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Born-4-Iaber cycles, such as those shown in Figures 6.7 and 6.8,are called cycles because they form dosed loops. If any five of the six energy changes ¡n the cycle are known, the value of the sixth can be calculated. Use the following five values to calculate the lattice energy in kilojoules per mole for sodium hydride, NaH(s):
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- Which compound in each of the following pairs of ionic substances has the most negative lattice energy? Justify your answers. a. LiF, CsF b. NaBr, NaI c. BaCl2, BaO d. Na2SO4, CaSO4 e. KF, K2O f. Li2O, Na2Sarrow_forwardSuppose a chemist discovers a new metallic element and names it "Xtrinsium" (Xt). Xt exhibits chemical behaviour similar to an alkaline earth. Xt(s) + F2(g) → XtF2(s) Lattice energy for XtF2 -2360. kJ/mol First Ionization energy of Xt 520. kJ/mol Second Ionization energy of Xt 936 kJ/mol Electron affinity of F -327.8 kJ/mol Bond energy of F2 154 kJ/mol Enthalpy of sublimation (atomization) of Xt 180. kJ/mol Use the above data to calculate ΔH°f for Xtrinsium fluoride.arrow_forwardSuppose a chemist discovers a new metallic element and names it "Xhaustium" (Xh).Xh exhibits chemical behaviour similar to an alkaline earth. Xh(s) + F2(g) → XhF2(s) Lattice energy for XhF2 -2140. kJ/mol First Ionization energy of Xh 310. kJ/mol Second Ionization energy of Xh 589 kJ/mol Electron affinity of F -327.8 kJ/mol Bond energy of F2 154 kJ/mol Enthalpy of sublimation (atomization) of Xh 150. kJ/mol Use the above data to calculate ΔH°f for Xhaustium fluoride. Your answer must be accurate and precise to the nearest 1 kJ/mol, as are the given parameters.arrow_forward
- The ionic substances KF, CaO and ScN are isoelectronic . Examine the 8.2 table lattice energies and account for any trends you observe.arrow_forwardThe substances NaF and CaO are isoelectronic (have thesame number of valence electrons). (a) What are the chargeson each of the cations in each compound? (b) What are thecharges of each of the anions in each compound? (c) Withoutlooking up lattice energies, which compound is predicted tohave the larger lattice energy? (d) Using the lattice energiesin Table 8.1, predict the lattice energy of ScN.arrow_forwardWhich ionic compounds would have the greatestlattice energy: NaCl, KCl, or MgC l 2 ? Explain youranswer.arrow_forward
- Use the Born Haber cycle (show relevant steps) to determine the lattice energy of CsCl (s) from the following data:Hf 0 [CsCl(s)] = -442.8 kJ/mol; enthalpy of sublimation of Cesium is 78.2 kJ/mol; enthalpy of dissociation of Cl2 (g) = 243 kJ/mol Cl2 ; IE1 for Cs(g) = 375.7 kJ/mol; electron affinity enthalpy-EA1 for Cl(g) = -349kJ/molarrow_forwardwhich of the following elements Na, Li, N , As, Ge is the most electronegative A) Ge B) N C) Na D) As E) Liarrow_forwardThe ionic radii of element E and a different metallic element, M, are shown in the following table: Both elements form oxides, E2O and MO. If lattice energy is defined as the energy required to separate an ionic solid into individual separate gaseous ions, would the lattice energy of MO be less than, equal to, or greater than the lattice energy of the oxide E2O? Justify your answer in terms of Coulomb's lawarrow_forward
- The electron affinity of oxygen is -141kj/mol, corresponding to the reaction O(g)+e-—>O-(g) The lattice energy of K2O(s) is 2238kj/mol.Use these data along with data in Appendix C and figure 7.10 to calculate the “second electron affinity” of oxygen, corresponding to the reaction O-(g)+e-—>O2-(g)arrow_forwardWhich of the following elements is the most electronegative? N, Na,As, or P?arrow_forwardImagine a metallic element had been discovered and was named "Gondolium" (Gn).Gn was found to exhibit chemistry like that of an alkaline earth. Gn(s) + F2(g) → GnF2(s) Lattice energy for GnF2 -1950. kJ/mol First Ionization energy of Gn 450. kJ/mol Second Ionization energy of Gn 855 kJ/mol Electron affinity of F -327.8 kJ/mol Bond energy of F2 154 kJ/mol Enthalpy of sublimation (atomization) of Gn 195 kJ/mol Use the above data to calculate ΔH°f for gondolium fluoride.arrow_forward
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