The analogous `CF_(6)^(2-)` anion does not exist. The reason is :

Answer

To understand why the analogous \( CF_6^{2-} \) anion does not exist, we can break down the reasoning into two main points:

### Step 1: Lack of Vacant d Orbitals
- **Explanation**: Carbon has the electronic configuration \( 1s^2 2s^2 2p^2 \). It does not have any vacant d orbitals available for bonding or accepting additional electrons. This is crucial because many larger elements can form stable complexes by utilizing their d orbitals to accommodate extra electron pairs.

### Step 2: Small Size of Carbon
- **Explanation**: The atomic size of carbon is relatively small. This small size makes it difficult for carbon to accommodate six fluorine atoms around it. Fluorine is a highly electronegative element and requires significant space to bond. The steric hindrance and the repulsion between the fluorine atoms would make the formation of \( CF_6^{2-} \) unstable.

### Conclusion
- **Final Statement**: Therefore, the combination of the absence of vacant d orbitals and the small atomic size of carbon prevents the formation of the \( CF_6^{2-} \) anion.