Assertion : `C_(3)O_(2)` is non-polar molecule.
Reason : Terminal `pi-bonds of the molecule are lying in different planes.

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 and the reason is not the correct explanation of assertion

Answer

To analyze the assertion and reason provided, we will go through the following steps:

### Step 1: Understanding the Assertion
The assertion states that \( C_3O_2 \) is a non-polar molecule. To evaluate this, we need to consider the molecular geometry and the distribution of charges within the molecule.

### Step 2: Drawing the Structure of \( C_3O_2 \)
The structure of \( C_3O_2 \) can be represented as follows:
- The molecule consists of three carbon atoms connected by double bonds, with the terminal carbon atoms bonded to oxygen atoms through double bonds.
- The structure can be depicted as:
\[ C=C=C=O \]
where the terminal carbon (C) is double-bonded to oxygen (O).

### Step 3: Analyzing Electronegativity
In \( C_3O_2 \), oxygen is more electronegative than carbon. This means that the oxygen atoms will attract the shared electrons in the double bonds more strongly than the carbon atoms. As a result, there will be a partial negative charge on the oxygen atoms and a partial positive charge on the carbon atoms, leading to a dipole moment.

### Step 4: Conclusion on the Assertion
Since there is an unequal distribution of charge due to the electronegativity difference, \( C_3O_2 \) is a polar molecule. Therefore, the assertion that \( C_3O_2 \) is non-polar is **false**.

### Step 5: Understanding the Reason
The reason states that the terminal pi-bonds of the molecule are lying in different planes. To evaluate this, we need to analyze the geometry of the molecule.

### Step 6: Analyzing the Molecular Geometry
In the structure of \( C_3O_2 \):
- The terminal pi-bonds (C=O) are indeed oriented in different planes due to the arrangement of the p-orbitals involved in bonding.
- The p-orbitals of the carbon atoms and oxygen atoms can be oriented such that the pi-bonds are not in the same plane.

### Step 7: Conclusion on the Reason
The reason provided is **true** because the terminal pi-bonds are indeed lying in different planes.

### Final Conclusion
- The assertion is **false**: \( C_3O_2 \) is a polar molecule.
- The reason is **true**: The terminal pi-bonds are lying in different planes.
- Therefore, the reason does not provide a correct explanation for the assertion.