Question

the number of radial nodes, nodal planes for an orbital with n=4,l=1 is​

Answer 1

Answer:

The number of nodal planes is equal to the value of the angular momentum quantum number, l. The 2s has one radial node and the 3s has two radial nodes. 3p have one radial node. In general, the number of radial nodes is equal to n – l - 1.

Answer 2

The radial nodes are 2 and nodal planes are 1 for n=4 and l=1

Explanation:

Principle Quantum Numbers : It describes the size of the orbital and the energy level. It is represented by n. Where, n = 1,2,3,4....

Azimuthal Quantum Number : It describes the shape of the orbital. It is represented as 'l'. The value of l ranges from 0 to (n-1). For l = 0,1,2,3... the orbitals are s, p, d, f...

To find the number of nodes:

total number of nodes = n−1.

angular nodes = nodal planes = ℓ

radial nodes=(number of nodes)−(angular nodes)

For n = 4,  total number of nodes = 4−1 = 3

For l= 1, angular nodes= 1

Thus radial nodes = (n-1)-l= (4-1)-1= 3-1 = 2

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