`XeO_(3)` is a trigonal pyramidal molecule .

Explanation

To determine whether the statement "XeO₃ is a trigonal pyramidal molecule" is correct, we can follow these steps:

### Step 1: Determine the number of valence electrons
- Xenon (Xe) has 8 valence electrons.
- Each oxygen (O) atom has 6 valence electrons. Since there are 3 oxygen atoms, the total contribution from oxygen is \(3 \times 6 = 18\) valence electrons.
- Therefore, the total number of valence electrons in XeO₃ is:
\[ 8 \, (\text{from Xe}) + 18 \, (\text{from 3 O}) = 26 \, \text{valence electrons} \]

### Step 2: Calculate the number of bond pairs and lone pairs
- To find the number of bond pairs and lone pairs, we can use the formula:
\[ \text{Number of bond pairs} = \frac{V - L}{2} \]
where \(V\) is the total number of valence electrons and \(L\) is the number of lone pairs.

- We can also calculate the number of bond pairs by dividing the total valence electrons by 8:
\[ \frac{26}{8} = 3 \quad \text{(quotient)} \quad \text{and remainder} = 2 \]
- The quotient (3) represents the number of bond pairs.
- The remainder (2) indicates that there is 1 lone pair (since each lone pair counts as 2).

### Step 3: Determine the hybridization and molecular shape
- With 3 bond pairs and 1 lone pair, the hybridization of the molecule is \(sp^3\).
- The presence of one lone pair affects the molecular geometry. The arrangement of the electron pairs is tetrahedral, but the molecular shape is determined by the positions of the atoms only.
- With 3 bonded atoms and 1 lone pair, the molecular shape is trigonal pyramidal.

### Conclusion
- The statement "XeO₃ is a trigonal pyramidal molecule" is correct.

### Final Answer
Therefore, the statement is **true**.