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For the 3p orbital of hydrogen, what is the total number of nodes (radial + angular)?

1. 1
2. 2
3. 3
4. 4

Correct answer: 2

Solution

For any orbital with quantum numbers n and l: number of radial nodes = n - l - 1, number of angular nodes = l, and total nodes = n - 1. For the 3p orbital: n = 3, l = 1. Radial nodes = 3 - 1 - 1 = 1. Angular nodes = 1. Total nodes = 3 - 1 = 2. The [R(r)]² vs r graph for 3p orbital shows one radial node (one point where the radial function crosses zero, not counting r = 0 and r = infinity).

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