Compounds of active metals `(Zn, Na, Mg)` are reducible by `H_(2)` whereas those of noble metals `(Cu,Ag,Au)` are not reducible.

Explanation

To determine whether the statement "Compounds of active metals (Zn, Na, Mg) are reducible by H₂ whereas those of noble metals (Cu, Ag, Au) are not reducible" is true or false, we can analyze the reduction potentials of these metals.

### Step-by-Step Solution:

1. **Understanding Reduction Potentials**:
- The ability of a substance to be reduced is determined by its reduction potential. A higher reduction potential means that the substance is more easily reduced.
- Hydrogen has a standard reduction potential of 0 V (in the form of H⁺ + e⁻ → H₂).

2. **Identifying Active Metals**:
- Active metals like Zinc (Zn), Sodium (Na), and Magnesium (Mg) have lower reduction potentials compared to hydrogen. This means they are more reactive and can displace hydrogen from acids.

3. **Identifying Noble Metals**:
- Noble metals like Copper (Cu), Silver (Ag), and Gold (Au) have higher reduction potentials than hydrogen. This means they are less reactive and cannot be reduced by hydrogen.

4. **Analyzing the Statement**:
- The statement claims that compounds of active metals are reducible by H₂. However, since active metals have lower reduction potentials than hydrogen, they cannot be reduced by hydrogen.
- Conversely, the statement claims that noble metals are not reducible by H₂, which is correct since they have higher reduction potentials.

5. **Conclusion**:
- Since the first part of the statement is false (active metals cannot be reduced by H₂), the overall statement is false.

### Final Answer:
The statement is **false**.