The correct sequence of electron gain enthalpy of the elements listed below is A. Ar B. Br C. F D. S Choose the most appropriate from the options given below:
Understanding Electron Gain Enthalpy: Electron gain enthalpy is the amount of energy released when an electron is added to a neutral atom in the gaseous state to form a negative ion. Higher negative values indicate that an element releases more energy when gaining an electron, signifying higher electron affinity.
Considering the Elements: We need to arrange Ar, Br, F, and S based on their electron gain enthalpy.
Argon (Ar): As a noble gas, Argon has a complete octet, making its electron affinity negligible.
Fluorine (F): Fluorine has a high electron affinity because it is one electron short of a complete octet, and it is known for having the highest electron affinity among halogens.
Bromine (Br): Bromine, being another halogen, also exhibits high electron affinity but not as much as Fluorine. It has less electron gain enthalpy compared to Fluorine.
Sulfur (S): Sulfur has a moderate electron affinity. It is less than that of halogens like Bromine or Fluorine.
Ranking based on Electron Gain Enthalpy: Considering the above information, the order of electron gain enthalpy from the most negative (most energy release) to the least is as follows:
The least electron gain enthalpy is Argon because it is a noble gas.
After Argon, Sulfur has lower electron gain enthalpy than Bromine.
Bromine has lower electron gain enthalpy than Fluorine.
Thus, the order is: \(A \gt D \gt B \gt C\)
Conclusion: Therefore, the correct sequence of electron gain enthalpy for the given elements is A > D > B > C.
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Approach Solution -2
\(Element\)
\(\Delta_{eg}\)\(H\) , \((\text{kJ/mol})\)
F
\(-333\)
S
\(-200\)
Br
\(-325\)
Ar
\(+96\)
Thus the correct answer is Option 2.
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