Question

The nodes present in 5p-orbital are:
A.One planar, five spherical
B.One planar, four spherical
C.One planar, three spherical
D.Four spherical

Answer 1

Hint:To approach this question, we should be aware of the four types of quantum numbers. We should also know the relation between the number of nodes and quantum numbers. Planar node is the plane where the probability of finding \[{e^ - }\]is zero.

Formula used:n= principal quantum number
Total number of nodes=n-1

Complete step-by-step answer:In 5p-orbital,
n= 5
For p orbital, azimuthal quantum number, l=1
 Total number of nodes= n- 1 = 5-1 =4
Angular nodes= value of azimuthal quantum number (l) = 1
Here, Number of angular nodes= number of planar nodes That is, l=1
So, for 5p- orbital, number of planar nodes is one.
Number of spherical nodes=n-1-1 =5-1-1 =3
So in 5p-orbital, there is one planar node and three spherical nodes. Hence, option C is correct answer to the given question.

Additional information:

Orbital	Shape
s-orbital	Spherical
p-orbital	Clover/ dumbbell
d-orbital	Double dumbbell shape

This shape is decided on the basis of the angular quantum number.

Note:Number of radial nodes can also be determined using these values. The formula that will be used here is one unit less than the number of total nodes. The formula is:
Number of radial nodes= total number of nodes-1
In this question, for 5p-orbital, number of radial nodes =4-1 =3