Question

8.
Imagine, which one in each of the following pairs is large in size relatively
with other ? Explain.
(X) Na, Al (Y) Na, Mg+2



i will mark brainliest for best answer​

Answer 1

hey mate here is your answer

(Y) Na, Mg2

explanation: The sodium (Na) is higher reactive metal due to less valency (1). In this case the magnesium (Mg2) is moderate reactive metal due to one more valency (2). The aluminium is less reactive metal with valency 3.

If u prefer the electronic configuration, valence electrons and valency of this three elements, it will be more clear to u.

Hope it helped u.......

Answer 2

Na is larger than aluminium.

Na is larger than $Mg^{2+}$

Explanation:

Atomic radius of an atom is defined as the total distance from the nucleus to the outermost shell of the atom.

1. On moving from left to right in a period, more and more electrons get added up in the same shell and the attraction between the last electron and nucleus increases, which results in the shrinkage of size of an atom. Thus, decreasing the atomic radii of the atom on moving towards right of the periodic table.

As Al lies right to Na in the periodic table, Al is smaller in size as compared to Na.

2.  Isoelectronic molecules are defined as the molecules which have the same electronic structure and have the same number of valence electrons.

For

Electrons of magnesium are 12 , and on losing 2 electrons the electrons are 10.

$[Mg]:12:1s^22s^22p^63s^2$

$[Mg^{2+}]:1:1s^22s^22p^63s^0$

For Na

Electrons of sodium are 11.

$[Na]:10:1s^22s^22p^63s^1$

As, the total number of electrons of  and Na are same, but as Mg has more protons, the attraction towards electrons will be more and hence  $Mg^{2+}$ will be smaller in size.

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