The estimated lattice energy for
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- Compare the electron affinity of fluorine to the ionization energy of sodium. Does the process of an electron being pulled from the sodium atom to the fluorine atom have a negative or a positive E? Why is NaF a stable compound? Does the overall formation of NaF have a negative or a positive E? How can this be?arrow_forwardConsider the reactions of silver metal, Ag(s), with each of the halogens: fluorine, F2(g), chlorine, Cl2(g), and bromine, Br2(l). What chapter data could you use to decide which reaction is most exothermic? Which reaction is that?arrow_forwardThe lattice energy of an ionic solid such as NaCl is the enthalpy change H for the process in which the solid changes to ions. For example, NaCl(s)Na+(g)+Cl(g)H=786kJ/mol Assume that the ionization energy and electron a affinity are H values for the processes defined by those terms. The ionization energy of Na is 496 kJ/mol. Use this, the electron affinity from Table 8.4, and the lattice energy of NaCl to calculate H for the following process: Na(g)+Cl(g)NaCl(s)arrow_forward
- Calculate the lattice energy of potassium fluoride, KF, using the BornHaber cycle. Use thermodynamic data from Appendix C to obtain the enthalpy changes for each step. (Note: You will obtain a slightly different answer if you use values given in Chapter 8 for the ionization energy and electron affinity, which are energy values at 0 K rather than the enthalpy changes at 298 K.)arrow_forwardSolid phosphorus pentabromide, PBr5, has been shown to have the ionic structure [PBr4] [Br]. Write the electron-dot formula of the PBr4+ cation.arrow_forwardThe 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?arrow_forward
- Given the following data calculate H for the reaction On the basis of the enthalpy change, is this a useful reaction for the synthesis of ammonia?arrow_forward6.941 mol atomic mass electronegativity 0.98 kJ 59.6 mol electron affinity kJ 520.2 mol ionization energy kJ 3.0 mol heat of fusion Does the following reaction absorb or release energy? O release O absorb (1) Li (g) + e Li(g) O Car be decided with the data given. Is it possible to calculate the amount of energy absorbed or released by reaction (1) using only the data above? O yes O no If you answered yes to the previous question, enter the amount of energy absorbed or released by reaction (1): O k/mol Does the following reaction absorb or release energy? O release O absorb (2) Li(g) → Li (g) + e O Can't be decided with the data given. Is it possible to calculate the amount of energy absorbed or released by reaction (2) using only the data above? O yes O no If you answered yes to the previous question, enter the amount of energy absorbed or released by reaction (2): I kJ/molarrow_forwardGiven the following information, construct a Born-Haber cycle to calculate the lattice energy of CrCl₂I(s): Net energy change for the formation of CrCl₂I(s) = -420 kJ/mol Bond dissociation energy for I2(g) = +243 kJ/mol Bond dissociation energy for Cl2(g) for Cl2(g) for 12(g) = +151 kJ/mol Heat of sublimation for I2(s) = +62 kJ/mol Heat of sublimation for Cr(s) = +397 kJ/mol = E₁₁ for Cr(g) = 652 kJ/mol E₁₂ for Cr(g) == 1588 kJ/mol E₁3 for Cr(g) = 2882 kJ/mol Eea for Cl(g)=-349 kJ/mol === Eea for I(g) = -295 kJ/molarrow_forward
- Consider an ionic compound, MX3, composed of generic metal M and generic gaseous halogen X. The enthalpy of formation of MX3 is Δ?∘f=−925 kJ/mol. The enthalpy of sublimation of M is Δ?sub=175 kJ/mol. The first, second, and third ionization energies of M are IE1=579 kJ/mol, IE2=1677 kJ/mol, and IE3=2479 kJ/mol. The electron affinity of X is Δ?EA=−369 kJ/mol. (Refer to the hint). The bond energy of X2 is BE=179 kJ/mol. Determine the lattice energy of MX3.arrow_forwardThe lattice energy of cesium iodide is the energy required for the following reaction. CsI(s) → Cs+(g) + I−(g) ΔHrxn = ΔHlattice Use the Born-Haber cycle to calculate ΔHlatticefor CsI(s) from the information given below. Equation 1: 2 Cs(s) + I2(g) → 2 CsI(s) ΔH1 = −692 kJ/mol Equation 2: Cs(s) → Cs(g) ΔH2 = 77 kJ/mol Equation 3: I2(g) → 2 I(g) ΔH3 = 214 kJ/mol Equation 4: Cs(g) → Cs+(g) + e− ΔH4 = 376 kJ/mol Equation 5: I(g) + e− → I−(g) ΔH5 = −294 kJ/molarrow_forwardg 44.956 mol atomic mass electronegativity 1.36 kJ 18.1 mol electron affinity kJ 633.1 mol ionization energy kJ 16. mol heat of fusion Does the following reaction absorb or release energy? O release O absorb (1) Sc(g) + e Sc (g) O Can't be decided with the data given. Is it possible to calculate the amount of energy absorbed or released by reaction (1) using only the data above? O yes O no If you answered yes to the previous question, enter the amount of energy absorbed or released by reaction (1): O kJ/mol Does the following reaction absorb or release energy? O release O absorb (2) Sc (g) - Sc (g) + e O Can't be decided with the data given. Is it possible to calculate the amount of energy absorbed or released by reaction (2) using only the data above? O yes O no If you answered yes to the previous question, enter the amount of energy absorbed or released by reaction (2): O kJ/molarrow_forward
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