It's a semantic difference. The formation of the intermolecular attractions that are formed during solvation is exothermic, just as formation of covalent bonds is. Bond breaking is always exothermic. See:
http://www.chemguide.co.uk/physical/energetics/solution.html
The only case where bond breaking alone would be
exergonic would be where the increase in entropy is so great that it outweighs the always positive change in enthalpy. Can you provide any example of this sort of case? This would constitute a spontaneous decomposition of some molecule where there is no change in the intermolecular interactions with the surroundings or solvent between the reactant and products.
Edit: Actually I don't even think such a case is possible, because breaking any bond frees that electronic region of each of the atoms involved to engage in an additional intermolecular interaction. Basically I just don't see any evidence to back up what you're saying. Every spontaneous reaction I've ever seen involves an enthalpy change that is the sum of both bond breakage and formation, be it from hydrolysis, solvation, or whatever.