The number of radial node/s for 3p orbital is:
- 1
- 4
- 2
- 3
The Correct Option is A
Approach Solution - 1
To determine the number of radial nodes in a 3p orbital, we need to understand the concept of radial nodes and how they are calculated for atomic orbitals.
Understanding Radial Nodes:
Radial nodes are regions where the probability of finding an electron is zero. They can be calculated using the formula:
\(N_{\text{radial}} = n - \ell - 1\)
where:
- \(n\) is the principal quantum number, and
- \(\ell\) is the azimuthal quantum number (angular momentum quantum number).
For a 3p orbital:
- The principal quantum number, \(n = 3\)
- Since it is a p orbital, \(\ell = 1\)
Substituting these values into the formula gives:
\(N_{\text{radial}} = 3 - 1 - 1 = 1\)
Thus, the number of radial nodes in a 3p orbital is 1.
Conclusion:
The correct answer is 1, which is consistent with the calculation based on quantum numbers. The remaining options (4, 2, 3) are incorrect because they do not align with the formula for radial nodes.
Approach Solution -2
The number of radial nodes for an orbital is given by the formula:
Number of radial nodes = n − l − 1
where: - n is the principal quantum number. - l is the azimuthal quantum number
(orbital angular momentum quantum number).
For a 3p orbital: - n = 3 - l = 1 (since it is a p-orbital)
Applying the formula:
Number of radial nodes = 3 − 1 − 1 = 1
Conclusion: The number of radial nodes for the 3p orbital is 1.
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