In noble gases, the outer s and p orbitals are filled. No more electrons can be filled in their orbitals. The electron gain enthalpy of noble gases is zero.
The electron gain enthalpy of noble gases is always positive because it will require a large amount of energy to add a electron(as it has completely filled orbitals).
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Yukti Prabhakar answered this
Because as the noble gas elements having completely filled or exactly half filled electronic configuration &are very stable so the energy has to supplied by the addition of electrons hence requires large amount of positive values of electron gain enthalpies
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Yogesh Kataria answered this
It is so because they have fully filled orbitals and hence when an electron comes , then all other electrons provides large hinderance to the incoming electron and hence energy is given to compensate the repulsion and so the electron gain enthalpy of noble gases is always positive.
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Somya Dipayan Majhi answered this
Electron Gain Enthalpy of Noble gases is always Positive as A large amount of energy to add an extra electron as Noble gases have a stable Electronic Configuration i.e Their orbitals are completely filled .
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Ravi Sharma answered this
inert gases have zero electron gain enthalpy
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Sujeet answered this
Give reasons-
(A) ionisation enthalpy of Mg is more than Al.
(B) electron gain enthalpy of flourine is less than chlorine.
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Ashu answered this
bcoz noble gases have thier fulfiled outermost electronic configuration. thus they doesnot need any electron in thier higher orbitals. for for accepting electron in higher orbitals of noble gas , external energy is used to give .therefore electron gain energy of noble gases is always positive.
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Ritik Narayan answered this
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Kundan Kumar answered this
Due to full filled and half filled electronic configuration a lot of energy is required to add electronic as a result its electron gain enthalpy is always positive
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...... __ answered this
Noble gases have large positive electron gain enthalpy. This is because the extra electron is placed in the next higher principal quantum energy levels. Thus, a highly unstable electronic configuration is produced.