The number of nodes in `3p` orbital

Options

A. 1
B. 2
C. 3
D. 4

Explanation

To find the number of nodes in a 3p orbital, we can follow these steps:

### Step 1: Identify the Principal Quantum Number (n)
The principal quantum number (n) for the 3p orbital is 3.

### Step 2: Identify the Angular Quantum Number (l)
For a p orbital, the angular quantum number (l) is 1.

### Step 3: Calculate the Number of Radial Nodes
The formula for calculating the number of radial nodes is given by:
\[ \text{Radial Nodes} = n - l - 1 \]
Substituting the values:
\[ \text{Radial Nodes} = 3 - 1 - 1 = 1 \]

### Step 4: Calculate the Number of Angular Nodes
The number of angular nodes is equal to the value of l:
\[ \text{Angular Nodes} = l = 1 \]

### Step 5: Calculate the Total Number of Nodes
The total number of nodes is the sum of radial nodes and angular nodes:
\[ \text{Total Nodes} = \text{Radial Nodes} + \text{Angular Nodes} = 1 + 1 = 2 \]

### Final Answer
The number of nodes in a 3p orbital is **2**.

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