Assertion : ` C Cl_(4)` is a non-polar molecule.
Reason : `C Cl_(4)` has polar bonds.

Options

A. If assertion is true but the reason is false
B. If assertion is false but reason is true
C. IF both assertion and reason are true and the reason is the correct explanation of assertion
D. If both assertion and reason are true but reason is not the correct explanation of assertion

Answer

To solve the question regarding the assertion and reason about CCl₄ (carbon tetrachloride), we will break down the concepts step by step.

### Step 1: Understand the Assertion
The assertion states that CCl₄ is a non-polar molecule. To evaluate this, we need to consider the molecular geometry and symmetry of CCl₄.

**Hint:** Look at the molecular structure and symmetry to determine polarity.

### Step 2: Determine the Geometry of CCl₄
CCl₄ has a tetrahedral geometry due to the sp³ hybridization of the carbon atom. This means that the four chlorine atoms are arranged symmetrically around the central carbon atom.

**Hint:** Remember that the shape of the molecule plays a crucial role in determining its polarity.

### Step 3: Analyze the Bonds in CCl₄
Each C-Cl bond is polar because chlorine is more electronegative than carbon. This creates a dipole moment in each bond, with chlorine carrying a partial negative charge (δ-) and carbon carrying a partial positive charge (δ+).

**Hint:** Consider the electronegativity values of the atoms involved to assess bond polarity.

### Step 4: Evaluate the Overall Polarity
Even though CCl₄ has polar bonds, the symmetrical tetrahedral shape means that the dipole moments of the four C-Cl bonds cancel each other out. This results in a net dipole moment of zero, making the molecule non-polar.

**Hint:** Think about how the arrangement of polar bonds affects the overall dipole moment.

### Step 5: Understand the Reason
The reason states that CCl₄ has polar bonds. This statement is true because of the difference in electronegativity between carbon and chlorine.

**Hint:** Identify whether the reason provides a valid explanation for the assertion.

### Step 6: Conclusion
Both the assertion and the reason are true:
- The assertion (CCl₄ is a non-polar molecule) is true because the dipole moments cancel out due to symmetry.
- The reason (CCl₄ has polar bonds) is also true, but it does not explain why CCl₄ is non-polar.

Therefore, the correct conclusion is that both the assertion and the reason are true, but the reason is not the correct explanation for the assertion.

### Final Answer
Both the assertion and the reason are true, but the reason is not the correct explanation for the assertion.