Exercises Molecular Geometry

Which of the following diatomic molecules has the shortest bond length  

Which of the following diatomic elements contains only 1 sigma (a) and 1 pi (ir) bond  

In a molecule in which the central atom exhibits sp3d hybrid orbitals, the electron pair arrangements form the shape of a(n) 

The electron-dot structure (Lewis structure) for which of the following molecules would have one unshared pairs of electrons on the central atom  

Which of the following molecules has a trigonal pyramidal shape  

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The quality of the available data are generally of a reliable standard, particularly the more recent X-ray diffraction studies. Caution, however, must be exercised when evaluating much of the earlier gas phase work, in view of limitations in both contemporary instrumentation and experimental methods which usually require implicit assumptions about molecular geometry. Such data are generally best assessed in groups, and reliance given to systematic trends rather than absolute values. 

EXERCISE 9.2 Molecular Geometries of Molecules with Expanded Valence Shells... 

EXERCISE 10,2 According to the VSEPR model, what molecular geometry would you predict for iodine trichloride, ICI3 ... 

Predicting Molecular Geometries UsingVSEPRTheory and the Effects of Lone Pairs (10.4) Examples 10.2-10.3 For Practice 10.2-10.3 Exercises 35-36... 

Exercises 1. First,valence-bond theory clearly distinguishes between sigma and pi bonds. In valence-bond theory, it is clear that a sigma bond must be stronger than a pi bond, for the orbitals overlap more effectively in a sigma bond (end-to-end) than they do in a pi bond (side-to-side). Second, molecular geometries are more directly obtained in valence-bond theory than in Lewis theory. Third, Lewis theory does not explain hindered rotation about double bonds. 3a. Lewis theory does not describe the shape of the water molecule. 

Exercise 3.6. A cluster is found to have the molecular formula [Os+CO ]2-. Generate a set of likely cluster geometries. 

Exercise 7.6. The solid-state compound Mg2CoH5 has been prepared and exhibits the same metal lattice as MgFeH6. Using the Zintl-Klemm approach and your knowledge of molecular coordination chemistry, suggest a logical geometry for the H atoms around the Co center. 

Consider the following compounds CO2, SO2, KrF2, SO3, NF3, IF3, CF4, SF4, XeF4, PF5, IF5, and SCIe. These 12 compounds are all examples of different molecular structures. Draw the Eewis 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 does not.) See Exercises 105 and 106 for the molecular structures based on the trigonal bipyramid and the octahedral geometries. 

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