The dipole moment of an ozone molecule, O₃, is 0.53 D. The molecule has a symmetrical bent structure so that, if the molecule is assumed to lie in the yz plane, the terminal atoms have coordinates ($\pm$0.678 Å,0,-0.362 Å) and the central atom has coordinates (0,0,0.724 Å). The terminal atoms have a net negative partial charge and the central atom has a net positive partial charge. Determine the magnitude of the partial charges on each of the oxygen atoms.

Question

Quizplus · Accepted Answer

The dipole moment ($\mu$) of a molecule can be calculated using the formula $\mu = q \times d$, where $q$ is the magnitude of the charge and $d$ is the distance between the charges. Given that the dipole moment of ozone is 0.53 D and the structure is symmetrical, we can deduce that the charges on the terminal atoms are equal in magnitude but opposite in sign to the charge on the central atom. The distance between the charges can be calculated based on the given coordinates, which leads to the conclusion that the charges must balance out to give the correct dipole moment. Option A provides a set of charges that, when multiplied by the appropriate distances, would result in the given dipole moment, considering the symmetry and geometry of the molecule.

The Dipole Moment of an Ozone Molecule, O3, Is 0 ±\pm±

The Dipole Moment of an Ozone Molecule, O₃, Is 0 $\pm$