The given question is about comparing electron gain enthalpies of some element pairs. Electron gain enthalpy is a measure of the energy change when an electron is added to a neutral atom to form a negative ion.
Let's go through each of the options:
Cl, Ar: Chlorine (Cl) has a high electron gain enthalpy because adding an electron completes its valence shell, resulting in a stable electronic configuration. Argon (Ar), being a noble gas with a completely filled valence shell, has an electron gain enthalpy of zero as it does not gain electrons easily.
Cl, Ne: Similar to the above, Cl has a high electron gain enthalpy. Neon (Ne), another noble gas with a filled outer shell, also has an electron gain enthalpy near zero. The difference between Cl, which strongly attracts an additional electron, and Ne, which does not want an additional electron, results in a large difference in electron gain enthalpy.
F, Ar: Fluorine (F) has an even higher electron gain enthalpy than Cl because it is more electronegative and has a higher tendency to gain electrons to achieve stability. Argon (Ar) has an electron gain enthalty near zero due to its stable configuration.
F, Ne: Similar to F, Ne is also a noble gas and its electron gain enthalpy is near zero. Thus, the difference between F and Ne is large but not as much as the difference between Cl and Ne.
Considering these comparisons, the pair with the highest difference in electron gain enthalpy is Cl, Ne. Therefore, the correct answer is:
Cl, Ne
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