`CaH_(2)` and `BaH_(2)` are covalent in nature.

Explanation

To determine whether `CaH_(2)` (calcium hydride) and `BaH_(2)` (barium hydride) are covalent in nature, we can analyze the properties of alkaline earth metals and their hydrides step by step.

### Step-by-Step Solution:

1. **Identify the Elements**:
- Calcium (Ca) and Barium (Ba) are both alkaline earth metals, which belong to Group 2 of the periodic table.

2. **Understand the Trend in Group 2**:
- As we move down the group from Beryllium (Be) to Radium (Ra), the atomic size increases due to the addition of electron shells. This results in a decrease in the effective nuclear charge experienced by the outermost electrons.

3. **Polarizing Power**:
- According to Fajans' rules, the polarizing power of a cation (positively charged ion) decreases with increasing size. Larger cations have lower charge density, which means they exert less influence on the electron cloud of nearby anions (negatively charged ions).

4. **Covalent Character**:
- The covalent character of a compound increases with the polarizing power of the cation. Therefore, smaller cations (like Be²⁺ and Mg²⁺) have a higher covalent character in their hydrides compared to larger cations (like Ca²⁺ and Ba²⁺).

5. **Comparison of Hydrides**:
- The order of covalent character in the hydrides of alkaline earth metals is as follows:
- BeH₂ > MgH₂ > CaH₂ > SrH₂ > BaH₂
- This indicates that as we move down the group, the covalent character decreases.

6. **Conclusion**:
- Since both `CaH_(2)` and `BaH_(2)` are derived from larger cations (Ca²⁺ and Ba²⁺), they exhibit more ionic character rather than covalent character. Therefore, the statement that `CaH_(2)` and `BaH_(2)` are covalent in nature is false.

### Final Answer:
`CaH_(2)` and `BaH_(2)` are not covalent in nature; they are ionic.

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