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electron gain enthalpy increases from F to Cl but then decreases . so can we say the more electron repulsion the less electron gain enthalpy and the less electron repulsion the more the electrongain enthalpy . what about bromine and Iodine , does the electron gain enthalpy decrease due to the presence of a d-orbital ? electron gain enthalpy increases from F to Cl but then decreases . so can we say the more electron repulsion the less electron gain enthalpy and the less electron repulsion the more the electrongain enthalpy . what about bromine and Iodine , does the electron gain enthalpy decrease due to the presence of a d-orbital ?
electron gain enthalpy increases from F to Cl but then decreases . so can we say the more electron repulsion the less electron gain enthalpy and the less electron repulsion the more the electrongain enthalpy . what about bromine and Iodine , does the electron gain enthalpy decrease due to the presence of a d-orbital ?
on moving down the group the atomic size as well as nuclear charge inreases.But the effect of increase in atomic size is much more pronounced than that of nuclear charge and thus the additional electrons feels less attraction consequently electron gain enthalpy becomes less negative on going down the groupX (g) + e- ===> X- (g)F = -328 kJ/molCl = -349 kJ/molBr = -325 kJ/molI = -295 kJ/molHowever the electron gain enthalpy of F is less negative than of Cl because of its small size. The additional electron in case of F will be added to the 2p orbital while in case of Cl it will go in the 3p orbital. As a 2p orbital occupies a smaller region of space than 3p orbital, it will be more compact because of which electron-electron repulsions would be more. Therefore the incoming electron would be accepted with much less ease in case of F. Hence its electron gain enthalpy is less negative than Cl.
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