"The number of radial node/s for $3 p$ orbital is :"

Question

Accepted Answer

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The number of radial nodes in an orbital is given by the formula:

$\text{Number of radial nodes} = n - l - 1$

where $n$ is the principal quantum number, $l$ is the azimuthal quantum number also known as the angular momentum quantum number.

For a $3p$ orbital,

$n = 3$ (since it is the 3rd energy level),

$l = 1$ (since $p$ orbitals correspond to $l = 1$).

Let's use the formula to determine the number of radial nodes:

$\text{Number of radial nodes} = 3 - 1 - 1 = 1$

So, the correct answer is: Option C : 1

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The number of radial node/s for $3 p$ orbital is :