Radial nodes present in 3s and 3p - orbitals are respectively

Options

A. 0,2
B. 2,1
C. 1,1
D. 2,2

Answer

To determine the number of radial nodes present in the 3s and 3p orbitals, we can use the formula for calculating the number of radial nodes:

**Formula:**
Number of radial nodes = n - l - 1

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

### Step-by-Step Solution:

1. **Identify the Principal Quantum Number (n):**
- For both 3s and 3p orbitals, the principal quantum number (n) is 3.

2. **Determine the Azimuthal Quantum Number (l):**
- For the s orbital (3s), the azimuthal quantum number (l) is 0.
- For the p orbital (3p), the azimuthal quantum number (l) is 1.

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

4. **Calculate the Number of Radial Nodes for 3p Orbital:**
- Using the formula:
\[ \text{Number of radial nodes in 3p} = n - l - 1 \]
- Substitute the values:
\[ \text{Number of radial nodes in 3p} = 3 - 1 - 1 = 1 \]

5. **Final Result:**
- The number of radial nodes in the 3s orbital is 2.
- The number of radial nodes in the 3p orbital is 1.

### Conclusion:
- The number of radial nodes present in the 3s and 3p orbitals are respectively **2 and 1**.

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