 2p subshell, n is 2.

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 equal to 1, indicating a specific shape (dumbbell) and the presence of three different orientations in space. Thus, for the 2p subshell, l is 1.