What orbitals do each respective quantum number fit into?

• n=2, l=0
• n=3, l=2
• n=4, l=1
• n=4, l=2

a) n=2, l=0 => 2s orbital

b) n=3, l=2 => 3d orbital

c) n=4, l=1 => 4p orbital

d) n=4, l=2 => 4d orbital

Step-by-step explanation

Principal Quantum number (n) :

•it determines the size of orbitals

and how far the electron is present from the nucleus.

• large size of orbitals represents large size of an atom.

• It's values can be 1,2,3,4.....

• n = 1 represents first principle shell or lowest energy state.

Similarly,

n = 2 second principle shell.

• n = 0 is not possible. Because it is not possible for an atom to have no value for principle quantum number.

Azimuthal quantum number (L) :

• it determines the shape of an orbital.

If L= 0 then shape = s

If L = 1 then shape = p

If L = 2 then shape = d

If L = 3 then shape = f

Hence,

a) If n = 2 and L = 0

then orbital will be : 2s

b) if n = 3 and L = 2

then orbital = 3d

c) if n = 4 and L = 1

then orbital = 4p

d) if n = 4 and L = 2

then orbital = 4d