Question

Complete the table by pairing each set of quantum numbers with the orbital it describes. If the set of quantum numbers is not possible, label it as not allowed. Use each orbital description as many times as necessary.

Orbital	Quantum numbers
	?=1,ℓ=1,?ℓ=0n=1,ℓ=1,mℓ=0
	?=4,ℓ=2,?ℓ=2n=4,ℓ=2,mℓ=2
	?=2,ℓ=1,?ℓ=−1n=2,ℓ=1,mℓ=−1
	?=3,ℓ=2,?ℓ=−3n=3,ℓ=2,mℓ=−3
	?=5,ℓ=3,?ℓ=1n=5,ℓ=3,mℓ=1

Answer 1

Orbital	Quantum numbers
not allowed	?=1,ℓ=1,?ℓ=0n=1,ℓ=1,mℓ=0
4d	?=4,ℓ=2,?ℓ=2n=4,ℓ=2,mℓ=2
2p	?=2,ℓ=1,?ℓ=−1n=2,ℓ=1,mℓ=−1
not allowed	?=3,ℓ=2,?ℓ=−3n=3,ℓ=2,mℓ=−3
5f	?=5,ℓ=3,?ℓ=1n=5,ℓ=3,mℓ=1

Explanation :

n = principle quantum number

l = n - 1 .

l < n .

ml = 2l + 1

if l = 2 , then possible ml values are : - 2 , -1 , 0 , 1 , 2

l = 0 : s-orbital

l = 1 : p-orbital

l = 2 : d-orbital

l = 3 : f- orbital