Question

The number of spherical nodes angular nodes and nodal planes for pz is

Answer 1

Answer:

The quantum number ℓ determines the number of angular nodes; there is 1 angular node, specifically on the xy plane because this is a pz orbital. Because there is one node left, there must be one radial node. To sum up, the 3pz orbital has 2 nodes: 1 angular node and 1 radial node

Explanation:

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Answer 2

(There is an error in the question. The shell number should also be mentioned. The correct question will be read as: The number of spherical nodes, angular nodes and nodal planes for $\[3{p_z}\]$ is)

Given:

$\[3{p_z}\]$ orbital

To Find: Number of spherical nodes, angular nodes and nodal planes

Solution:

The formula for calculating spherical nodes is given as:

Spherical or radial nodes $\[ = n - l - 1\]$

where, $n=$ principal quantum number and $l=$ azimuthal number

The formula for angular nodes and nodal planes are

Angular nodes $\[ = l\]$

Nodal planes $\[ = l\]$

For $\[3{p_z}\]$ orbital: $\[n = 3,\,l = 1\]$

Therefore,

Spherical nodes $\[ = 3 - 1 - 1\]$

Spherical nodes $\[ = 1\]$

Angular nodes $\[ = l = 1\]$

Nodal planes $\[ = l = 1\]$

Hence, the number of spherical nodes, angular nodes and nodal planes for $\[3{p_z}\]$ is $\[1,\,1\]$ and $1$.

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