Dismiss Notice
Join Physics Forums Today!
The friendliest, high quality science and math community on the planet! Everyone who loves science is here!

Why energy released when bonds formed

  1. Jul 27, 2011 #1
    In chemistry its often said that energy must be added to system to break atomic bonds and conversely when atoms bond energy is released. I can picture why it takes energy to break a bond, for instance to ionize a hydrogen atom you have to exert a force on the electron to overcome the electrostatic attraction of the electron for the proton. I don't however see how that electron bonding to the proton to form a netral hydrogen atom would release energy.
     
  2. jcsd
  3. Jul 27, 2011 #2
    Classical mechanics doesn't really work to describe how/why two species bond. For instance the positive charges of 2 Hydrogen nuclei should be repelled from each other and therefore you would think that Hydrogen gas should exist as Hydrogen atoms. However, Hydrogen gas exists as 2 Hydrogen atoms sharing a pair of electrons because the configuration of the electrons around the two protons is such that it is of lower energy when the electrons are "shared" then when they are not.

    In Chemistry we do not talk about electrons bonding with protons. In Chemistry, a bond is when an ion/atom/molecule "decides" to share electrons with another ion/atom/molecule. The two species will "decide" to bond if the energy of the overall system will decrease by them forming bonds.

    There are two main factors involved, entropy and enthalpy, commonly thought of as disorder and heat, respectively. The relation of these factors to energy is known as the Gibbs' Free Energy equation ΔG=ΔH-TΔS (H is enthalpy and S is entropy). In order for a process to proceed spontaneously, you need the ΔG to be negative (all systems tend to the lowest energy state possible).

    When two species become one, the entropy of the system (typically) is decreasing making the [-TΔS] term positive. In order to have that process be spontaneous, the ΔH term must be negative enough to overcome the positive TΔS term. Physically this is observed as heat or spark or an explosion or what have you. Now you have a system where covalent bonds were formed and the system is at its lowest energy state. In order to go the other way, you need to put energy back into the system to break those bonds.

    The funny thing is, that blanket statements like that tend to be a little misleading. Even if a process is spontaneous (overall negative ΔG), there is a certain amount of energy that you need to put into the system to "get things started." This is called the Activation Energy and is the reason why the wood that is around you right now is not bursting into flames as you read this message.
     
    Last edited: Jul 27, 2011
  4. Jul 28, 2011 #3
    Its pretty simple, you have explained it yourself already, Where does the energy used to knock off an electron from a Hydrogen atom go? into the electron, right? when another electron of similarly high energy is attracted by the proton, it must lose energy (in the form of heat, a photon etc) before it can be accepted by the 1s orbital. If you had an electron that was low in energy... You must ask... where exactly did this electron come from? because to have left an atom it must have had some energy supplied to it... right?

    Another way to think of it with classical mechanics is as a body being gravitationally attracted to the earth... Up high, it has a large amount of gravitational potential energy, but when it falls it loses this energy to air resistance etc.
     
Know someone interested in this topic? Share this thread via Reddit, Google+, Twitter, or Facebook