Question:
Select the 'WRONG' statement about polar molecules.
Select the 'WRONG' statement about polar molecules.
Show Hint
A polar molecule has a lopsided charge distribution, so its shape is not symmetrical.
Updated On: Oct 1, 2026
- A molecule in which centre of mass of positive charges does not coincide with the centre of mass of negative charges is a polar molecule.
- They have permanent dipole moment.
- They act as tiny electric dipoles.
- They have symmetrical shape.
Show Solution
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The Correct Option is D
Solution and Explanation
Step 1: Understanding the Concept
A polar molecule has a permanent separation between its positive and negative charge centres. This gives it a permanent dipole moment.
Step 2: Statement (A)
Positive and negative charge centres not coinciding is the definition of a polar molecule. True.
Step 3: Statement (B)
Because of this separation, it has a permanent dipole moment. True.
Step 4: Statement (C)
Each polar molecule behaves like a tiny electric dipole. True.
Step 5: Statement (D)
Symmetrical shape is a feature of non-polar molecules, whose charge centres coincide, as in \(\text{CO}_2\) or \(\text{CH}_4\). Polar molecules like \(\text{H}_2\text{O}\) are bent and unsymmetrical. So (D) is the wrong statement.
Final Answer:
Polar molecules have an unsymmetrical charge arrangement, so the symmetrical-shape statement is wrong, option (D). \[ \boxed{\text{(D)}} \]
A polar molecule has a permanent separation between its positive and negative charge centres. This gives it a permanent dipole moment.
Step 2: Statement (A)
Positive and negative charge centres not coinciding is the definition of a polar molecule. True.
Step 3: Statement (B)
Because of this separation, it has a permanent dipole moment. True.
Step 4: Statement (C)
Each polar molecule behaves like a tiny electric dipole. True.
Step 5: Statement (D)
Symmetrical shape is a feature of non-polar molecules, whose charge centres coincide, as in \(\text{CO}_2\) or \(\text{CH}_4\). Polar molecules like \(\text{H}_2\text{O}\) are bent and unsymmetrical. So (D) is the wrong statement.
Final Answer:
Polar molecules have an unsymmetrical charge arrangement, so the symmetrical-shape statement is wrong, option (D). \[ \boxed{\text{(D)}} \]
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