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

🧠 The Spherical Gaps Radial nodes are the "empty shells" within an orbital where the probability of finding an electron drops to zero. They occur as the wave function crosses the axis along the radius.

🗺️ The Node Count

1. Identify Quantum Numbers: For a 3p orbital:
   • Principal shell ($n$) = 3
   • Azimuthal/Angular ($l$) = 1 (for 'p')
2. Apply the Formula: $\text{Radial Nodes} = n - l - 1$ $\text{Radial Nodes} = 3 - 1 - 1 = 1$

⚡ The "Total Nodes" Check Remember that Total Nodes always equals $n-1$. For 3p: Total $= 3-1 = 2$. Since Angular Nodes $= l = 1$, the remaining $1$ node must be radial!

⚠️ Common Traps Confusing radial nodes with angular nodes (which is simply $l$). A 3p orbital has 1 of each, summing to $2$ nodes total.

$\boxed{\text{Answer: (a)}}$