its hard to understand why since Z effective for any element shows that it attracts electrons and the work done by the whole system in the diplacement of the electron by the force exerted by the effective nuclear charge will lowerise energy,as given by the formula U=-W,assuming U initial zero for the system.
Inert gases are the most stable ones, so if we try to add another electron, the stable electronic configuration is disturbed. So, we have supply energy for this process. Hence, electron gain enthalpy is positive.
Electron affinity is the energy released when an atom gains an electron to form a negative ion, while electron gain enthalpy is the enthalpy change accompanying the addition of an electron to a gaseous atom. Electron affinity is a specific term used in the context of forming an ion, while electron gain enthalpy is a general term for the enthalpy change associated with gaining an electron.
The electron gain enthalpy of hydrogen is approximately -72.8 kJ/mol, indicating that it releases energy when gaining an electron. In contrast, the electron gain enthalpy of phosphorus is approximately -78.6 kJ/mol, showing a larger energy release when phosphorus gains an electron due to its higher electronegativity.
It should be Fluorine but Chlorine has most EGE value because the F atom has very small sizeas compared to Cl. Addition of extra electron creates higher electron density and thus strong electron - electron repulsion comes into act. So extra electron is not accepted with the same ease as in the case of remaining elements of the group
Electron Gain Enthalpy is the amount of Energy released when an isolated gaseous atom accepts an electron to become a monovalent gaseous anion.For Example:Atom(gas) +Electron ---->Anion(gas) +Energy(Electron Gain Enthalpy)
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Even though Fluorine has the highest electronegativity among all the elements and it should have the highest electron gain enthalpy among all the halogens but this is an exception and chlorine has higher electron gain enthalpy than Fluorine. The reason for this is that the size of Fluorine atom is very small and hence there is very high inter-electronic repulsion among the electrons of fluorine. This makes incoming of another electron not very favourable. Even though fluorine has large negative electron gain enthalpy but for chlorine its even more negative.
Good question. Halogens have their outer electronic configuration as ns2np5 and require only one more electron to gain a stable electronic configuration. So they have a great affinity for electrons and will accept them very easily by releasing energy. So they have the highest electron gain enthalpy.
Yes, the elements in Group 14 (carbon, silicon, germanium, tin, and lead) generally have a decreasing trend in electron gain enthalpy as you move down the group. This is due to increasing atomic size and shielding effect, which make it less favorable for larger atoms to gain electrons. Thus, carbon has the highest electron gain enthalpy, followed by silicon, germanium, tin, and lead in decreasing order.
The second electron gain of an oxygen atom would be expected to be less negative. The reason for this outcome is that the oxygen atom gaining a second electron already has one electron and thus a negative charge. This negative charge repels the second electron to some extent, making the enthalpy of this process less negative than when the first electron was added to the neutral oxygen atom.
In a nitrogen atom's ground state, it has five atoms. The electron will have to gain three electrons to become stable.
Nitrogen has to gain three electrons