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The following quantum numbers are possible for how many orbitals: n = 3, l = 2, m = +2
A
1
B
2
C
3
D
4
Detailed Solution
The three quantum numbers n, l and $m_l$ together specify exactly one orbital.
n = 3, l = 2 is the 3d subshell, which has five orbitals with $m_l$ = –2, –1, 0, +1, +2.
Only one of these has $m_l = +2$.
So the given quantum numbers are possible for 1 orbital (which can hold 2 electrons with $m_s = \pm\dfrac{1}{2}$).
n = 3, l = 2 is the 3d subshell, which has five orbitals with $m_l$ = –2, –1, 0, +1, +2.
Only one of these has $m_l = +2$.
So the given quantum numbers are possible for 1 orbital (which can hold 2 electrons with $m_s = \pm\dfrac{1}{2}$).