Question

Can someone help me
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Answer 1

$\huge\bf\mathfrak{QUESTION\: :}$

Arrange the following in the increasing order of ionic radii :

$( {f}^{ - } )({o}^{2 - } )( {mg}^{2 + } )( {na}^{ + } )$

$\huge\bf\mathcal{ATOMIC \: RADIUS\: :}$

Atomic radius is generally stated as being the total distance from an atom’s nucleus to the outermost orbital of electron.

In simpler terms, it can be defined as something similar to the radius of a circle, where the center of the circle is the nucleus and the outer edge of the circle is the outermost orbital of electron

$\huge\bf\mathcal{PERIODIC\: TRENDS\: :}$

An atom gets larger as the number of electronic shells increase; therefore the radius of atoms increases as you go down a certain group in the periodic table of elements.

In general, the size of an atom will decrease as you move from left to the right of a certain period

$\huge\bf\mathfrak{IONIC\: TRENDS\: :}$

Cations have smaller ionic radii than their neutral atoms.

In contrast, anions have bigger ionic radii than their corresponding neutral atoms.

$\huge\bf\mathfrak{ANSWER\: :}$

As the electronic configuration of all given elements is same

i.e 2,8

we will follow ionic trends

Hence the correct increasing order is

${mg}^{2 + } < {na}^{ + } < {f}^{ - } < {o}^{2 - }$