A Group 1 metal, M, formed an ionic compound with chlorine.
The enthalpy of lattice dissociation for this compound is +773 kJ mol-1 and the hydration enthalpy of a chloride ion is -363 kJ mol-1.
The enthalpy of solution of the Group 1 chloride is +4 kJ mol-1.
Using the information in Table 4.1, identify the Group 1 ion, M+. Show your working.
Group 1 ion |
Enthalpy of hydration (kJ mol-1) |
Li+ |
-519 |
Na+ |
-406 |
K+ |
-321 |
Rb+ |
-296 |
Identity of M+ = ...........................
The same Group 1 metal from part (a) forms an ionic lattice with another halide ion. This new ionic compound has an enthalpy of lattice formation of -705 kJ mol-1.
Using M to represent the Group 1 metal, suggest a formula for the new ionic lattice and explain your answer.
The enthalpy of hydration becomes less exothermic as you go down Group 1. Using the values in part (a):
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