The number of angular nodes and radial nodes is 3s orbital are

Options

A. 1 and 0, respectively
B. 3 and 0, respectively
C. 0 and 1, respectively
D. 0 and 2, respectively

Explanation

To determine the number of angular nodes and radial nodes in a 3s orbital, we can follow these steps:

### Step 1: Identify the Principal Quantum Number (n) and Azimuthal Quantum Number (l)
- The principal quantum number (n) for the 3s orbital is **3**.
- The azimuthal quantum number (l) for an s orbital is **0** (since s corresponds to l = 0).

### Step 2: Calculate the Number of Angular Nodes
- The formula for calculating the number of angular nodes is given by:
\[ \text{Number of Angular Nodes} = l \]
- Since l = 0 for the s orbital, we have:
\[ \text{Number of Angular Nodes} = 0 \]

### Step 3: Calculate the Number of Radial Nodes
- The formula for calculating the number of radial nodes is given by:
\[ \text{Number of Radial Nodes} = n - l - 1 \]
- Substituting the values of n and l:
\[ \text{Number of Radial Nodes} = 3 - 0 - 1 = 2 \]

### Conclusion
- Therefore, for the 3s orbital:
- **Number of Angular Nodes = 0**
- **Number of Radial Nodes = 2**

### Final Answer
The number of angular nodes in a 3s orbital is **0**, and the number of radial nodes is **2**.

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