Question

The correct set of four quantum numbers for an electron in a 4d subshell is: 
 

• A. 4, 2, 1, \(-\frac{1}{2}\)
• B. 4, 2, 1, 0
• C. 4, 3, 2, \(-\frac{1}{2}\)
• D. 4, 3, -2, \(-\frac{1}{2}\)

Hint:

Quantum numbers are fundamental to understanding electron configurations in atoms. Each number has specific ranges based on the type of orbital (s, p, d, f) considered.

Answer 1

The Correct Option is A

For an electron in the 4d subshell: - The principal quantum number (n) for the 4th shell is 4.
- The azimuthal quantum number (l) for the d subshell is 2.
- The magnetic quantum number (m_l) can range from -l to +l, which for d is -2 to +2. The given value 1 is within this range.
- The spin quantum number (m_s) has possible values of \(-\frac{1}{2}\) or \(\frac{1}{2}\). Here, it is \(-\frac{1}{2}\).
These values correctly represent an electron in a 4d subshell, making option (1) the correct set of quantum numbers.