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Chemistry: The Molecular Science

Chemistry: The Molecular Science

5th Edition

ISBN:9781285199047

Author:John W. Moore, Conrad L. Stanitski

Publisher:John W. Moore, Conrad L. Stanitski

Chapter7: Molecular Structures

Section: Chapter Questions

Problem 20QRT

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What are the angles a and b in the actual molecule of which this is a Lewis structure?
:0:
H
44.
H
Note for advanced students: give the ideal angles, and don't worry about small differences from the ideal that might be caused by the fact that different electron
groups may have slightly different sizes.
a = 0 °
b=0°

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It is possible to write a simple Lewis structure for the SO42- ion, involving only single bonds, which follows the octet rule. However, Linus Pauling and others have suggested an alternative structure, involving double bonds, in which the sulfur atom is surrounded by six electron pairs. (a) Draw the two Lewis structures. (b) What geometries are predicted for the two structures? (c) What is the hybridization of sulfur in each case? (d) What are the formal charges of the atoms in the two structures?
a Carbonyl fluoride, COF2, is an extremely poisonous gas used in organofluorine synthesis. Give the valence bond description of the carbonyl fluoride molecule. (Both fluorine atoms are attached to the carbon atom.) b Nitrogen, N2, makes up about 80% of the earths atmosphere. Give the valence bond description of this molecule.
Consider the following molecules: SiH4, PH3, H2S. In each case, a central atom is surrounded by four electron pairs. In which of these molecules would you expect the bond angle to be less than 109.5? Explain your reasoning.
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The formula for nitryl chloride is ClNO2 (in which N is the central atom). (a) Draw the Lewis structure for the molecule, including all resonance structures. (b) What is the NO bond order? (c) Describe the electron-pair and molecular geometries, and give values for all bond angles. (d) What is the most polar bond in the molecule? Is the molecule polar? (e) The computer program used to calculate electrostatic potential surfaces gave the following charges on atoms in the molecule: A = 0.03, B = 0.26, and C = +0.56. Identify the atoms A, B, and C. Are these calculated charges in accord with your predictions?
For each of the following molecules, state the bond angle (or bond angles, as appropriate) that you would expect to see on the central atom based on the simple VSEPR model. Would you expect the actual bond angles to be greater or less than this? a CCl4 b SCl2 c COCl2 d AsH3
Consider the following compounds: CO2, SO2, KrF2, SO3, NF3, IF3, CF4, SF4, XeF4, PF5, TF5, and SCl6. These 12 compounds are all examples of different molecular structures. Draw the Lewis structures for each and predict the molecular structures. Predict the bond angles and the polarity of each. (A polar molecule has a net dipole moment, while a nonpolar molecule does not.) See Exercises 25 and 26 for the molecular structures based on the trigonal bipyramid and the octahedral geometries.
Which of these molecules have an odd number of valence electrons: NO2, SCl2, NH3, NO3?
Consider the following compounds: CO2, SO2, KrF2, SO3, NF3, IF3, CF4, SF4, XeF4, PF5, IF5, and SCl6. These 12 compounds arc all examples of different molecular structures. Draw the Lewis structures for each and predict the molecular structure. Predict the bond angles and the polarity of each. (A polar molecule has a net dipole moment, while a nonpolar molecule docs not.) See Exercises 115 and 116 for the molecular structures based on the trigonal bipyramid and the octahedral geometries.
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Which of the molecules in Exercise 121 have net dipole moments (are polar)?

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