Use the Born-Haber cycle and given data AHF (CCI) 438.0 kJ/mol, ICs) 376 kJ/mol, sublimation energy A Hub (Cs) = 78.0 kJ/mol, the bond energy of Cl2 (g) is 243 kJ/mol EA(CI) -349 kJ/mol to calculate the lattice energy of CsCl

Which of the compounds below will have the GREATEST lattice energy? *Sizes are given in pm (picometers) Charge & Atomic size X +1 155pm G-1 225 pm Y +1 356 pm D-1 289 pm A +2 110 pm E -2 185 pm B +2 265 pm N -2 325 pm O XG O YD O AE BN

Use the Born Haber cycle (show relevant steps) to determine the lattice energy of CsCl (s) from the following data: ΔHf°[CsCl(s)] = -442.8 kJ/mol; enthalpy of sublimation of Cesium is 78.2 kJ/mol; enthalpy of dissociation of Cl2 (g) = 243 kJ/mol Cl2 ; IE1 for Cs(g) = 375.7 kJ/mol; electron affinityenthalpy-EA1 for Cl(g) = -349kJ/mol.

use bond energies to estimate the H for the following reaction. State wethere the reaction is endothemic or exothemic, and the state whether tthe reactant or product bond are stronger( on average). Frist draw the lewis structure of each molecules. nh2-nh2(L) + 2F2(g) --> N2(g) + 4HF(g)

The following compounds all display the NaCl structure. For each pair, indicate which would have the lattice energy of lesser magnitude. A)  CaO CaSe B)  NaClNaF C) MgOCaO D) MgSMgSe E) SrO NaI

The standard heat of formation of BaBr2BaBr2 is −−764 kJ/molkJ/mol. The first ionization energy of BaBa is 503 kJ/molkJ/mol and its second ionization energy is 965 kJ/molkJ/mol. The heat of sublimation of Ba[Ba(s)→Ba(g)]Ba[Ba(s)→Ba(g)] is 175 kJ/molkJ/mol. The bond energy of Br2Br2 is 193 kJ/molkJ/mol, the heat of vaporization of Br2(l)Br2(l) is 31 kJ/molkJ/mol, and the electron affinity of BrBr is −−325 kJ/molkJ/mol.   Calculate the lattice energy of BaBr2BaBr2.

The magnitude of the lattice energy (energy required to separate the ions) for the compounds K2O and CaO are shown below with respect to Coulombic attraction, which is the best explanation for the difference in lattice energy?

Given the quantities below, what is the lattice energy of AgCl? Select the correct answer below: -680 kJ/mol -917 kJ/mol -895 kJ/mol O-1742 kJ/mol Ionization energy of Ag = 734 kJ/mol Sublimation energy of Ag = 287 kJ/mol Dissociation energy of Cl₂ = 242 kJ/mol Enthalpy of formation of AgCl = -127 kJ/mol Electron affinity of Cl = -352 kJ/mol

-U * USing average bond enthalpies (linked above), Estimate the enthalpy change for the following reaction: 2 HCI (g) + Brz (g) → 2 HBr (g) + C/₂ (g) KJ

we would predict that the imaginary ionic compound XF would have a (higher /lower) lattice energy than YyF2 because