8.83 Construct a Born-Haber cycle for the formation of the hy- pothetical compound NaCl2, where the sodium ion has a 2+ charge (the second ionization energy for sodium is given in Table 7.2). (a) How large would the lattice energy need to be for the formation of NaCl2 to be exothermic? (b) If we were to estimate the lattice energy of NaCl2 to be roughly equal to that of MgCl2 (2326 kJ/mol from Table 8.1), what value would you obtain for the standard enthalpy of formation, AH, of NaCl2? ing together of Na (g) and Cl (AH=-788 kJ/mol). Notice Table 8.1 lists the lattice energies for a number of ionic compounds. The large itive values indicate that the ions are strongly attracted to one another in ionic solid Pos TABLE 8.1 Lattice Energies for Some Ionic Compounds Lattice Energy (kJ/mol) Lattice Energy (kJ/mo Compound 2526 Compound MgCl2 1030 2127 LiF SrCl2 834 LiCl 730 Lil 3795 MgO 910 NaF 3414 CaO 788 NaCl 3217 SrO 732 NaBr 682 Nal ScN 7547 KF 808 КС. 701 KBr 671 CsCl 657 CsI 600

8.83 Construct a Born-Haber cycle for the formation of the hy- pothetical compound NaCl2, where the sodium ion has a 2+ charge (the second ionization energy for sodium is given in Table 7.2). (a) How large would the lattice energy need to be for the formation of NaCl2 to be exothermic? (b) If we were to estimate the lattice energy of NaCl2 to be roughly equal to that of MgCl2 (2326 kJ/mol from Table 8.1), what value would you obtain for the standard enthalpy of formation, AH, of NaCl2? ing together of Na (g) and Cl (AH=-788 kJ/mol). Notice Table 8.1 lists the lattice energies for a number of ionic compounds. The large itive values indicate that the ions are strongly attracted to one another in ionic solid Pos TABLE 8.1 Lattice Energies for Some Ionic Compounds Lattice Energy (kJ/mol) Lattice Energy (kJ/mo Compound 2526 Compound MgCl2 1030 2127 LiF SrCl2 834 LiCl 730 Lil 3795 MgO 910 NaF 3414 CaO 788 NaCl 3217 SrO 732 NaBr 682 Nal ScN 7547 KF 808 КС. 701 KBr 671 CsCl 657 CsI 600

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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The lattice energy of NaCl is 769 kJ/mole. Which of the following is a correct statement about NaCl? When one mole each of gaseous Nat and CI- ions form solid NaCl, 769 kJ of heat is consumed. It requires 769 kJ to separate one mole of solid NaCl into one mole of each gaseous Na* and CI- ions. It requires 769 kJ to separate one mole of solid NaCl into gaseous one mole of Na* and two moles of CI- ions.
2. Use the data provided below to calculate the lattice energy of calcium chloride. Electron affinity of Cl = -348.7 kJ/mol 1st ionization energy of Ca = 590.0 kJ/mol 2nd ionization energy of Ca = 1145.0 kJ/mol Bond energy of Cl2 = 242.6 kJ/mol Sublimation energy of Ca = 178.0 kJ/mol AH¡ [CaCl. (s)] =-795.0 kJ/mol
Consider the reaction below. Mg2+ (g) + 2 Br (g) →→ MgBr₂ (s) - When this type of reaction occurs, energy is emitted The energy involved in producing MgBr₂ (s) in this way is known as the lattice energy of MgBr₂.
Estimate the lattice energy, AU, for NaCl if the ionic radii for Na* and Cl" are 102.0 pm and 181.0 pm, respectively. AU kJ/mo + TOOLS x10
KBr has a lattice energy -671 kJ/mol. Consider a hypothetical salt XY. X3+ has the same radius of K+ and Y3− has the same radius as Br−. Estimate the lattice energy of XYXY.
The charges and sizes of the ions in an ionic compound affect the strength of the electrostatic interaction between the ions and thus the strength of the lattice energy of the ionic compound. Arrange the compounds according to the magnitudes of their lattice energies based on the relative ion charges and sizes. Highest lattice energy Lowest lattice energy Answer Bank KCI MgO NaF MgF₂
Which one of the following trends appears when considering lattice energies? Anion A) The higher the charge on the ions, the higher the lattice energy. Cation F- CI- Br- |- O2- B) The more ions present in an ionic compound, the smaller the lattice energy. Lit 1036 853 807 757 2925 Na+ 923 787 747 704 2695 C) The larger the distance between ions in the ionic compound, the higher the lattice energy. K+ 821 715 682 649 2360 Mg2+ 2957 2524 2440 2327 3791 D) In general, alkali metals have larger lattice energies than alkaline earth metals with the same anions. Ca2+ 2630 2258 2176 2074 3401 Al3+ 5215 5492 5361 5217 15,916
The charges and sizes of the ions in an ionic compound affect the strength of the electrostatic interaction between the ions and thus the strength of the lattice energy of the ionic compound. Arrange the compounds according to the magnitudes of their lattice energies based on the relative ion charges and sizes. (highest to lowest) Mgo,NaF,MgF2, and KCI
Which one of the following ions has the greatest lattice energy? A. KCI = KF = KBr = KI B. KCI C. KI D. KBr E. KF
The lattice energy of NaF is 904 kJ/mol, and the Na–F distance is 190 pm. An unknown metal oxide crystallizes in the same structure as NaF but with distance of 207 pm. The metal oxide has the formula MO, where M is the unknown metal. Which of the following values most closely approximates the lattice energy of the metal oxide? Question 6 options: a) 256 kJ/mol b) 512 kJ/mol c) 904 kJ/mol d) 1046 kJ/mol e) 4090 kJ/mol
Calculate the lattice energy of RbH (s) using the following thermodynamic data (all data is in kJ/mol). Note that the data given has been perturbed, so looking up the answer is probably not a good idea. AHsublimation 61 kJ/mol Ionization energy = 383 kJ/mol Rb (s) Rb (g) H - H (g) Bond energy = 416 kJ/mol H (g) Electron affinity = -93 kJ/mol RbH (s) AHOf = -72 kJ/mol kJ/mol
16) ( , Using the thermochemical data below calculate the lattice energy for the formation of Na₂O. Na(s) → Na(g) 107.3 kJ/mol Na(g) → Na*(g) + 1 e 495.9 kJ/mol 2 Na(s) + O₂(g) → Na₂O(s) -418 kJ/mol 1/2 O₂(g) → O(g) 249.1 kJ/mol O(g) + 1 e→O(g) -141 kJ/mol -1484.5 kJ/mol O(g) + 1 e0²(g) s) If 115 or pressu