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With n=2 you could have l= 0 or 1. If your l=0, then your ml can only=0 (this is one orbital). Since l can also equal 1, your ml can be -1,0,+1. This corresponds to 3 more orbitals so the total number of orbitals would be 4.
n=2 can either be the 2s or 2p subshell. The 2s subshell has 1 orbital while the 2p subshell has 3 orbitals. Since it asks for the general principal quantum number of n=2, we must take into account 2s and 2p so we add 1 orbital + 3 orbitals to get 4 possible orbitals.
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