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MightySmurf Group Title

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

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  1. MightySmurf Group Title
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    a. Mg²+,Si⁴-, S²-

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  2. heena Group Title
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    Mg2+< S2- < S 4-

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  3. heena Group Title
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    do you need a reason too..???????

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  4. MightySmurf Group Title
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    no just need help with more if you dnt mind

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  5. MightySmurf Group Title
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    b. Mg²+, Ca²+,Ba²+ c.F-,Cl-, Br- d.Ba²+,Cu²+,Zn²+ e. Si⁴-, P³-, O²-

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  6. heena Group Title
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    ok 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

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    conclusion: in anion more charge greater radius in cation more charge smaller radius

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  8. heena Group Title
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    as 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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