Which of the following isoelectronic series w | vedclass

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

Question

(A) The given species $S^{2-}$,$Cl^{-}$,$Ar$,and $K^{+}$ are isoelectronic,meaning they all have $18$ electrons. For isoelectronic species,the ease of

Vedclass · Accepted Answer

$S^{2-}$

Vedclass · Answer

(A) The given species $S^{2-}$,$Cl^{-}$,$Ar$,and $K^{+}$ are isoelectronic,meaning they all have $18$ electrons. For isoelectronic species,the ease of losing an electron (ionization energy) depends on the nuclear charge (number of protons). As the nuclear charge increases,the attraction between the nucleus and the valence electrons increases,making it harder to remove an electron. The nuclear charges are: $S^{2-} (Z=16)$,$Cl^{-} (Z=17)$,$Ar (Z=18)$,and $K^{+} (Z=19)$. Since $S^{2-}$ has the lowest nuclear charge $(Z=16)$,it has the weakest hold on its electrons,making it the easiest to lose an electron.

Which of the following isoelectronic series would lose an electron most easily?

Similar Questions

Correct increasing order of first ionisation potential is

Identify the element having lowest first ionization enthalpy.

The first ionisation potentials $(eV)$ of $Be$ and $B$ respectively are :-

In the photoelectric effect,if the work functions of $Li$,$Na$,and $Rb$ are $2.41 \ eV$,$2.30 \ eV$,and $2.09 \ eV$ respectively,the work function of $K$ could approximately be in $eV$?

The atomic numbers of $V, Cr, Mn$ and $Fe$ are $23, 24, 25$ and $26$ respectively. Which of these elements will have the highest second ionization enthalpy?

Vedclass Test Series

Exam Paper Generator

Online Exam Module