Question

Define the quantum numbers n, l, m_l, s, and m_s .

a) n - Principal quantum number; l - Azimuthal quantum number; m_l - Magnetic quantum number; s - Spin quantum number; m_s - Secondary magnetic quantum number.

b) n - Principal quantum number; l - Orbital quantum number; m_l - Magnetic quantum number; s - Spin quantum number; m_s - Spin magnetic quantum number.

c) n - Principal quantum number; l - Angular momentum quantum number; m_l - Magnetic quantum number; s - Spin quantum number; m_s - Spin magnetic quantum number.

d) n - Principal quantum number; l - Linear momentum quantum number; m_l - Magnetic quantum number; s - Spin quantum number; m_s - Secondary magnetic quantum number.

Answer 1

The correct definitions of the quantum numbers are: n is the principal quantum number, l is the angular momentum quantum number, m_l is the magnetic quantum number, s is the spin quantum number, and m_s is the spin magnetic quantum number.

Step-by-step explanation:

The correct option that defines the quantum numbers is:

(c) n - Principal quantum number; l - Angular momentum quantum number; ml - Magnetic quantum number; s - Spin quantum number; ms - Spin magnetic quantum number.

This can be broken down as follows:

• The principal quantum number (n) specifies the energy level of an electron in an atom and is a positive integer (n = 1, 2, 3, ...).
• The angular momentum quantum number (l) defines the shape of the electron's orbital and can take on integer values from 0 to n - 1.
• The magnetic quantum number (ml) describes the orbital's orientation in space, and it can range between -l to +l, including zero.
• The spin quantum number (s) defines the intrinsic spin of the electron and is always equal to 1/2.
• The spin magnetic quantum number (ms) indicates the direction of the electron's spin and can be either +1/2 or -1/2.