2. Compare the charge density values of the three silver ions: Ag+, Ag2+, and Ag3+ (see Appendix 2). Which is most likely to form compounds exhibiting ionic bonding?
3. Using data tables, find the melting points of uranium(III) fluoride, uranium(IV) fluoride, uranium(V) fluoride, and uranium(VI) fluoride. At what point does the bonding type appear to change?
4. Would you expect sodium chloride to dissolve in carbon tetrachloride, CCl4? Explain your reasoning.
5. Which member of the following pairs has the higher melting point? Give your reasoning in each case. (a) copper(I) chloride, CuCl, or copper(II) chloride, CuCl2; (b) lead(II) chloride, PbCl2, or lead(IV) chloride, PbCl4.
6. Rubidium chloride adopts the sodium chloride structure. Calculate the radius of a rubidium ion if the density of rubidium chloride is 2.76 g?cm23 and it is assumed that the ions touch along the edges of the unit cell.
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