Lattice energies and electron affinities are very difficult to measure experimentally. Fairly reliable theoretical values for lattice energies can be calculated from simple models. The Born-Haber cycle can then be used to estimate electron affinities. Use the data below to calculate the electron affinity of iodine (in kJ mol1), where a negative EA value indicates a favourable anion formation. Name of enthalpy change Value in kJ/mol Formation enthalpy of Cal2(s) -533.46 Lattice energy of Cal2 -2074 Sublimation enthalpy of Ca 177.7 First ionization energy of Ca 589.8 Second ionization energy of Ca 1145.4 Sublimation enthalpy of I2 62.44 Bond energy of l2 151.1

Lattice energies and electron affinities are very difficult to measure experimentally. Fairly reliable theoretical values for lattice energies can be calculated from simple models. The Born-Haber cycle can then be used to estimate electron affinities. Use the data below to calculate the electron affinity of iodine (in kJ mol1), where a negative EA value indicates a favourable anion formation. Name of enthalpy change Value in kJ/mol Formation enthalpy of Cal2(s) -533.46 Lattice energy of Cal2 -2074 Sublimation enthalpy of Ca 177.7 First ionization energy of Ca 589.8 Second ionization energy of Ca 1145.4 Sublimation enthalpy of I2 62.44 Bond energy of l2 151.1

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...

See similar textbooks

Similar questions

Lattice energies and electron affinities are very difficult to measure experimentally. Fairly reliable theoretical values for lattice energies can be calculated from simple models. The Born-Haber cycle can then be used to estimate electron affinities. Use the data below to calculate the electron affinity of iodine (in kJ mol-1), where a negative EA value indicates a favourable anion formation. Name of enthalpy change Value in kJ/mol Formation enthalpy of Cal 2(s) -533.46 Lattice energy of Cal2 -2074 Sublimation enthalpy of Ca 177.7 First ionization energy of Ca 589.8 Second ionization energy of Ca 1145.4 Sublimation enthalpy of I2 62.44 Bond energy of 12 151.1 -293 +265 -599 -482
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.
Consider the following data for chlorine: atomic mass electronegativity electron affinity ionization energy heat of fusion 35.453 3.16 328. mol 1251.2 3.2 kJ mol kJ mol kJ mol You may find additional useful data in the ALEKS Data tab. Does the following reaction absorb or release energy? (1) C1 (₂) +- C (g) Is it possible to calculate the amount of energy absorbed or released by reaction (1) using only the data above? If you answered yes to the previous question, enter the amount of energy absorbed or released by reaction (1): Does the following reaction absorb or release. energy? (2) C1¹ () +- Cl (g) Is it possible to calculate the amount of energy absorbed or released by reaction (2) using only the data above? If you answered yes to the previous question, enter the amount of energy absorbed or released by reaction (2): O release absorb Can't be decided with the data given. O yes O no release O absorb Can't be decided with the data given. O yes O no mol S
Use the following data to calculate the enthalpy change for the following reaction: 2Na(s) + O2(g) -> Na2O(s) Quantity Magnitude (kJ/mol) Ionization energy of Na(g) 495 Electron affinity of O(g) for 2e 603 Vaporization energy of Na(s) 109 Bond energy of O2(g) 499 Lattice energy for Na2O(s) –2,477
The energy for the following reaction was measured to be -653.0 kJ/mol. K(g) + Cl(g) → KCl(s). Using this fact and data in the table below, calculate the enthalpy (in kJ/mol) required to separate the ions from the lattice for this reaction: KCl(s) → K⁺(g) + Cl⁻(g).
Use the data given below to construct a Born-Haber cycle to determine the lattice energy of CaO. A H°(kJ) Ca(s) → Ca(g) 193 Ca(g) → Cat (g) + e 590 Cat (g) → Ca2+(g) + e 1010 20(g) → O2(g) -498 O(g) + e O(g) -141 O(g) + e → O2(g) 878 Ca(s) + O2(g) → CaO(s) -> -635 O-2667 kJ O-3414 kJ O +1397 kJ +3028 kJ O-2144 kJ
Consider an ionic compound, MXMX, composed of generic metal MM and generic, gaseous halogen XX. The enthalpy of formation of MXMX is Δ?∘f=−411ΔHf∘=−411 kJ/mol. The enthalpy of sublimation of MM is Δ?sub=101ΔHsub=101 kJ/mol. The ionization energy of MM is IE=461IE=461 kJ/mol. The electron affinity of XX is Δ?EA=−325ΔHEA=−325 kJ/mol. (Refer to the hint). The bond energy of X2X2 is BE=189BE=189 kJ/mol. Determine the lattice energy of MXMX.
In each row, pick the compound with the bigger lattice energy. Note: lattice energy is always greater than zero. Which compound has the bigger lattice energy? BaF2 BaO K Br Na Br SrS Rb, S ?
KBr 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.
1a)Rank the following ionic compounds in order of lattice energy, from the least exothermic (least negative lattice enthalpy) to the most exothermic (most negative lattice enthalpy): KCI, SrO, RbBr, CaO 1b)Rank the following elements in order of decreasing metallic character (from most metallic to least metallic): S, CI, K, Cs, Se 1c) by using the table of bond enthalpies, predict ?rH of the following reaction in kJ/mol H2C=CH2 + Cl2 ---> Cl-CH2-CH2-Cl
1. Given the following information, calculate the lattice energy for LiI(s). Show all work and construct a diagram(cycle) that shows each step in the process of forming LiI(s) from gaseous ions.
Calculate the average A-B bond energy in AB3(g). AH for AB3(g)=-75.9 kJ/mol, AH, for A(g) = 288.9 kJ/mol, AH, for B(g) = 134.9 kJ/mol, AH for A2(g) = 0 kJ/mol, AH for B2(g)=0 kJ/mol. Enter a number in kJ/mol to 1 decimal place.