The electron affinity values are negative for | vedclass

Name: Exam Paper Generator | JEE NEET Paper Generator | Vedclass
Brand: Vedclass
Rating: 5 (35 reviews)

Question

(D) Electron affinity is the energy released when an electron is added to a neutral gaseous atom or ion.$A$. $Be (2s^2)$ has a stable fully-filled con

Vedclass · Accepted Answer

$A, B$ and $C$ only

Vedclass · Answer

(D) Electron affinity is the energy released when an electron is added to a neutral gaseous atom or ion.$A$. $Be (2s^2)$ has a stable fully-filled configuration. Adding an electron is unfavorable,making the electron affinity negative (energy must be supplied).$B$. $N (2s^2 2p^3)$ has a stable half-filled configuration. Adding an electron is unfavorable,making the electron affinity negative.$C$. $O^{-} + e^{-} \rightarrow O^{2-}$. Adding an electron to a negatively charged ion $(O^{-})$ experiences strong inter-electronic repulsion,making the process endothermic (negative electron affinity).$D$. $Na (3s^1)$ has a low energy orbital available. Adding an electron releases energy (positive electron affinity).$E$. $Al (3s^2 3p^1)$ has an available $3p$ orbital. Adding an electron releases energy (positive electron affinity).Therefore,the processes $A, B,$ and $C$ have negative electron affinity values.

The electron affinity values are negative for:
$A$. $Be \rightarrow Be^{-}$
$B$. $N \rightarrow N^{-}$
$C$. $O^{-} \rightarrow O^{2-}$
$D$. $Na \rightarrow Na^{-}$
$E$. $Al \rightarrow Al^{-}$
Choose the most appropriate answer from the options given below:

Similar Questions

The electron affinity values of elements $A, B, C$ and $D$ are respectively $-135, -60, -200$ and $-348 \ kJ \ mol^{-1}$. The outer electronic configuration of element $B$ is

In which of the following pairs,electron gain enthalpies of constituent elements are nearly the same or identical?
$A$. $Rb$ and $Cs$
$B$. $Na$ and $K$
$C$. $Ar$ and $Kr$
$D$. $I$ and $At$
Choose the correct answer from the options given below.

The energy evolved is highest for which of the following reactions?

Which halogen has the highest value of negative electron gain enthalpy?

Given below are two statements:
Statement $I$: Fluorine has most negative electron gain enthalpy in its group.
Statement $II$: Oxygen has least negative electron gain enthalpy in its group.
In the light of the above statements,choose the most appropriate from the options given below.

Vedclass Test Series

Exam Paper Generator

Online Exam Module

The electron affinity values are negative for:$A$. $Be \rightarrow Be^{-}$$B$. $N \rightarrow N^{-}$$C$. $O^{-} \rightarrow O^{2-}$$D$. $Na \rightarrow Na^{-}$$E$. $Al \rightarrow Al^{-}$Choose the most appropriate answer from the options given below: