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Chapter 7: Q116E (page 406)

Use the Molecule Shape simulator (http://openstaxcollege.org/l/16MolecShape) to explore real molecules. On the Real Molecules tab, select 鈥渕odel鈥� mode and S2O. What is the model bond angle? Explain whether the 鈥渞eal鈥� bond angle should be larger or smaller than the ideal model angle.

Short Answer

Expert verified

The model angle is\({120^\circ }\), as expected for a trigonal planar electron-group shape.

Step by step solution

01

Definition of molecules

The number of atomic nuclei making up a molecule is a determinate number.

A molecule is a particle made up of two or more atoms that are chemically bonded together.

02

Explanation

As expected for a trigonal planar electron-group shape, the model angle is \({120^\circ }\)

The true angle, on the other hand, should be smaller, owing to the fact that the lone pair takes up more space and compresses the bonds to\({119^\circ }\).

Therefore, for a trigonal planar electron-group shape, the model angle is\({120^\circ }\), as expected.

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Most popular questions from this chapter

Methanol,\({{\text{H}}_{\text{3}}}{\text{COH}}\), is used as the fuel in some race cars. Ethanol,\({{\text{C}}_{\text{2}}}{{\text{H}}_{\text{5}}}{\text{OH}}\), is used extensively as motor fuel in Brazil. Both methanol and ethanol produce\({\text{C}}{{\text{O}}_{\text{2}}}\)and\({{\text{H}}_{\text{2}}}{\text{O}}\)when they burn. Write the chemical equations for these combustion reactions using Lewis structures instead of chemical formulas.

Draw the Lewis electron dot structures for these molecules, including resonance structures where appropriate:

(a) \({\rm{CS}}_{\rm{3}}^{{\rm{2 - }}}\)

(b) \({\rm{C}}{{\rm{S}}_{\rm{2}}}\)

(c) \({\rm{CS}}\)

(d) predict the molecular shapes for \({\rm{C}}{{\rm{S}}_{\rm{3}}}^{{\rm{2 - }}}\) and \({\rm{C}}{{\rm{S}}_{\rm{2}}}\)and explain how you arrived at your predictions

Explain the difference between a nonpolar covalent bond, a polar covalent bond, and an ionic bond.

Question: Using the standard enthalpy of formation data in Appendix G, calculate the bond energy of the carbon-sulphur double bond in \({\rm{C}}{{\rm{S}}_{\rm{2}}}\).

Correct the following statement: 鈥淭he bonds in solid\({\text{PbC}}{{\text{I}}_{\text{2}}}\)are ionic; the bond in a\({\text{HCl}}\)molecule is covalent. Thus, all of the valence electrons in\({\text{PbC}}{{\text{I}}_{\text{2}}}\)are located on the\({\text{C}}{{\text{I}}^{\text{ - }}}\)ions, and all of the valence electrons in a\({\text{HCl}}\)molecule are shared between the\({\text{H}}\)and\({\text{CI}}\)atoms.鈥�
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