Question

Choose the polar molecule from the following:

• A. \(CH_2=CH_2\)
• B. \(CHCl_3\)
• C. \(CCl_4\)
• D. \(CO_2\)

Answer 1

The Correct Option is B

To identify the polar molecule, we will analyze the molecular geometry and the distribution of electronegative atoms for each provided compound:

1. \(CH_2=CH_2\): Ethylene is a symmetrical molecule. The carbon atoms share electrons equally, resulting in no net dipole moment. Therefore, ethylene is nonpolar.
2. \(CHCl_3\): Chloroform possesses a tetrahedral geometry. The three chlorine atoms are more electronegative than hydrogen, inducing a net dipole moment. The asymmetrical placement of these electronegative atoms renders the molecule polar.
3. \(CCl_4\): Carbon tetrachloride, despite having polar C-Cl bonds, exhibits a symmetrical tetrahedral structure. This symmetry causes the individual bond dipoles to cancel out, rendering the molecule nonpolar.
4. \(CO_2\): Carbon dioxide is linear. The dipole moments of the two C=O bonds are equal and opposite, resulting in their cancellation and making the molecule nonpolar.

Consequently, \(CHCl_3\) is the sole polar molecule among the options, making it the correct answer.