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MightySmurf
 3 years ago
For each of the following sets of ions, rank them from smallest to largest ionic radius.
MightySmurf
 3 years ago
For each of the following sets of ions, rank them from smallest to largest ionic radius.

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heena
 3 years ago
Best ResponseYou've already chosen the best response.0do you need a reason too..???????

MightySmurf
 3 years ago
Best ResponseYou've already chosen the best response.0no just need help with more if you dnt mind

MightySmurf
 3 years ago
Best ResponseYou've already chosen the best response.0b. Mg²+, Ca²+,Ba²+ c.F,Cl, Br d.Ba²+,Cu²+,Zn²+ e. Si⁴, P³, O²

heena
 3 years ago
Best ResponseYou've already chosen the best response.0ok in anion the greater will be the charge more will be the radius because when we add an electron no. of proton decreases as compare to electron which means nucleous effective charge decreaes as a rseult size increaes in anion more the positive charge less the radius as proton no. increses because of lose of an electron means more nuclear charge which attracts the electron present aND bring closer as a result bond length decreases

heena
 3 years ago
Best ResponseYou've already chosen the best response.0conclusion: in anion more charge greater radius in cation more charge smaller radius

heena
 3 years ago
Best ResponseYou've already chosen the best response.0as u know down the group bond length increaes and if there is charge also same then we will use normal trend b)Mg2+ < Ca2+ <Ba2+ c)f < Cl < Br d) Cu 2+< Zn 2+ <Ba 2+ (as u know in period bond length decrease e)O2 <P3 < Si 4 ( in isolelectronic species we will also consider the same method acc. to charge)
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