It may seem counter-intuitive but breaking bonds absorb energy. In simplicity, the reason is energy is required to overcome the electrostatic attractions between bonded atoms. Bonded atoms are attracted to each other by interactions between the electron cloud of one atom and the positive (proton filled) nucleus of the other atom.
Yes.
That's rather less informative than it might be had the question been worded a bit more exclusively.
The formation of bonds is exergonic, while the breaking of bonds is endergonic.
Breaking bonds requires energy.
Heat is the most common one
The enthalpy change associated with a reaction = sum of (energies of bonds broken) - sum of (energies of bonds formed). Thus, if this value is net negative, the reaction is exothermic; the products are also more stable than the reactants (lower-energy bonds). A positive enthalpy indicates an endothermic reaction.
Breaking bonds uses energy, making bonds releases energy.
Bond forming releases energy. Atoms will begin with a high potential energy, and will bond with other atoms to form compounds which have a lower potential energy, and are therefore more stable. Bond breaking takes in energy i.e. energy is required to break bonds.
energy is release by the breaking of bonds
Breaking bonds requires energy.
The process of breaking down food so we can absorb it is called digestion. Releasing the energy by breaking it down further in our cells is respiration.
Yes, a stronger bond requires more energy to break, and also releases more energy when it is made. In a chemical reaction, if you are breaking strong bonds, and only making weak ones, the reaction will require a lot of energy (endothermic). If instead you are breaking weak bonds and making very strong ones in the products, the reaction will release energy (exothermic).
Heat is the most common one
The enthalpy change associated with a reaction = sum of (energies of bonds broken) - sum of (energies of bonds formed). Thus, if this value is net negative, the reaction is exothermic; the products are also more stable than the reactants (lower-energy bonds). A positive enthalpy indicates an endothermic reaction.
breaking the bonds in a disaccharide/ polysaccharide
Bond Dissociation Enthalpy is the energy required for breaking the bonds. This energy is supplied mostly by giving thermal energy (Heat).
Gasoline is an example of energy being released by and exothermic reaction. Which is caused by the breaking of bonds and the creation of new bonds which use a lesser energy to form than the energy release by the previous bonds.
The formation of chemical bonds releases energy. It is an exothermic process. The breaking of chemical bonds takes energy. It is an endothermic process.
Breaking bonds uses energy, making bonds releases energy.
This is it