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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

Compare the relative stability of these species and indicate their magnetic properties (that is, diamagnetic or paramagnetic): \(\mathrm{O}_{2}, \mathrm{O}_{2}^{+}, \mathrm{O}_{2}^{-}\) (superoxide ion), \(\mathrm{O}_{2}^{2-}\) (peroxide ion).

What are the hybrid orbitals of the carbon atoms in these molecules? (a) \(\mathrm{H}_{3} \mathrm{C}-\mathrm{CH}_{3}\) (b) \(\mathrm{H}_{3} \mathrm{C}-\mathrm{CH}=\mathrm{CH}_{2}\) (c) \(\mathrm{CH}_{3}-\mathrm{C} \equiv \mathrm{C}-\mathrm{CH}_{2} \mathrm{OH}\) (d) \(\mathrm{CH}_{3} \mathrm{CH}=\mathrm{O}\) (e) \(\mathrm{CH}_{3} \mathrm{COOH}\).

Predict the bond angles for these molecules: (a) \(\mathrm{BeCl}_{2},\) (b) \(\mathrm{BCl}_{3},\) (c) \(\mathrm{CCl}_{4},\) (d) \(\mathrm{CH}_{3} \mathrm{Cl}\) (e) \(\mathrm{Hg}_{2} \mathrm{Cl}_{2}\) (arrangement of atoms: \(\mathrm{ClHgHgCl}\) ), (f) \(\mathrm{SnCl}_{2}\) (g) \(\mathrm{H}_{2} \mathrm{O}_{2},\) (h) \(\mathrm{SnH}_{4}\).

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

The compound 1,2 -dichloroethane \(\left(\mathrm{C}_{2} \mathrm{H}_{4} \mathrm{Cl}_{2}\right)\) is nonpolar, while cis-dichloroethylene \(\left(\mathrm{C}_{2} \mathrm{H}_{2} \mathrm{Cl}_{2}\right)\) has a dipole moment: The reason for the difference is that groups connected by a single bond can rotate with respect to each other, but no rotation occurs when a double bond connects the groups. On the basis of bonding considerations, explain why rotation occurs in \(1,2-\) dichloroethane but not in \(c i s\) -dichloroethylene.
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