Why is energy released when bonds are formed?

PLEASE HELP! Which of the following statements regarding energy changes during a reaction are true?

• Chemical reactions occur when molecules or atoms collide, the bonds between atoms are broken, and new bonds are formed. Breaking the bonds of the reactants requires energy; bond formation releases energy. Which of the following statements regarding energy changes during a reaction are true? 1) Decreasing the temperature decreases the kinetic energy of the reactants, and the reaction goes more slowly. 2) Two or more atoms must collide, with proper orientation, with energy greater than or equal to the activation energy for a reaction to occur. 3) The activation energy (Ea) of the forward reaction is the difference between the energy of the products and the energy of the transition state. 4) If the heat of reaction, ΔH, is positive, the energy of the products is lower than the energy of the reactants, and the reaction is endothermic. 5) When the activation energy is high, the reaction rate is fast. 6) Increasing the concentration of reactants increases the number of collisions, and the reaction goes faster. 7) The energy of a collision between atoms or molecules must be greater than the activation energy (Ea) for bonds to be broken.

• Answer:

  1) True 2) True 3) No, It's the difference between the energy of the REACTANTS and the energy of the transition state. 4) It's all true except the bit that says 'the energy of the products is lower'.... it's actually higher. 5) No, the activation energy doesn't effect reaction rate, its just the energy needed to get the reaction started. 6)True 7) False, it can also be equal to the activation energy, but maybe I'm just being picky.