{"id":991,"date":"2019-10-22T12:47:13","date_gmt":"2019-10-22T12:47:13","guid":{"rendered":"http:\/\/chemdictionary.org\/?p=991"},"modified":"2019-10-22T12:47:21","modified_gmt":"2019-10-22T12:47:21","slug":"bond-energy","status":"publish","type":"post","link":"https:\/\/chemdictionary.org\/bond-energy\/","title":{"rendered":"Bond Energy"},"content":{"rendered":"\n

Definition <\/strong><\/h2>\n\n\n\n

\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0 When a bond is formed between two atoms, energy is released. The same amount of energy is absorbed when the bond is broken to form neutral atoms. So, \u2018\u2019the bond energy is the average amount of energy required to break all bonds of a particular type in one mole of the substance\u2019\u2019. <\/p>\n\n\n\n

Explanation <\/strong><\/h2>\n\n\n\n

It is determined experimentally, by measuring the heat involved in a chemical reaction. It is also called bond enthalpy as it is a measure of enthalpy change at 298 K. <\/p>\n\n\n\n

The\nenthalpy change in splitting a molecule into its component atoms is called\nenthalpy of atomization.<\/p>\n\n\n\n

IUPAC defines the average value of bond disassociation energies in the gas phase for all same chemical species of the same type of bond. For example carbon-hydrogen bond energy in methane H(C-H), their enthalpy change involved with breaking up the molecule of methane into carbon atom and four hydrogen radicals divided by 4 [1]. <\/p>\n\n\n\n

The bond energy is given in kJ\/mol which is the energy required to break an Avogadro\u2019s number (6.02 x 1022<\/sup>) of bonds. It is also released when an Avogadro\u2019s number of the bonds are formed. It may be noted that energies of multiple bonds are greater than those of single bonds. But a double bond is not twice as strong as a single bond or a triple bond is not as strong as a single bond.it means that \u03c3- bond is stronger than a \u03c0- bond. Similarly a polar covalent bond stronger than a non- polar covalent bond.<\/p>\n\n\n\n

Factors Affecting Bond Energy<\/strong><\/p>\n\n\n\n

Bond energy is the measure of the strength of a bond. The strength of the bond depends upon the following factors [2].<\/p>\n\n\n\n

  1. Electronegativity\ndifference of bonded atom<\/li>
  2. Sizes\nof the atom<\/li>
  3. Bond\nlength<\/li><\/ol>\n\n\n\n

    Electronegativity difference of\nbonded atom<\/strong><\/h3>\n\n\n\n

    The\nbond energies of H-X type of compounds, where X= F, Cl, Br, I. electrons are\nnor equally shared between the bonded atoms i.e. HX. As halogen atom is more\nelectronegative, the bonded pair is more attracted towards X atom and thereby\npolarity develop. This give rise to additional attractive force for binding.<\/p>\n\n\n\n

    For\nexample: calculate the increase in the strength of H-Cl bond due to ionic\ncharacter present in it.<\/p>\n\n\n\n

    The\nH-H bond energy is 436 kJ\/mol<\/p>\n\n\n\n

                                           H + H \u2192\nH2<\/sub>                               \n\u0394H = -436 kJ\/mol<\/p>\n\n\n\n

    It\nmeans 436 kJ\/mol of heat is required to break the Avogadro\u2019s number of H2 <\/sub>molecules\ninto individual atoms. Thus, bond energy per bond is 72.42 x 1023<\/sup>\nkJ\/mol. This is obtained by dividing 436 by 6.02 x 10 23<\/sup>. As the\nbonding electron pair is equally shared between the two H-atoms, we assume that\neach bonded H-atom contributes half of the bond energy i.e., 36.21 x1023<\/sup>Kj\/mol.<\/p>\n\n\n\n

    Similarly, the bond energy for Cl2 is 240 kJ\/mol. Therefore each Cl-atom should contribute 19.93 x 1023 kJ to any bond where sharing of an electron pair is equal. This bond is polar so bond energy of H-Cl is 56.14 x 1023 kJ per molecule which is the sum of 36.21 x1023 and 19.93 x 1023 kJ. For Avogadro\u2019s number of HCl molecule, the calculated bond energy is 337.96 kJ\/mol, which is obtained by multiplying 56.14 x 10 23<\/sup> with 6.02 x 1023<\/sup>. <\/p>\n\n\n\n

    The\nbonds with higher bond energy values have shorter bond lengths. The bond\nenergies of C to C bonds being in the order C=C \u02c3 C=C \u02c3 C-C. Their bond\nlength are in the reverse order i.e., C-C \u02c3 C=C \u02c3 C=C<\/p>\n\n\n\n

    Size of the Atom<\/strong><\/h3>\n\n\n\n

    There is a direct relationship between the size of atom and bond dissociation. Larger the atomic size of atom lesser the energy will be required to break the bond. For example HI. Iodine is larger as compared to other elements in the halogens group so the attraction from the nucleus and outermost orbit is low. So a small amount of energy is required to break the bond.<\/p>\n\n\n\n

    Bond length <\/strong><\/h3>\n\n\n\n

    The distance between the nuclei of two atoms forming a covalent bond is called the bond length. The bond lengths are experimentally determined by physical techniques [3]. The techniques may be electron diffraction, X-ray diffraction or spectral studies. The covalent bond length between two atoms is often but not always independent of the nature of the molecules. For example, the bond length of C-C is 154 pm, it is also found to be same in the diamond. <\/p>\n\n\n\n

    The covalent radii for different elements are almost addictive in nature. The single bond covalent radius of carbon is 77 pm which is half of the C-C bond length (154 pm). Similarly, the covalent radius of Cl is 99 pm i.e. one half of the Cl-Cl bond length (198). So the bond length of C-Cl will be 77 + 99 =176 pm.<\/p>\n\n\n\n

    With the increase in electronegativity difference between the bonded atoms, the bond becomes shortened. The ionic character results in shortening of the bond length due to the force of attraction between polar ends. Moreover, the hybridization scheme involved, also explains the shortening of bonds due to the predominant participation of s- orbitals. Since, the 2s- orbital of carbon has a smaller mean radius than the 2p-orbitals, greater the s character in the hybrid orbital shorter will be the bond distance. Thus C-C bond lengths are 154, 133 and 120pm for ethane, ethane and ethyne. The \u03c0 bonding also reduces bond distance. The bond length increases as we move from top to bottom in IV-A group of the periodic table. Thus Si-Si bond length is greater than C-C in group IV-A and P-P bond length is greater than N-N. As the atomic radii increases in the group, the effect of the effective nuclear charge decreases on electron.<\/p>\n\n\n\n

    \u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0 In the periodic table shortening of bond, length occurs from left to right in a periodic table. Therefore C-C bond length is greater than N-N bond length. <\/p>\n\n\n\n

    Enthalpy changes of reaction from\nbond enthalpies<\/strong><\/h3>\n\n\n\n

    In Gaseous Phase <\/strong><\/p>\n\n\n\n

    In gas-phase we can easily use bond enthalpies [4]. For example in the reaction of carbon monoxide and steam hydrogen is produced.<\/p>\n\n\n\n

                 CO (g)<\/sub> + H2<\/sub>O\n(g)<\/sub> \u2192 CO2 (g)<\/sub> + H2 (g)<\/sub><\/p>\n\n\n\n

     The bond enthalpies are:<\/p>\n\n\n\n
    \n  \n <\/td>\n Bond enthalpy (kJ\/mol)\n <\/td><\/tr>
    \n C-O in carbon monoxide\n <\/td>\n +1077\n <\/td><\/tr>
    \n C-O in carbon dioxide\n <\/td>\n +805\n <\/td><\/tr>
    \n O-H\n <\/td>\n +464\n <\/td><\/tr>
    \n H-H\n <\/td>\n +436\n <\/td><\/tr><\/tbody><\/table>\n\n\n\n

    Now\nsolve the equation to find the enthalpy change in the reaction.<\/p>\n\n\n\n

    \u0394H\n+ 2(805) +436 = 1077 + 2(464)<\/p>\n\n\n\n

    \u0394H=\n1077 + 2(464) – 2(805) \u2013 436<\/p>\n\n\n\n

    \u0394H=\n-41 kJ\/mol<\/p>\n\n\n\n

    Shortcut\nmethod for simple cases<\/p>\n\n\n\n

    In\nsome cases where there is small changes occur in the molecule like chlorine\nreacts with ethane and produce chloroethane and hydrogen chloride. <\/p>\n\n\n\n

                                           C2<\/sub>H6<\/sub>\n+ Cl2<\/sub> \u2192 C2<\/sub>H5<\/sub>Cl + HCl<\/p>\n\n\n\n

    The\nchanged is that actually C-H bond and Cl-Cl bond broken and made a new C-Cl\nbond and H-Cl bond.<\/p>\n\n\n\n
    \n  \n <\/td>\n Bond enthalpy (kJ\/mol)\n <\/td><\/tr>
    \n C-H\n <\/td>\n +413\n <\/td><\/tr>
    \n Cl-Cl\n <\/td>\n +243\n <\/td><\/tr>
    \n C-Cl\n <\/td>\n +346\n <\/td><\/tr>
    \n H-Cl\n <\/td>\n +432\n <\/td><\/tr><\/tbody><\/table>\n\n\n\n

    Energy\nrequired to break C-H and C-Cl<\/p>\n\n\n\n

    +413\n+ 243 = +656 kJ\/mol<\/p>\n\n\n\n

    Energy\nreleased when make C-Cl and H-Cl<\/p>\n\n\n\n

    -346\n\u2013 432 =-778 kJ\/mol<\/p>\n\n\n\n

    So\nnet change is +656-778= -122 kJ\/mol<\/p>\n\n\n\n

    Liquid phase <\/strong><\/p>\n\n\n\n

    Bond\nenergy is working directly in the gas phase but in liquid extra energy is\nrequired to convert liquid into gas that is called enthalpy change of\nvaporization. It is represented by the symbol \u0394Hvap <\/sub>or \u0394Hv<\/sub>.<\/p>\n\n\n\n

    This\nenthalpy change is defined as when 1 mole of the liquid convert into gas at its\nboiling point with a pressure of 1 bar.<\/p>\n\n\n\n

    For\nwater: \u0394Hvap<\/sub> is +41 kJ\/mol, it means that it take 41 kJ to change 1\nmol of water into steam, changing liquid into gas required heat and reverse\nback reaction of changing gas to liquid also required same amount of heat,<\/p>\n\n\n\n

    For\nexample, combustion of methane        <\/p>\n\n\n\n

                     CH4<\/sub> + 2O2<\/sub>\n\u2192 CO2<\/sub> + 2 H2<\/sub>O<\/p>\n\n\n\n

         The bond enthalpies are <\/p>\n\n\n\n
    \n  \n <\/td>\n Bond enthalpy (kJ\/mol)\n <\/td><\/tr>
    \n C-H\n <\/td>\n +413\n <\/td><\/tr>
    \n O=O\n <\/td>\n +498\n <\/td><\/tr>
    \n C=O in carbon dioxide\n <\/td>\n +805\n <\/td><\/tr>
    \n O-H\n <\/td>\n +464\n <\/td><\/tr><\/tbody><\/table>\n\n\n\n

    Now\ncalculations<\/p>\n\n\n\n

    \u0394H\n+2(805) + 2(41) + 4(464) = 4(413) + 2(498)<\/p>\n\n\n\n

    \u0394H\n= 4(413) + 2(498) – 2(805) – 2(41) – 4(464) <\/p>\n\n\n\n

    \u0394H=\n-900 kJ\/mol<\/p>\n\n\n\n

    References <\/strong><\/p>\n\n\n\n

    1.  IUPAC<\/a>, Compendium of Chemical Terminology<\/a>,\n2nd ed. (the “Gold Book”) (1997). Online corrected version:\n (2006\u2013) “Bond\nenergy (mean bond energy)<\/a>“. doi<\/a>:10.1351\/goldbook.B00701<\/a><\/li>
    2. https:\/\/en.wikipedia.org\/wiki\/Bond_energy<\/a><\/li>
    3. https:\/\/chem.libretexts.org\/Bookshelves\/Physical_and_Theoretical_Chemistry_Textbook_Maps\/Supplemental_Modules_(Physical_and_Theoretical_Chemistry)\/Chemical_Bonding\/Fundamentals_of_Chemical_Bonding\/Chemical_Bonds\/Bond_Lengths_and_Energies<\/a><\/li>
    4. https:\/\/www.chemguide.co.uk\/physical\/energetics\/bondenthalpies.html<\/li><\/ol>\n","protected":false},"excerpt":{"rendered":"

      Definition \u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0 When a bond is formed between two atoms, energy is released. The same amount of energy is absorbed when the bond is broken to form neutral atoms. So, \u2018\u2019the bond energy is the average amount of energy required to break all bonds of a particular type in one mole of the substance\u2019\u2019. Explanation … Read more<\/a><\/p>\n","protected":false},"author":6,"featured_media":0,"comment_status":"closed","ping_status":"open","sticky":false,"template":"","format":"standard","meta":{"rating_form_position":"","rating_results_position":"","mr_structured_data_type":""},"categories":[2],"tags":[],"multi-rating":{"mr_rating_results":[{"adjusted_star_result":3.67,"star_result":3.67,"total_max_option_value":5,"adjusted_score_result":3.67,"score_result":3.67,"percentage_result":73.33,"adjusted_percentage_result":73.33,"count":3,"post_id":991}]},"_links":{"self":[{"href":"https:\/\/chemdictionary.org\/wp-json\/wp\/v2\/posts\/991"}],"collection":[{"href":"https:\/\/chemdictionary.org\/wp-json\/wp\/v2\/posts"}],"about":[{"href":"https:\/\/chemdictionary.org\/wp-json\/wp\/v2\/types\/post"}],"author":[{"embeddable":true,"href":"https:\/\/chemdictionary.org\/wp-json\/wp\/v2\/users\/6"}],"replies":[{"embeddable":true,"href":"https:\/\/chemdictionary.org\/wp-json\/wp\/v2\/comments?post=991"}],"version-history":[{"count":2,"href":"https:\/\/chemdictionary.org\/wp-json\/wp\/v2\/posts\/991\/revisions"}],"predecessor-version":[{"id":1037,"href":"https:\/\/chemdictionary.org\/wp-json\/wp\/v2\/posts\/991\/revisions\/1037"}],"wp:attachment":[{"href":"https:\/\/chemdictionary.org\/wp-json\/wp\/v2\/media?parent=991"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/chemdictionary.org\/wp-json\/wp\/v2\/categories?post=991"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/chemdictionary.org\/wp-json\/wp\/v2\/tags?post=991"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}