Statement-I : 2p orbitals do not have spherical nodes.
Because
Statement-II : The number of spherical nodes in p-orbitals is given by `(n-2)`

Options

A. Statement-I is true, Statement-II is true, Statement-II is correct explanation for Statement-I.
B. Statement-I is true, Statement-II is true , Statement-II is NOT a correct explanation for statement-I
C. Statement-I is true, Statement-II is false
D. Statement-I is false, Statement-II is true

Answer

To solve the question, we need to analyze both statements and determine their validity.

### Step 1: Understand Statement-I
**Statement-I:** 2p orbitals do not have spherical nodes.

- The 2p orbital is characterized by the principal quantum number \( n = 2 \) and the azimuthal quantum number \( l = 1 \) (since it's a p orbital).
- Spherical nodes are regions where the probability of finding an electron is zero and are determined by the formula for the number of spherical nodes, which is given by \( n - 1 - l \).

### Step 2: Calculate the Number of Spherical Nodes for 2p
Using the formula for spherical nodes:
- For the 2p orbital, \( n = 2 \) and \( l = 1 \).
- Plugging in these values into the formula:
\[ \text{Number of spherical nodes} = n - 1 - l = 2 - 1 - 1 = 0 \]
- This means that the 2p orbital has 0 spherical nodes.

### Step 3: Understand Statement-II
**Statement-II:** The number of spherical nodes in p-orbitals is given by \( n - 2 \).

- We can verify this by substituting \( n \) into the formula for spherical nodes.
- For p orbitals, we already calculated that the number of spherical nodes is \( n - 1 - l \).
- Since \( l = 1 \) for p orbitals, we can rewrite it as:
\[ n - 1 - 1 = n - 2 \]
- This confirms that Statement-II is also correct.

### Step 4: Conclusion
Both statements are true:
- Statement-I is true because the 2p orbital indeed has 0 spherical nodes.
- Statement-II is true as it correctly describes the number of spherical nodes for p orbitals.

### Final Answer
Both statements are correct, and Statement-II provides the correct explanation for Statement-I.