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The formation of a typical covalent bond can be visualised as follows. If two atoms approach one another sufficiently closely for a bond to form, their outermost – most electrons are attracted towards both nuclei with comparable force. These electrons are known as the valence electrons and they are responsible for bonding. By providing energy, such as heat or light, valence electron can become excited and jump into next orbital. Therefore, the distance between nuclei and valence electron increases resulting in a weaker bond. In this excited state, the molecule stores more internal kinetic energy, have a greater vibration but the bond is weaker because there is a greater distance between atoms and between valence electrons and nuclei. The molecule is unstable, and less energy is required to break the bond. Therefore, the energy diagram in the exothermic reactions shows higher potential energy for reactants than for products and less activation energy is needed to initiate the reaction. During exothermic reaction, the potential energy is transformed into kinetic energy and released into surroundings. The products store less internal kinetic energy, and form stronger and more stable bonds, hence they have a lower potential energy.