How many radial and angular nodes are present in 2p orbital.

Answer

To determine the number of radial and angular nodes in a 2p orbital, we can follow these steps:

### Step 1: Identify the principal quantum number (n) and the azimuthal quantum number (l).
- For the 2p orbital, the principal quantum number \( n = 2 \).
- The azimuthal quantum number \( l \) for a p orbital is \( l = 1 \).

### Step 2: Calculate the number of radial nodes.
- The formula for calculating radial nodes is given by:
\[ \text{Radial Nodes} = n - l - 1 \]
- Substituting the values:
\[ \text{Radial Nodes} = 2 - 1 - 1 = 0 \]
- Therefore, there are **0 radial nodes** in the 2p orbital.

### Step 3: Calculate the number of angular nodes.
- The formula for calculating angular nodes is:
\[ \text{Angular Nodes} = l \]
- Since \( l = 1 \) for the 2p orbital:
\[ \text{Angular Nodes} = 1 \]
- Therefore, there is **1 angular node** in the 2p orbital.

### Final Answer:
- The 2p orbital has **0 radial nodes** and **1 angular node**.

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