The overall energy involved in the formation of CsCl from Cs(s) and Cl2(g) is − 443 kJ mol−1 . Given the following information: heat of sublimation for Cs is 76 kJ mol−1 , bond dissociation energy for 12Cl2 is 121 kJ mol−1 , Ei1 for Cs is 376 kJ mol−1 , and Eea for Cl(g) is 349 kJ mol−1 . what is the magnitude of the lattice energy for CsCl ? Express your answer numerically in kJ mol−1 . View Available Hint(s)for Part B Hint 1for Part B. How to approach the problem The overall energy is the sum of the energies of five steps. The only unknown value is step 5 (ion condensation energy), which we can find by the following: step 1: 76 kJ mol−1 step 2: 121 kJ mol−1 step 3: 376 kJ mol−1 step 4: −349 kJ mol−1 step 5: ? ––––––––––––––––––––– overall: −443 kJ mol−1 Note that ion condensation (step 5) is equivalent to the magnitude of the lattice energy ( U ). Therefore, step 5 and U must have the same value. Activate to select the appropriates template from the following choices. Operate up and down arrow for selection and press enter to choose the input value typeActivate to select the appropriates symbol from the following choices. Operate up and down arrow for selection and press enter to choose the input value type magnitude of U = nothing kJ mol−1 Request Answer Part C Consider the lattice energy of any ionic compound. What combination of ions and charges will produce the largest (in magnitude) lattice energies? View Available Hint(s)for Part C small ions and small charges large ions and large charges small ions and large charges large ions and small charges Part D Complete previous part(s) Provide Feedback Correct. No additional followup.
