Bond enthalpy of fluorine is lower than that of chlorine why
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Fluorine atoms have the smallest radii so it can be supposed that they have the greatest attraction of their nuclei to the shared pair of electrons which would thus make the covalent bond very hard to break indeed.But,
Such a strong nuclear attraction to the valence electrons , however means that inter-electronic repulsion will exist- electrons within the small F-F molecule will repel each other due to the valence electrons being closer to the other electrons (due to the stronger nuclear attraction) which will in turn weaken the F-F bond and result in it having a small bond enthalpy
Such a strong nuclear attraction to the valence electrons , however means that inter-electronic repulsion will exist- electrons within the small F-F molecule will repel each other due to the valence electrons being closer to the other electrons (due to the stronger nuclear attraction) which will in turn weaken the F-F bond and result in it having a small bond enthalpy
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Hey !!
Bond enthalpy of F ---- F is smaller due to greater repulsive interactions between the lone pair of one F atom with those of other. The repulsive interactions arise due to greater concentration of electron density on each F atom because of it's extremely small size.
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