Calculate the angular and radial node of 4d and 4s orbital
Answers
Answer:
4 is the angular node
d and s are radial node.
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Explanation:
\h
Given:−
Orbitals are 3p , 4d , 4s
\huge {\bold {\underline {\underline{To \: find : - }}}}
Tofind:−
Total number of Angular and radial nodes of orbitals 3p , 4d , 4s
\huge {\bold {\underline {\underline{Solution : - }}}}
Solution:−
Number of Angular nodes of the orbital is given by ,
\large {\bold {\boxed{ \bigstar{ | {N}_{A} = l | }}}}
★∣N
A
=l∣
Where ,
l is azimuthal quantum number
Number of radial nodes of the orbital is given by ,
\large {\bold {\boxed{ \bigstar{ | {N}_{R} = n - l - 1 | }}}}
★∣N
R
=n−l−1∣
Where ,
n is principal quantum number
l is azimuthal quantum number
Fist let us calculate the angular and Radial nodes for ,
3d
4d
4s
i] 3d
a) Number of angular nodes
l value of 3d = 2
∴ Number of angular nodes for 3d-subshell is 2
b) Number of Radial nodes
n- Value for 3d subshell = 3
l - value for 3d subshell = 2
Number of radial nodes = 3 - 2 - 1 = 0
∴ Number of radial nodes for 3d subshell is 0
ii] 4d
a) Number of angular nodes
l - value for 4d orbital = 2
∴ Number of angular nodes for 4d subshell is 2
b) Number of radial nodes
n-value for 4d orbital = 4
l - value for 4d orbital = 2
∴ Number of radial nodes for 4d subshell = 4 - 2 - 1 = 3
iii] 4s
a) Number of angular nodes
l - value for 4s subshell = 0
∴ Number of angular nodes for 4s subshell = 0
b) Number of radial nodes
n - value for 4s subshell = 4
l - Value for 4s subshell = 0
∴ Number of radial nodes for 4s subshell = 4 - 0 - 1 = 3