To which of the following atoms is the attach | vedclass

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(A) The difficulty of electron attachment is related to the electron gain enthalpy. $A$ positive or very low negative electron gain enthalpy indicates

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Radon

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(A) The difficulty of electron attachment is related to the electron gain enthalpy. $A$ positive or very low negative electron gain enthalpy indicates that the process is difficult.$A)$ Radon $(Rn)$ is a noble gas with a stable,fully filled valence shell configuration: $[Xe] 4f^{14} 5d^{10} 6s^2 6p^6$. It has no tendency to accept an electron,making the process highly endothermic and most difficult.$B)$ Nitrogen $(N)$ has a half-filled $2p$ subshell: $[He] 2s^2 2p^3$. This provides extra stability,making electron attachment difficult,but less so than for a noble gas.$C)$ Oxygen $(O)$ has a $2p^4$ configuration and readily accepts an electron to achieve a more stable state.$D)$ Radium $(Ra)$ is an alkaline earth metal with a $7s^2$ configuration. While it has a low electron affinity,it is still more likely to accept an electron than a noble gas.Therefore,the attachment of an electron is most difficult for Radon.

To which of the following atoms is the attachment of an electron most difficult?

Similar Questions

The increasing order of electron affinity for the given electronic configurations of elements is:
$I$. $1s^2 \ 2s^2 \ 2p^6 \ 3s^2 \ 3p^5$ $(Cl)$
$II$. $1s^2 \ 2s^2 \ 2p^3$ $(N)$
$III$. $1s^2 \ 2s^2 \ 2p^5$ $(F)$
$IV$. $1s^2 \ 2s^2 \ 2p^6 \ 3s^2 \ 3p^1$ $(Al)$

Which of the following elements will have the lowest electron affinity?

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