Which of the following molecular geometries is most likely to result in a polar molecule, assuming the central atom is bonded to atoms of different electronegativities?

• A. Bent
• B. Tetrahedral
• C. Linear
• D. Trigonal planar

Answer: (A)

Verified step by step guidance

1. Understand that molecular polarity depends on both the polarity of individual bonds and the overall molecular geometry, which affects how bond dipoles combine.
2. Recall that a molecule is polar if it has a net dipole moment, meaning the bond dipoles do not cancel out due to symmetry.
3. Analyze each geometry: Linear and trigonal planar geometries are generally symmetrical, so if bonded atoms have different electronegativities, the dipoles may cancel out, resulting in a nonpolar molecule.
4. Consider the tetrahedral geometry, which can be symmetrical if all bonded atoms are the same, but if bonded atoms differ, the dipoles may or may not cancel depending on their arrangement.
5. Recognize that the bent geometry is inherently asymmetrical, causing bond dipoles to not cancel out, making it the most likely geometry to result in a polar molecule when bonded to atoms of different electronegativities.