Do high-energy chemical bonds indicate strong chemical bonds?
There are two factors here to consider.
First, the energy released by a given reaction is (partly) due to the difference between the bond strength in the product vs reactant, not the absolute bond strength, unless the reaction involves just breaking a bond and not forming a new one.
Second, even if your reaction is just a bond breaking, there are multiple ways to break a bond. Reported bond enthalpies are usually defined in terms of the energy required for homolytic bond breaking, ie one electron stays on each component. For example,
$$\ce{HCl -&gt; H. + Cl.}$$
By that measure, the H-Cl bond is quite strong, but we know that in a polar solvent that mitigates the negative effect of charge separation, the H-Cl will readily undergo heterolytic bond cleavage, where both electrons stay on one atom:
$$\ce{HCl -&gt; H+ + Cl-}$$
In that context, we might consider the H-Cl bond to be very weak. (Note, though, that I'm also overlooking the amount of &quot;bonding&quot; between solvent and ions in this case, which means that it's not an example of a pure bond breaking reaction.)
All of which is to say that before you can make a statement about bond energy and bond &quot;strength&quot; you need to define both terms more specifically.