Interpretation:
The second
Concept introduction:
Lattice energy is the amount of energy needed for the conversion of one mole of an ionic solid to its constituent ions in the gaseous form.
The higher the value of lattice energy for a compound, the higher is its stability.
Born–Haber cycle is the method of calculating the lattice energy of a compound using different values of its constituent elements.
The steps to calculate lattice energy using Born–Haber cycle are given below:
The enthalpies of the formation of the metal as well as the non-metal are to be added.
The ionization energy of the metal is added, and electron affinity is subtracted from the calculated value.
The mode of the enthalpy of formation of the required compound is added to the above value.
Want to see the full answer?
Check out a sample textbook solutionChapter 8 Solutions
CHEMISTRY MCC CUSTOM W/CONNECT >CI<
- Some plant fertilizer compounds are HNO3, H2SO4, H3PO4, NH4NO3, and K2CO3. Which of these compounds contain both ionic and covalent bonds? (Select all that apply.)arrow_forwardQuestion 1 Draw the Bond-Haber cycle for the formation of one mole of calcium sulphide (CaS). The relevant data from which the cycle is constructed are: Standard Enthalpy of formation of CaS =-482KJ/mol Sublimation energy of Calcium = +176 KJ/mol Sum of first two ionization energy for calcium = +1690 KJ/mol Enthalpy of formation of gaseous sulphur atoms = +240 KJ/mol Electron affinity for sulphur for two electrons = +449KJ/mol Calculate the lattice energy for CaS What is lattice energy Why is the total electron affinity for sulphur positive? Cucl2 is a stable compound, whereas neither CaCl nor CaC3 are known as unstable compounds. Account for this observation.arrow_forwardUse ionic properties to choose the hypothetical compound with larger lattice energy: AG or ED. Elements A and E are in group 1A of the periodic table and A is below C. Elements G and D are in group 7A of the periodic table and G is below D. Good hand written explanation Asaparrow_forward
- Question A 1.(a) 6C(g) + 14H(g) CH14(g) H= -7510KJ/mol 7C(g) + 16H(g) C7H16(g) H= -7510KJ/mol Use the information given above to determine the average (C-C)and (C-H) bond energies Use the value obtained in (i) to calculate H for the following changes. 3C(g) + 8H(g) C3H8(g) (b) You are given the following data of enthalpy of atomization of AI (KJ/mol). Enthalpy of atomization of AI = +324 1st I.E of AI = +580 2nd I.E of AI = +1800 3rd I.E of AI = +2700 Enthalpy of atomization of Cl = +121 Electron affinity of Chlorine = -364 Estimated L.E of AlCl2 = -2602 L.E of AlCl3 = -5380 (i) Draw an energy level diagram for the following reaction Al(s) + 3/2Cl(g) AlCl3(s) (ii) Calculate the standard enthalpy of formation (Hf) of AlCl3 (iii) Why is AlCl3 formed in the reaction in (i) rather than AlCl2(s)?arrow_forwardThe 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.arrow_forward(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.arrow_forward
- Consider the ionic compounds KF, NaCl, NaBr, and LiCl.(a) Use ionic radii (Figure 7.8) to estimate the cation–aniondistance for each compound. (b) Based on your answer topart (a), arrange these four compounds in order of decreasinglattice energy. (c) Check your predictions in part (b) with theexperimental values of lattice energy from Table 8.1. Are thepredictions from ionic radii correct?arrow_forwardQUESTION 2 Use the table below to determine ΔH for the following reaction H 2C=CH 2(g) + F 2(g) ↔ CH 2FCH 2F(g) Bond Energies, kJ/mol Single Bonds H C N O S F Cl Br I H 432 C 411 346 N 386 305 167 O 459 358 201 142 S 363 272 --- --- 286 F 565 485 283 190 284 155 Cl 428 327 313 218 255 249 240 Br 362 285 243 201 217 249 216 190 I 295 213 --- 201 --- 278 208 175 149 Multiple Bonds C=C 602 C=N 615 C=O 799 C≡C 835 C≡N 887 C≡O 1072 N=N 418 N=O 607 S=O (in SO2) 532 N≡N 942 O2 494 S=O (in SO3) 469 Key Concept: ΔH° rxn = ∑ΔH ° bonds broken - ∑ΔH ° bonds formedarrow_forwardANSWER PLS. THANK YOU! How important is the rule of eight? What do you call the molecule that is formed from non-metal atoms? How do non-metals combine?arrow_forward
- Calculate H for the following process: K(g)+Br(g)KBr(s) The lattice energy of KBr is 689 kJ/mol, and the ionization energy of K is 419 kJ/mol. The electron affinity of Br is given in Table 8.4. See Problem 8.119.arrow_forwardThe 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_forwardQuestion 1: CuCl2 is a stable compound, whereas neither CaCl nor CaCL3 are known as unstable compounds. Account for this observation. a)i) Distinguish between the expression (bond energy term and Bond dissociation ) Under what circumstances would these necessarily have the same value?arrow_forward
- General Chemistry - Standalone book (MindTap Cour...ChemistryISBN:9781305580343Author:Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; DarrellPublisher:Cengage LearningChemistry by OpenStax (2015-05-04)ChemistryISBN:9781938168390Author:Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark BlaserPublisher:OpenStaxChemistryChemistryISBN:9781305957404Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCostePublisher:Cengage Learning
- Chemistry In FocusChemistryISBN:9781305084476Author:Tro, Nivaldo J., Neu, Don.Publisher:Cengage Learning