(1.) What are the two types of layer arrangement in metals? Which has the closer packing?
(2.) What properties of a compound would lead you to expect that it contains ionic bonds?
(3.) Which one of each of the following pairs will be smaller? Explain your reasoning in each case.
(a.) K or K+
(b.) K+ or Ca2+
(c.) Br- or S2-
(4.) Which one NaCl or NaI, would be expected to have the higher melting point? Explain your reasoning.
(5.) Explain the difference between the 227 degrees C melting point of tin(II) chloride, SnCl2, and the -33 degrees C melting point of tin(IV) chloride, SnCl4.
(6.) Would you expect sodium chloride to dissolve in carbon tetrachloride, CCl4? Explain your reasoning.
(7.) Which of sodium chloride and magnesium chloride is more likely to be hydrated in the solid phase? Explain your reasoning.
(8.) Of lithium nitrate and sodium nitrate, which is more likely to exist as a hydrate in the solid phase? Explain your reasoning.
(9.) Explain the factor affecting the ion coordination number in an ionic compound.
(10.) Which would be more polarizable, the fluoride ion or the iodide ion. Give your reason.
This solution is provided in an attached .doc file. It discusses close packing, ionic bonds in reference to the periodic table, melting point, cations and anions in order to answer each question.