which of the folllowing species is not isoelctric with any of the others?
a)V3+
b)Ca2+
c)Ar
d)CL-
e)S2-
To determine which of the following species is not iso-electric with any of the others, we need to understand what it means for species to be iso-electric.
Iso-electric species are those that have the same number of electrons. In other words, they have the same electronic configuration.
Let's analyze each option one by one:
a) V3+: Vanadium(V) ion loses three electrons, resulting in a 3+ charge. To determine its electronic configuration, we need to look at the electron configuration of neutral vanadium (V). The electron configuration of neutral vanadium is [Ar] 4s2 3d3. By removing three electrons, we get [Ar] 3d3. So, V3+ has the same electron configuration as Argon (Ar).
b) Ca2+: Calcium(II) ion loses two electrons, resulting in a 2+ charge. The electronic configuration of neutral calcium is [Ar] 4s2. By removing two electrons, we get [Ar]. Thus, Ca2+ has the same electron configuration as Argon (Ar).
c) Ar: Argon is a noble gas with an electron configuration of [Ne] 3s2 3p6. It already has a stable and full valence shell, so it does not lose or gain electrons. Therefore, the electron configuration of Ar remains unchanged.
d) Cl-: Chloride ion gains one electron, resulting in a 1- charge. The electron configuration of neutral chlorine is [Ne] 3s2 3p5. By gaining one electron, it becomes [Ne] 3s2 3p6, which is the same electron configuration as Argon (Ar).
e) S2-: Sulfide ion gains two electrons, resulting in a 2- charge. The electron configuration of neutral sulfur is [Ne] 3s2 3p4. By gaining two electrons, it becomes [Ne] 3s2 3p6, which is the same electron configuration as Argon (Ar).
Based on the analysis above, all of the given species (V3+, Ca2+, Ar, Cl-, and S2-) have the same electron configuration as Argon (Ar). Therefore, they are all iso-electric with each other. None of them is not iso-electric with any of the others.