91Ó°ÊÓ

Sketch a choralkali cell. Show the half-cell reactions and indicate the direction of diffusion of the ions. Give the chemical equation for the unwanted reaction that would occur if \(\mathrm{OH}^{-}\)migrated through the membrane and into the anode compartment.

Nitrogen trifluoride, \(\mathrm{NF}_{3}\), boils at \(-129^{\circ} \mathrm{C}\) and is a very weak Lewis base. By contrast, the lower molar mass compound \(\mathrm{NH}_{3}\) boils at \(-33^{\circ} \mathrm{C}\) and is well known as a Lewis base. (a) Describe the origins of this very large difference in volatility. (b) Describe the probable origins of the difference in basicity.

Given that \(1.84 \mathrm{~g}\) of \(\mathrm{IF}_{3}\) reacts with \(0.93 \mathrm{~g}\) of \(\left[\left(\mathrm{CH}_{3}\right)_{4} \mathrm{~N}\right] \mathrm{F}\) to form a product \(\mathrm{X},(\mathrm{a})\) identify \(\mathrm{X},(\mathrm{b})\) use the VSEPR model to predict the shapes of \(\mathrm{IF}_{3}\) and the cation and anion in \(\mathrm{X}\), and (c) predict how, many \({ }^{19} \mathrm{~F}\)-NMR signals would be observed in \(\mathrm{IF}_{3}\) and \(\mathrm{X}\).

Use the VSEPR model to predict the shapes of \(\mathrm{SbCl}_{5}, \mathrm{FClO}_{3}\), and \(\left[\mathrm{ClF}_{6}\right]^{+}\)

]Indicate the product of the reaction between \(\mathrm{CIF}_{5}\) and \(\mathrm{SbF}_{5}\). Predict the shapes of the reactants and products.

Sketch all the isomers of the complexes \(\mathrm{MCl}_{4} \mathrm{~F}_{2}\) and \(\mathrm{MCl}_{3} \mathrm{~F}_{3}\). Indicate how many fluorine environments would be indicated in the \({ }^{19} \mathrm{~F}\)-NMR spectrum of each isomer.

(a) Use the VSEPR model to predict the probable shapes of \(\left[\mathrm{IF}_{6}\right]^{+}\)and \(\mathrm{IF}_{7}\). (b) Give a plausible chemical equation for the preparation of \(\left[\mathrm{IF}_{6}\right]\left[\mathrm{SbF}_{6}\right] .\)

Predict the shape of the doubly chlorine-bridged \(\mathrm{I}_{2} \mathrm{Cl}_{6}\) molecule by using the VSEPR model, and assign the point group.

Predict the structure and identify the point group of \(\mathrm{ClO}_{2} \mathrm{~F}\).

Predict whether each of the following solutes is likely to make liquid \(\mathrm{BrF}_{3}\) act as a Lewis acid or a Lewis base: (a) \(\mathrm{SbF}_{5}\), (b) \(\mathrm{SF}_{6}\), (c) CsF.