Answer:
Sol. n = 3
...(i)
\[l=0,1,2,........(n-1)\]
\[\therefore \] \[l=0,1,2\]
\[l=0;\,\,{{m}_{1}}=0\]
\[l=1;\,\,{{m}_{1}}=-1,0,+1\]
\[l=2;\,\,{{m}_{1}}=-2,-1,0,+1,+2\]
(ii) List the quantum numbers (\[{{m}_{l}}\]
and \[l\]) of electrons for 3d orbital.
Sol: 3d: l = 2 for d-subshell
\[m=-l,.....0.....+l\]
\[=-2,-1,0,+1,+2\]
(iii) Which of the following orbitals
are possible?
\[1p,2s,2p\] and \[3f\]
Sol: 2s and \[2p\]-orbitals are possible
while \[1p\] and \[3f\] orbitals are not possible.
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