Statement-1 : The `5^(th)` period of periodic table contains 18 elements not 32.
Statement-2 : n=5,l=0,1,2,3. The order in which the energy of available orbitals 4d, 5s, 5p increases is `5slt4dlt5p` and the total number of orbitals available are 9 and thus 18 electrons can be accomodated.

Options

A. Statement-1 is True, Statement-2 is True, Statement-2 is a correct explanation for Statement-1
B. Statement-1 is True, Statement-2 is True, Statement-2 is NOT a correct explanation for Statement-1
C. Statement-1 is True, Statement-2 is False.
D. Statement-1 is False, Statement-2 is True.

Explanation

To solve the question, we need to analyze both statements provided and verify their correctness.

### Step 1: Analyze Statement 1
**Statement 1:** The 5th period of the periodic table contains 18 elements, not 32.

- The 5th period corresponds to the principal quantum number \( n = 5 \).
- In the 5th period, the following orbitals are filled:
- \( 5s \) (1 orbital)
- \( 4d \) (5 orbitals)
- \( 5p \) (3 orbitals)

**Calculation of total orbitals:**
- Total orbitals = 1 (from \( 5s \)) + 5 (from \( 4d \)) + 3 (from \( 5p \)) = 9 orbitals.

**Calculation of total electrons:**
- Each orbital can hold a maximum of 2 electrons.
- Therefore, total electrons = \( 9 \text{ orbitals} \times 2 \text{ electrons/orbital} = 18 \text{ electrons} \).

Thus, the 5th period contains 18 elements, confirming that Statement 1 is **correct**.

### Step 2: Analyze Statement 2
**Statement 2:** The order in which the energy of available orbitals \( 4d, 5s, 5p \) increases is \( 5s < 4d < 5p \).

- According to the \( n + l \) rule:
- For \( 5s \): \( n + l = 5 + 0 = 5 \)
- For \( 4d \): \( n + l = 4 + 2 = 6 \)
- For \( 5p \): \( n + l = 5 + 1 = 6 \)

Since both \( 4d \) and \( 5p \) have the same \( n + l \) value, we compare their \( n \) values:
- \( 5s \) has the lowest energy, followed by \( 4d \) and then \( 5p \).

Thus, the correct order of increasing energy is indeed \( 5s < 4d < 5p \), confirming that Statement 2 is also **correct**.

### Step 3: Conclusion
Both statements are correct, and Statement 2 provides a correct explanation for Statement 1.

### Final Answer
The answer to the question is: **Both statements are true, and Statement 2 is a correct explanation of Statement 1.**

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