What is the maximum number of electrons that can be accommodated in the subshell represented by following set of quantum numbers:
(i) n=2,l=1
(ii) n=5, l=3
(iii) n=3, l=2
(iv) n=6, l=0
Answers
Answer:
3 part .
Explanation:
No two electrons in an atom can have the same set of quantum numbers.
The first quantum number is the principle quantum number , which is
n=3
This means the electron is in the third energy level (shell).
The second quantum number, the angular momentum , is
l=2
and means the electron is in the
d sublevel (subshell).
The third quantum number, the magnetic quantum number ,
m
l
=2
represents one of the five
3d orbitals.
Lastly, we have the spin quantum number ,
m
s
=+1/2
It indicates the direction of the spin of the electron.
solution
In this case, the second energy level holds a total of
no. of orbitals
=
n
2
=
2
2
=
4
orbitals. Therefore, a maximum of
no. of electrons
=
2
⋅
4
=
8
electrons can share the quantum number
n
=
2
.
2
nd
set
→
n
=
4
,
l
=
3
This time, you are given both the energy level,
n
=
4
, and the subshell,
l
=
3
, on which the electrons reside.
similarly you can do all parts .
I hope this will help you