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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

Define dipole moment. What are the units and symbol for dipole moment?

What is the hybridization of atomic orbitals? Why is it impossible for an isolated atom to exist in the hybridized state?

The ionic character of the bond in a diatomic molecule can be estimated by the formula $$ \frac{\mu}{e d} \times 100 \% $$ where \(\mu\) is the experimentally measured dipole moment (in \(\mathrm{C} \mathrm{m}\) ), \(e\) is the electronic charge \((1.6022 \times\) \(10^{-19} \mathrm{C}\) ), and \(d\) is the bond length in meters. (The quantity \(e d\) is the hypothetical dipole moment for the case in which the transfer of an electron from the less electronegative to the more electronegative atom is complete.) Given that the dipole moment and bond length of \(\mathrm{HF}\) are \(1.92 \mathrm{D}\) and \(91.7 \mathrm{pm},\) respectively, calculate the percent ionic character of the molecule.

What is the angle between these two hybrid orbitals on the same atom? (a) \(s p\) and \(s p\) hybrid orbitals, (b) \(s p^{2}\) and \(s p^{2}\) hybrid orbitals, (c) \(s p^{3}\) and \(s p^{3}\) hybrid orbitals.

List these molecules in order of increasing dipole moment: \(\mathrm{H}_{2} \mathrm{O}, \mathrm{CBr}_{4}, \mathrm{H}_{2} \mathrm{~S}, \mathrm{HF}, \mathrm{NH}_{3}, \mathrm{CO}_{2}\)
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