The element having atomic number Z = 107 and Z = 109 have been made recently, element Z = 108 has not yet been made. Indicate the group number in which you will place the above element.

Explanation

To determine the group number for the elements with atomic numbers Z = 107, Z = 108, and Z = 109, we will follow these steps:

### Step-by-Step Solution:

1. **Identify the Atomic Numbers**:
- We have three elements with atomic numbers Z = 107, Z = 108, and Z = 109.

2. **Determine the Electronic Configuration**:
- For Z = 107:
- The electronic configuration is:
\[ \text{Rn} \, (86) \, 5f^{14} \, 6d^5 \, 7s^2 \]
- For Z = 108:
- The electronic configuration can be assumed as:
\[ \text{Rn} \, (86) \, 5f^{14} \, 6d^6 \, 7s^2 \]
- For Z = 109:
- The electronic configuration is:
\[ \text{Rn} \, (86) \, 5f^{14} \, 6d^7 \, 7s^2 \]

3. **Identify the Block**:
- All three elements (Z = 107, 108, and 109) have their last electrons in the d orbital, indicating that they belong to the d-block of the periodic table.

4. **Determine the Group Number**:
- For d-block elements, the group number can be determined by counting the total number of electrons in the outermost d and s orbitals.
- For Z = 107:
- Total electrons in the outermost orbitals: \(5 (from \, 6d^5) + 2 (from \, 7s^2) = 7\)
- Therefore, it belongs to **Group 7**.
- For Z = 108:
- Total electrons in the outermost orbitals: \(6 (from \, 6d^6) + 2 (from \, 7s^2) = 8\)
- Therefore, it belongs to **Group 8**.
- For Z = 109:
- Total electrons in the outermost orbitals: \(7 (from \, 6d^7) + 2 (from \, 7s^2) = 9\)
- Therefore, it belongs to **Group 9**.

5. **Conclusion**:
- The group numbers for the elements are:
- Z = 107: Group 7
- Z = 108: Group 8
- Z = 109: Group 9

### Final Answer:
- Element Z = 107 is in **Group 7**.
- Element Z = 108 is in **Group 8**.
- Element Z = 109 is in **Group 9**.