To determine which of the given molecules is non-polar despite having polar bonds, we need to analyze each option regarding their molecular geometry and bond polarity.
1. Option A: [tex]\( BCl_3 \)[/tex] (Boron Trichloride)
- Bond Polarity: The bonds between Boron (B) and Chlorine (Cl) are polar due to the difference in electronegativity between B and Cl.
- Molecular Geometry: [tex]\( BCl_3 \)[/tex] has a trigonal planar shape. It is symmetrical, meaning that the polarities of the bonds cancel out each other.
- Result: Despite having polar bonds, the molecule is non-polar due to its symmetry.
2. Option B: [tex]\( CH_4 \)[/tex] (Methane)
- Bond Polarity: The bonds between Carbon (C) and Hydrogen (H) have very little difference in electronegativity, making them essentially non-polar.
- Molecular Geometry: [tex]\( CH_4 \)[/tex] has a tetrahedral shape, but since the bonds are non-polar, the molecule itself is non-polar.
- Result: This molecule has non-polar bonds and is non-polar overall.
3. Option C: [tex]\( H_2O \)[/tex] (Water)
- Bond Polarity: The bonds between Hydrogen (H) and Oxygen (O) are polar due to a significant difference in electronegativity.
- Molecular Geometry: [tex]\( H_2O \)[/tex] has a bent shape due to the lone pairs on the oxygen atom.
- Result: The asymmetrical shape and polar bonds make the water molecule polar.
4. Option D: [tex]\( CHCl_3 \)[/tex] (Chloroform)
- Bond Polarity: The bonds between Carbon (C) and Chlorine (Cl) are polar due to the difference in electronegativity.
- Molecular Geometry: [tex]\( CHCl_3 \)[/tex] has a tetrahedral shape, but it is asymmetrical due to the different types of atoms attached to the carbon.
- Result: The presence of asymmetrical polar bonds makes the chloroform molecule polar.
After analyzing all the options, the molecule that stands out as non-polar with polar bonds is:
Answer: A. [tex]\( BCl_3 \)[/tex]
