The real amount of energy in $rm HBr$ greater than the real energy stored in $rm HCl$

Our teacher told when a system contains more energy its unstable.
Bond dissociation enthalpy of $rm HCl$ is around 430kJ/mol and $rm HBr$ is around 360kJ/mol.
The bond length between $rm HCl$ is smaller than that of $rm HBr$ and so HCl have more strength because of that breaking the bond of HCl will absorb more energy than HBr.

Below is just my thoughts I don’t know whether it’s correct.
HCl is made by hydrogens orbit and 3p orbital of HCl overlap, and HBr bond is made by hydrogens orbit overlap and 4p of Br overlap. 4p contains more energy than 3p. So the energy stored inside HBr is higher than HCl and when energy is high the stability will low so HBr bonds strength is lower than HCl.
In ionization if we want to remove Na last electron a few amount of energy supply is sufficient but for a noble gas we have to supply a lot of ENERGY. Just like this to break hbr bond we have to supply a little amount of energy compared to hcl.
Is this correct or someone please explain me