Statement I: The inner transition elements are placed in Group 3 B.
Statement II: The most stable oxidation state in case of the inner transition elements is +3.

Options

A. If both Statement I and Statement II are true and Statement II is the correct explanation of Statement I.
B. If both Statement I and Statement II are true but Statement II is not the correct explanation for Statement I.
C. If Statement I is true but Statement II is false.
D. If Statement I is false but Statement II is true.

Answer

To analyze the statements provided in the question, we will break down each statement and evaluate their validity step by step.

### Step 1: Evaluate Statement I
**Statement I:** The inner transition elements are placed in Group 3B.

**Analysis:**
- Inner transition elements refer to the f-block elements in the periodic table, which include the lanthanides (4f series) and actinides (5f series).
- These elements are typically placed below the main body of the periodic table and are often associated with Group 3B (or Group 3 in some notations).
- Therefore, this statement is **true**.

### Step 2: Evaluate Statement II
**Statement II:** The most stable oxidation state in case of the inner transition elements is +3.

**Analysis:**
- The inner transition elements, particularly the lanthanides and actinides, often exhibit a variety of oxidation states. However, +3 is indeed one of the most common and stable oxidation states for many of these elements.
- For lanthanides, +3 is the most stable oxidation state, while for actinides, +3 is also prevalent but other oxidation states can be significant as well.
- Hence, this statement is also **true**.

### Step 3: Determine the Relationship Between the Statements
- Both statements are true, but we need to assess if Statement II correctly explains Statement I.
- Statement I discusses the placement of inner transition elements in the periodic table, while Statement II discusses their oxidation states. The oxidation state does not explain their placement in the periodic table.
- Therefore, while both statements are true, Statement II is **not the correct explanation** of Statement I.

### Conclusion
- Both statements are true, but Statement II does not serve as a correct explanation for Statement I.

### Final Answer
- **Both statements are true, but Statement II is not the correct explanation of Statement I.**

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