Look at example 1.2 in the link above.
Use the equation and Lewis structures from 0:40 of Professor Dave's video and the bond energies from Table 1 in the link above to determine the change in enthalpy (H) of the reaction.
Did you use Dave's suggestion (H = products - reactants) and get a positive number? A positive H indicates an endothermic reaction, which absorbs heat from the surroundings. However, we know that combustion reactions give off heat and are therefore exothermic. What's wrong with Dave's explanation?
Dave has made the common mistake of interpreting the bond energies as energy stored within the bonds. In fact, the bond energies represent the energy required to break a bond (when it is a reactant) and the energy released by the formation of that bond (when it is a product).
Energy required to break bonds is an endothermic process (+H). Energy released to break bonds is an exothermic process (-H).
So the correct formula for determining enthalpy of a reaction is:
H = reactants - products
Develop a storyboard that shows how the combustion of methane absorbs and releases energy. Use bond energies to explain how the reaction is exothermic so that we can help Professor Dave understand his mistake.