Asseration: `SeCl_(4)`, does not havea tetrahedral structure.
Reason: `Se` in `SeCl_(4)` has two lone pairs.

Explanation

To solve the question regarding the assertion and reason provided, we will analyze both statements step by step.

### Step 1: Analyze the Assertion
The assertion states that SeCl₄ does not have a tetrahedral structure.

- **Explanation**: The molecular geometry of SeCl₄ can be determined by considering the number of bonding pairs and lone pairs around the central selenium (Se) atom. Selenium is in group 16 and can expand its octet. In SeCl₄, selenium is bonded to four chlorine atoms.

### Step 2: Determine the Electron Configuration
To understand the bonding in SeCl₄, we need to look at the electron configuration of selenium.

- **Explanation**: Selenium has an atomic number of 34, and its electron configuration is [Ar] 4s² 4p⁴. In the formation of SeCl₄, selenium can promote one of its 4p electrons to a higher energy level, allowing it to form four bonds with chlorine atoms.

### Step 3: Count Lone Pairs
Next, we need to determine how many lone pairs are present on the selenium atom in SeCl₄.

- **Explanation**: After forming four bonds with chlorine, selenium will have one lone pair remaining. This means that there are not two lone pairs as stated in the reason.

### Step 4: Determine the Molecular Geometry
Now, we can determine the molecular geometry based on the number of bonding pairs and lone pairs.

- **Explanation**: With four bonding pairs and one lone pair, the electron geometry is trigonal bipyramidal, and the molecular shape is seesaw. This confirms that SeCl₄ does not have a tetrahedral structure.

### Conclusion
- The assertion is **correct**: SeCl₄ does not have a tetrahedral structure.
- The reason is **incorrect**: Se in SeCl₄ has one lone pair, not two.

### Final Answer
- Assertion: True
- Reason: False

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