Confused about energy change diagrams I have been reading about endothermic and exothermic reactions, as well as change in enthalpy.

From what I have read, an exothermic reaction is where more energy is given out as bonds are made when products form than energy taken in as the bonds of reactants are broken. 

Wouldn't this mean that the products have more enthalpy? However, a diagram online shows this (https://www.bbc.com/bitesize/guides/zg84y4j/revision/2):



Why does this diagram show that more energy is taken in as the bonds of reactants are broken? Isn't it incorrect?

I am only just getting started with this topic so I'm just learning concepts. I am not yet familiar with the formulas.
Wouldn't this mean that the products have more enthalpy?


The products have less enthalpy, maybe the following diagram remediates misconception :


$ΔH=Σproducts-Σreactants = {-965.5 -(-74.87)}=-890.63$