Given below are two statements: Statement I: Fluorine has most negative electron gain enthalpy in its group. Statement II: Oxygen has least negative electron gain enthalpy in its group. In the light of the above statements, choose the most appropriate from the options given below.
To analyze the statements given in the question, we need to understand the concept of electron gain enthalpy within the groups of the periodic table.
Statement I: "Fluorine has the most negative electron gain enthalpy in its group."
Explanation: Electron gain enthalpy refers to the energy change when an electron is added to an isolated gaseous atom. In general, as we move across a period from left to right, electron gain enthalpy becomes more negative. However, this trend doesn't hold perfectly in a group. For Group 17 (halogens), chlorine actually has a more negative electron gain enthalpy than fluorine. This is due to the smaller atomic size of fluorine, resulting in a higher electron-electron repulsion in its compact structure, making chlorine's electron addition more favorable. Therefore, Statement I is false.
Statement II: "Oxygen has the least negative electron gain enthalpy in its group."
Explanation: Oxygen is part of Group 16. Within this group, oxygen does indeed have the least negative electron gain enthalpy. This is because, like with fluorine, the small size of the oxygen atom leads to increased electron-electron repulsion upon gaining an additional electron. Thus, Statement II is true.
Conclusion: Based on the explanations above, the most appropriate choice is: "Statement I is false but Statement II is true."
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Statement I is false because chlorine has the most negative electron gain enthalpy in its group. Statement II is true as oxygen has the least negative electron gain enthalpy in its group. The Correct Answer is: Statement I is false but Statement II is true
