H2S has a net dipole moment while BeF2 has zero dipole moment, because of:
Correct answer: B. H2S molecule is angular, while BeF2 molecule is linear.
- A. H2S molecule is linear, while BeF2 is angular.
- B. H2S molecule is angular, while BeF2 molecule is linear.
- C. Fluorine has more electronegativity.
- D. Be is more electronegative than S.
Explanation
The molecular geometry determines the net dipole moment of a molecule. H2S has a bent shape due to the presence of lone pairs on the sulfur atom, leading to a net dipole moment. On the other hand, BeF2 is linear and symmetrical, which causes the individual bond dipoles to cancel out, resulting in a net dipole moment of zero. Options A, C, and D are incorrect because they either describe the wrong molecular shapes or focus on electronegativity differences, which are not the primary reason for the observed dipole moments.
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Chemical bonding explains molecular shape through VSEPR theory and distinguishes sigma bonds from pi bonds. Questions involve hybridization, bond angles, dipole moment and bond energy, including how electron-pair repulsion determines geometry and how bond polarity differs from the overall polarity of a molecule.
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