Which of the following is a correct set of values for the magnetic quantum number, m, for one of the subshells when n = 2?

• A. m = -1, +1
• B. m = -2, -1, 0, +1, +2
• C. m = -1, 0, +1
• D. m = 0, +1, +2

Answer: (C)

Verified step by step guidance

1. Recall that the principal quantum number \(n\) determines the energy level and the possible subshells (values of the azimuthal quantum number \(l\)) within that level. For \(n = 2\), the possible values of \(l\) are \$0\( and \)1$.
2. Understand that the magnetic quantum number \(m\) depends on \(l\) and can take integer values from \(-l\) to \(+l\), including zero. So for each \(l\), \(m\) ranges as \(m = -l, -(l-1), ..., 0, ..., (l-1), +l\).
3. For \(n = 2\), when \(l = 0\) (the 2s subshell), \(m\) can only be \$0\( because \)m\( ranges from \)-0\( to \)+0$.
4. For \(n = 2\), when \(l = 1\) (the 2p subshell), \(m\) can be \(-1\), \$0\(, or \)+1\( because \)m\( ranges from \)-1\( to \)+1$.
5. Compare the given options with the allowed \(m\) values for \(l = 1\) at \(n = 2\). The correct set of \(m\) values for a subshell at \(n = 2\) is \(m = -1, 0, +1\).