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Study the graph and answer the questions that follow:1. On moving down a group what happens to electron gain enthalpy?2. Why chlorine shows more negative electron gain enthalpy than fluorine? |
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Answer» 1. On moving down a group, electron gain enthalpy becomes less negative because the size of the atom increases and the added electron would be farther from the nucleus. 2. Due to small size of F, the added electron goes to the smaller 2p quantum level and suffers significant replusion from the other electrons present in this level. But due to big size of Cl, the added electron goes to the n = 3p quantum level and occupies a larger region of space and the electron electron repulsion is much less. 1-->>The electron gain enthalpy becomes less negative as we move down a group. 2-->>>The negative electron gain enthalpy of fluorine is less than that of chlorine. It is due to small size of fluorine atom. As a result, there are strong interelectronic repulsions in the relatively small 2p orbitals of fluorine and thus, the incoming electron does not experience much attraction. |
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