Statement I: Each f-block series contains 14 elements. 
Statement II: The f-orbitals can have seven possible orientations in space and can accommodate maximum of 14 electrons in the f-subshell. 

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 given statements regarding the f-block elements and their orbitals, we can break down the solution into the following steps:

### Step 1: Understanding the f-block Elements
The f-block elements are divided into two series: the lanthanides (6th period) and the actinides (7th period). Each series contains a total of 14 elements.

### Step 2: Confirming Statement I
Statement I claims that each f-block series contains 14 elements. This is true because:
- The lanthanide series includes elements from Cerium (Ce) to Lutetium (Lu), which totals 14 elements.
- The actinide series includes elements from Actinium (Ac) to Lawrencium (Lr), also totaling 14 elements.

### Step 3: Understanding f-orbitals
The f-orbitals can have a total of 7 different orientations in space. Each orientation can hold a maximum of 2 electrons.

### Step 4: Confirming Statement II
Statement II states that the f-orbitals can accommodate a maximum of 14 electrons. This is true because:
- Since there are 7 orientations and each can hold 2 electrons, the total number of electrons that can be accommodated in the f-subshell is:
\[ 7 \text{ orientations} \times 2 \text{ electrons/orientation} = 14 \text{ electrons} \]

### Conclusion
Both statements are correct:
- Statement I: Each f-block series contains 14 elements. (True)
- Statement II: The f-orbitals can have seven possible orientations in space and can accommodate a maximum of 14 electrons in the f-subshell. (True)

Thus, the final answer is that both statements are correct.

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