Enthalpy and Bond Energy Sign Convention

I read that a negative enthalpy of formation means an exothermic reaction. Does that mean this reaction is true? The enthalpy of formation for $\ce{H\_2O}$ is -285.8 kJ/mol.


$$\ce{2H2(g) + O2(g) -> 2H2O(l) + 285.8\*2 kJ}$$


What about the enthalpy of reaction though? Is it also negative for exothermic reactions, like the one above? I think it's calculated with: $\Delta H$(Rxn) = Sum of Heat of Formation of Products – Sum of Heat of Formation of Products.


What about bond enthalpy (bond energy)? I know the calculation is different:  

$\Delta H$(bond energy) = Sum of Bond Energy of **reactants** – Sum of Bond Energy of **products**, so are **positive** bond enthalpies exothermic (like in the example above)?


Finally, for Gibbs free energy, $\Delta G=\Delta H-T \Delta S$, is enthalpy in the equation for enthalpy of reaction since it's the change in enthalpy?


