Question

question 19
select the reaction that will require the greatest amount of energy.
o o(g)→o^{+}(g)+e^{-}
o f^{+}(g)→f^{2+}+e^{-}
o o^{+}(g)→o^{2+}+e^{-}
o f(g)→f^{+}(g)+e^{-}

Explanation:

Ionization energy is the energy required to remove an electron from an atom or ion in the gaseous state. Fluorine (F) has a very high electronegativity and a small atomic radius. The second ionization energy (removing an electron from \(F^{+}\) to form \(F^{2+}\)) is extremely high because \(F^{+}\) has a stable electron configuration similar to a noble - gas - like configuration (after losing one electron, it has a more stable arrangement, and removing a second electron disrupts this relative stability). Oxygen (O) has a lower ionization energy compared to fluorine in general. For \(O(g)\to O^{+}(g)+e^{-}\), it is the first ionization energy of O. For \(O^{+}(g)\to O^{2+}(g)+e^{-}\), it is the second ionization energy of O. But fluorine's ionization energies are higher due to its higher nuclear charge and smaller size. Among the given options, \(F^{+}(g)\to F^{2+}+e^{-}\) requires the greatest amount of energy.

Answer:

\(F^{+}(g)\to F^{2+}+e^{-}\)