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Chapter 10: Problem 20

Does the molecule OCS have a higher or lower dipole moment than \(\mathrm{CS}_{2} ?\)

Short Answer

Expert verified
The OCS molecule has a higher dipole moment than CS2.

Step by step solution

01

Understand the structure of the molecules

Start by examining the structure of the two molecules, OCS and CS2. OCS is a linear molecule with sulfur atom bonded with an oxygen atom on one side and carbon atom on other side. CS2 is also a linear molecule, but both sides of the sulphur atom are bonded with carbon atoms.
02

Evaluate the electronegativity

The electronegativity of O (oxygen) is more than that of C (carbon) and S (sulphur). In OCS, the greater electronegativity of Oxygen creates a shift of electron density towards it, creating a resultant dipole moment. Whereas in CS2, both carbon atoms have the same electronegativity so no net dipole moment exists.
03

Compare the Dipole Moments

As the OCS molecule has a net dipole moment due to the presence of the highly electronegative oxygen atom, while the CS2 molecule does not have a net dipole moment, we can conclude that the OCS molecule has a higher dipole moment than CS2.

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Most popular questions from this chapter

Antimony pentafluoride, \(\mathrm{SbF}_{5}\), reacts with \(\mathrm{XeF}_{4}\) and \(\mathrm{XeF}_{6}\) to form ionic compounds, \(\mathrm{XeF}_{3}^{+} \mathrm{SbF}_{6}^{-}\) and \(\mathrm{XeF}_{5}^{+} \mathrm{SbF}_{6}^{-}\). Describe the geometries of the cations and anion in these two compounds.

Draw the Lewis structure of ketene \(\left(\mathrm{C}_{2} \mathrm{H}_{2} \mathrm{O}\right)\) and describe the hybridization states of the \(\mathrm{C}\) atoms. The molecule does not contain \(\mathrm{O}-\mathrm{H}\) bonds. On separate diagrams, sketch the formation of sigma and pi bonds.

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