Which one of the following trends appears when considering lattice energies?AnionA) The higher the charge on the ions, thehigher the lattice energy.Cation F-CI-Br-|-O2-B) The more ions present in an ioniccompound, the smaller the lattice energy.Lit1036 853807757 2925Na+923787747704 2695C) The larger the distance between ions in theionic compound, the higher the lattice energy.K+8217156826492360Mg2+ 2957 2524 2440 2327 3791D) In general, alkali metals have larger latticeenergies than alkaline earth metals with thesame anions.Ca2+ 2630 2258 2176 2074 3401Al3+5215 5492 5361 5217 15,916

Lattice energy is the energy required by one mole of ionic compound in order to get separated to its…

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. Br I- 02- 807 757 2925 B) The more ions present in an ionic compound, the smaller the lattice energy. 747 704 2695 C) The larger the distance between ions in the ionic compound, the higher the lattice energy. 682 649 2360 42440 2327 3791 D) In general, alkali metals have larger lattice energies than alkaline earth metals with the same anions. 8 2176 2074 3401 2 5361 5217 15,916

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. Br I- 02- 807 757 2925 B) The more ions present in an ionic compound, the smaller the lattice energy. 747 704 2695 C) The larger the distance between ions in the ionic compound, the higher the lattice energy. 682 649 2360 42440 2327 3791 D) In general, alkali metals have larger lattice energies than alkaline earth metals with the same anions. 8 2176 2074 3401 2 5361 5217 15,916

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

Chapter8: Bonding: General Concepts

Section: Chapter Questions

Problem 26Q: In general the higher the charge on the ions in an ionic compound, the more favorable the lattice...

See similar textbooks

Similar questions

In general the higher the charge on the ions in an ionic compound, the more favorable the lattice energy. Why do some stable ionic compounds have +1 charged ions even though +4, + 5, and +6 charged ions would have a more favorable lattice energy?
The 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.
Think of forming an ionic compound as three steps (this is a simplification, as with all models): (I) removing an electron from the metal; (2) adding an electron to the nonmetal; and (3) allowing the metal cation and nonmetal anion to come together. a. What is the sign of the energy change for each of these three processes? b. In general, what is the sign of the sum of the first two processes? Use examples to support your answer. c. What must be the sign of the sum of the three process d. Given your answer to part c, why do ionic bonds occur? e. Given your above explanations, why is NaCl stable but not Na2Cl? NaCl2? What about MgO compared to MgO2? Mg2O?
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.
What main factors control the magnitude of lattice energies? Give a specific example of a compound that should have a high lattice energy, and explain why its lattice energy is high.
Calculate the enthalpy of reaction for HCN(g)H(g)+C(g)+N(g) from enthalpies of formation (see Appendix C). Given that the CH bond enthalpy is 411 kJ/mol, obtain a value for the CN bond enthalpy. Compare your result with the value given in Table 9.5.
When a reaction is exothermic, is the sum of bond energies of products or of reactants greater?
hat is the enthalpy change for a process? Is enthalpy a state function? In what experimental apparatus are enthalpy changes measured?
Using the bond energies in Table 7.2, determine the approximate enthalpy change for each of the following reactions: (a) Cl2(g)+3F2(g)2ClF3(g) (b) H2C=CH2(g)+H2(g)H3CCH3(g) (c) 2C2H6(g)+7O2(g)4CO2(g)+6H2O(g) .
The lattice energy of LiF is 1023 kJ/mol, and the Li—F distance is 200.8 pm. NaF crystallizes in the same structure as LiF but with a Na—F distance of 231 pm. Which of the following values most closely approximates the lattice energy of NaF: 510, 890, 1023, 1175, or 4090 kJ/mol? Explain your choice.
Enthalpy changes for the following reactions can be determined experimentally: N2(g) + 3 H2(g) 2 NH3(g) rH = 91.8 kJ/mol-rxn 4 NH3(g) + 5 O2(g) 4 NO(g) + 6 H2O(g) rH = 906.2 kJ/mol-rxn H2(g) + O2(g) H2O(g) rH = 241.8 kl/mol-rxn Use these values to determine the enthalpy change for the formation of NO(g) from the elements (an enthalpy change that cannot be measured directly because the reaction is reactant-favored). N2(g) + O2(g) NO(g) rH = ?
Draw a curve that describes the energy of a system with H and Cl atoms at varying distances. Then, find the minimum energy of this curve two ways. (a) Use the bond energy found in Table 8.1 to calculate the energy for one single HCl bond (Hint: How many bonds are in a mole?) (b) Use the enthalpy of reaction and the bond energies for H2 and Cl2 to solve for the energy of one mole of HCl bonds. H2(g)+Cl2(g)2HCl(g)Hrxn=184.7kJ/mol