Student Solutions Manual For Chemistry: Atoms First
3rd Edition
ISBN: 9781259923098
Author: Julia Burdge, Jason Overby Professor
Publisher: McGraw-Hill Education
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Chapter 10.8, Problem 10.8.1SR
Interpretation Introduction
Interpretation:
The correct statement has to be identified.
Concept Introduction:
Lattice energy:
The amount of energy that is necessary for the conversion of one mole of ionic solid to its constituent ions in gaseous phase is called Lattice energy.
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(a) Based on the lattice energies of MgCl2 and SrCl2 given inTable 8.1, what is the range of values that you would expectfor the lattice energy of CaCl2? (b) Using data from AppendixC, Figure 7.11, Figure 7.13, and the value of the secondionization energy for Ca, 1145 kJ>mol, calculate the latticeenergy of CaCl2.
MA, MD, ME, and MG are ionic compounds in which M is a metal. A, D, E, and G are monovalent non-metals of the same Group in the Periodic Table. The order of atomic numbers for these elements is E > D > G > A. With which one of the following, the metal has the most exothermic value of lattice energy?
☐A
☐D
☐E
☐G
☐The value is the same for all.
The lattice energy of LiF is 1023 kJ/mol, and the Li–F distance is 201 pm. MgO crystallizes in the same structure as LiF but with a Mg–O distance of 205 pm. Which of the following values most closely approximates the lattice energy of MgO: 256 kJ/mol, 512 kJ/mol, 1023 kJ/mol, 2046 kJ/mol, or 4008 kJ/mol? Explain your choice.
Chapter 10 Solutions
Student Solutions Manual For Chemistry: Atoms First
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- The lattice energy of LiF is 1023 kJ/mol, and the LiF distance is 201 pm. MgO crystallizes in the same structure as LiF but with a Mg—O distance of 205 pm. Which of the following values most closely approximates the lattice energy of MgO: 256 kJ/mol, 512 kJ/mol, 1023 kJ/mol, 2046 kJ/mol, or 4008 kJ/mol? Explain your choice.arrow_forwardThe lattice energy of KF is 794 kJ/mol, and the interionic distance is 269 pm. The Na—F distance in NaF, which has the same structure as KF, is 231 pm. Which of the following values is the closest approximation of the lattice energy of NaF: 682 kJ/mol, 794 kJ/mol, 924 kJ/mol, 1588 kJ/mol, or 3175 kJ/mol? Explain your answer.arrow_forwardDetermine the lattice energy of NaCl(s), using the data provided.arrow_forward
- Estimate the ionic radius of Cs+. The lattice energy of CsCl is 633 kJ/mol. For CsCl the Madelungconstant, M, is 1.763, and the Born exponent, n, is 10.7. The ionic radius of Cl– is known to be 1.81 Åarrow_forwardKBr has a lattice energy -671 kJ/mol . Consider a hypothetical salt XY. X2+ has the same radius of K+ and Y2− has the same radius as Br−. Estimate the lattice energy of XY.arrow_forwardLattice energy of which compound will be maximum: a NaCl b KClarrow_forward
- Using the following data, calculate the lattice energy of calcium chloride: Ca2+(g) + 2Cl– (g) → CaCl2(s) ΔHlattice = ? Sublimation enthalpy of calcium ΔH = 177.8 kJ/mol First ionization energy of calcium ΔH = 590.2 kJ/mol Second ionization energy of calcium ΔH = 1144.2 kJ/mol First electron affinity of chlorine ΔH = –349 kJ/mol Heat of formation of CaCl2(s) ΔH = –795.4 kJ/mol Bond energy of Cl2 (see Table 2) Use Hess’s law to calculate the lattice energy of calcium chloride. set-up must show all the chemical equations and you must show how their H values add up to give your answer.arrow_forwardthe lattice energy of CaC2(s) is -2911 kJ/mol. calculate a value for the thermochemical radius of the carbide ion, C2^2-.arrow_forwardThis thermodynamic cycle describes the formation of an ionic compound MX2 from a metal element M and nonmetal element X in their standard states. Based of the table (picture): A. What is the lattice enthalpy of MX2 ? (in kJ/mol) B. What is the enthalpy of formation of MX2 ? (in kJ/mol) C. Suppose both the electron affinity of X and the heat of sublimation of M were smaller. Would MX2 be more or less stable?arrow_forward
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