Write the steps (reactions) for the Born-Haber cycle for MgCl2(s). Use the Born-Haber cycle to calculate the lattice energy of MgCl2(s). Some useful data to work with: For Mg: ΔΔHsub = 147 kJ/mol, IE1 and IE2 are 738 kJ/mol and 1450 kJ/mol, respectively. For chlorine: Bond energy = 243 kJ/mol, EA1 = -349 kJ/mol, respectively.

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): BaO, NaF, MgO, CsBr Least exothermic ◆ ◆ 4 ◆ Most exothermic

please explain each

based on the following information calculate the approximate lattice energy of XCl2.X is 3x larger than Na+. The lattice energy for NaCl is 787kj/mole

Determine the crystal lattice energy for MgCl2, given the following information: Cl2(g) → Mgčl2(s)AH°f = -642 kJ/mol 2+ (Mg - AHvaporization = 147.7 kJ/mol, Mg- Ejionization = 2188.4 kl/mol, Cl2 - EBond = 248 kJ/mol, Cl" - Ejonization = -349 kJ/mol)

Consider hypothetical element X and Y.  Suppose the enthalpy of formation of the compound XY is -336 kJ/mol, the bond enthalpy for X2 is 414 kJ/mol, and the bond enthalpy of Y2 is 159 kJ/mol.  Estimate the XY bond enthalpy in units of KJ/mol.

Calculate the lattice energy for the formation of Mg+2(g)   +   S -2 (g) → MgS (s)   ΔH= ?

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.

Question 5

V, PIER the compound with the bigger lattice energy. Note: lattice energy is always greater than zero. Which compound has the bigger lattice energy? MgBr2 SrBr2 Cs,0 CsF KF KI