Select a correct set of values for an electron found within the designated 5d orbital.

• A. n = 5, l = 2, m_l = 0
• B. n = 5, l = 3, m_l = +1
• C. n = 5, l = 3, m_l = 0
• D. n = 5, l = 5, m_l = – 2
• E. n = 5, l = 2, m_l = +5

Answer: (A)

Verified step by step guidance

1. Understand the quantum numbers: Quantum numbers are used to describe the properties of atomic orbitals and the electrons in those orbitals. The principal quantum number (n) indicates the energy level, the azimuthal quantum number (l) indicates the shape of the orbital, and the magnetic quantum number (ml) indicates the orientation of the orbital.
2. Identify the principal quantum number (n): For a 5d orbital, the principal quantum number is n = 5. This indicates that the electron is in the fifth energy level.
3. Determine the azimuthal quantum number (l): The azimuthal quantum number for d orbitals is l = 2. This number defines the shape of the orbital, and for d orbitals, it is always 2.
4. Find the possible values for the magnetic quantum number (ml): The magnetic quantum number can range from -l to +l, including zero. For l = 2, the possible values for ml are -2, -1, 0, +1, and +2.
5. Select the correct set of values: Based on the quantum numbers for a 5d orbital, the correct set of values is n = 5, l = 2, ml = 0, as this matches the criteria for a 5d orbital and the image provided highlights ml = 0.