Arrange the following ionic compounds in order of decreasing lattice energy: RbI, NaCl, KBr, LiF, MgS, BeO, BN. Arrange the following anions in order of increasing ionic radii: F-, O2-, N3-, P3-, As3-, Ge4- Arrange the following cations in order of increasing ionic radii: Fr+, Cs+, Rb+, B3+, Al3+, Ga3+

Arrange the following ionic compounds in order of decreasing lattice energy: RbI, NaCl, KBr, LiF, MgS, BeO, BN. Arrange the following anions in order of increasing ionic radii: F-, O2-, N3-, P3-, As3-, Ge4- Arrange the following cations in order of increasing ionic radii: Fr+, Cs+, Rb+, B3+, Al3+, Ga3+

Chemistry: Principles and Practice

3rd Edition

ISBN:9780534420123

Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Publisher:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Chapter9: Chemical Bonds

Section: Chapter Questions

Problem 9.31QE: Arrange the following series of compounds in order of increasing lattice energies. (a) NaBr, NaCl,...

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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, Na2S
Arrange the following series of compounds in order of increasing lattice energies. (a) NaBr, NaCl, KBr (b) MgO, CaO, CaCl2 (c) LiF, BeF2, BeO
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The standard enthalpies of formation for S(g), F(g), SF4(g), and SF6(g) are + 278.8, + 79.0, 775, and 1209 kJ/mol, respectively. a. Use these data to estimate the energy of an SF bond. b. Compare your calculated value to the value given in Table 8.5. What conclusions can you draw? c. Why are the Ht0 values for S(g) and F(g) not equal to zero, since sulfur and fluorine are elements?
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Rank the following ionic compounds in order of lattice energy, from least exothermic to most exothermic: KCl, SrO, RbBr, CaO
Suppose 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.
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