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Chapter 10: Problem 70
Which of these molecules are linear? \(\mathrm{ICl}_{2}^{-}, \mathrm{IF}_{2}^{+}, \mathrm{OF}_{2}\), \(\mathrm{SnI}_{2}, \mathrm{CdBr}_{2}\).
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Sketch the bond moments and resultant dipole moments for these molecules: \(\mathrm{H}_{2} \mathrm{O}, \mathrm{PCl}_{3}, \mathrm{XeF}_{4}, \mathrm{PCl}_{5}\) \(\mathrm{SF}_{6}\)
The bonds in beryllium hydride \(\left(\mathrm{BeH}_{2}\right)\) molecules are polar, and yet the dipole moment of the molecule is zero. Explain.
The formation of \(\mathrm{H}^{+}\) from two \(\mathrm{H}\) atoms is an energetically favorable process. Yet statistically there is less than a 100 percent chance that any two \(\mathrm{H}\) atoms will undergo the reaction. Apart from energy considerations, how would you account for this observation based on the electron spins in the two \(\mathrm{H}\) atoms?
Sketch the shape of a linear triatomic molecule, a trigonal planar molecule containing four atoms, a tetrahedral molecule, a trigonal bipyramidal molecule, and an octahedral molecule. Give the bond angles in each case.
The geometry of \(\mathrm{CH}_{4}\) could be square planar, with the four \(\mathrm{H}\) atoms at the corners of a square and the \(\mathrm{C}\) atom at the center of the square. Sketch this geometry and compare its stability with that of a tetrahedral \(\mathrm{CH}_{4}\) molecule.
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