The number of orbital nodes of `3s` and `2p` orbital are, respectively

Options

A. `2,0`
B. `0,2`
C. `1,7`
D. `2,11`

Explanation

To determine the number of orbital nodes for the 3s and 2p orbitals, we can use the formula:

**Number of Orbital Nodes = n - l - 1**

Where:
- **n** = principal quantum number
- **l** = azimuthal quantum number

### Step-by-Step Solution:

1. **Identify the quantum numbers for the 3s orbital:**
- For the 3s orbital, the principal quantum number (n) is 3.
- The azimuthal quantum number (l) for an s orbital is 0 (since s corresponds to l = 0).

2. **Calculate the number of nodes for the 3s orbital:**
- Using the formula: Number of Orbital Nodes = n - l - 1
- Substitute the values:
\[ \text{Number of Nodes for 3s} = 3 - 0 - 1 = 2 \]

3. **Identify the quantum numbers for the 2p orbital:**
- For the 2p orbital, the principal quantum number (n) is 2.
- The azimuthal quantum number (l) for a p orbital is 1 (since p corresponds to l = 1).

4. **Calculate the number of nodes for the 2p orbital:**
- Using the same formula: Number of Orbital Nodes = n - l - 1
- Substitute the values:
\[ \text{Number of Nodes for 2p} = 2 - 1 - 1 = 0 \]

5. **Final Result:**
- The number of orbital nodes for the 3s orbital is 2.
- The number of orbital nodes for the 2p orbital is 0.

### Summary:
- Number of nodes for 3s = 2
- Number of nodes for 2p = 0

### Answer:
The number of orbital nodes of 3s and 2p orbitals are, respectively, **2 and 0**.

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