In general, the higher the charge on the ions in an ionic compound, the more favorable is the lattice energy. Why do some stable ionic compounds have 11 charged ions even though 14, 15, and 16 charged ions would have a more favorable lattice energy?
Answer to relevant QuestionsConsider the following energy changes: a. Magnesium oxide exists as Mg2+O2-, not as Mg+O-. Explain. b. What experiment could be done to confirm that magnesium oxide does not exist as Mg+O-? Compare your answers from parts a and b of Exercise 43 with ΔH values calculated for each reaction using standard enthalpies of formation in Appendix 4. Do enthalpy changes calculated from bond energies give a reasonable ...Acetic acid is responsible for the sour taste of vinegar. It can be manufactured using the following reaction: Use tabulated values of bond energies (Table 13.6) to estimate DH for this reaction. Compare this result to the ...Peroxyacetyl nitrate, or PAN, is present in photochemical smog. Draw Lewis structures (including resonance forms) for PAN. The skeletal arrangement is The most common type of exception to the octet rule are compounds or ions with central atoms having more than eight electrons around them. PF5, SF4, ClF3, and Br3- are examples of this type of exception. Draw the Lewis ...
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