11. A species is said to be paramagnetic if it has unpaired electrons in its outermost shell.
a) Electronic configuration of Fe = 3d6 4s2
Electronic configuration of Fe3+ = 3d5
Each d- orbital will have 1 unpaired electron and a total of 5 unpaired electrons. So, it will be paramagnetic.
b) Electronic configuration of Sr = 4p6 5s2
Electronic configuration of Sr2+ = 4p6
There are no unpaired electrons, so it will be diamagnetic.
c) electronic configuration of O = 2p4
Electronic configuration of O2- = 2p6
There are also no unpaired electrons, so it will be diamagnetic.
d) electronic configuration of Mg = 3s2
The electrons are paired and hence, it is diamagnetic
e) electronic configuration of Zn = 3d10 4s2
Electronic configuration of Zn2+ = 3d10
So, this is also diamagnetic.
Hence, Fe3+ is paramagnetic among given species.
12. For comparing ionic radius, first check whether the species are isoelectronic (containing same number of electrons).
In this case, all the given species are isoelectronic containing 36 electrons.
In such a case ionic radius varies as: Anion > Neutral species > Cation
And, ionic radius of more charged anionic species > ionic radius of less charged anionic species.
Ionic radius of less charged cationic species > ionic radius of more charged cationic species.
Therefore, order of ionic radius: Se2- > Br- > Sr2+.
Option E is correct.
13.
Version 1 11) Which of the following species would be paramagnetic? A) Fest B) Sr C)...
Which of the following radii comparisons is incorrect? A) Sr²⁺ < Sr B) Br⁻ < Br C) Fe³⁺ < Fe²⁺ D) Se²⁻ > Se E) Sn²⁺ > Sn⁴⁺
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