Observe the following data. IonRadius (pm)Q^{ | vedclass

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(D) The ions $Na^{+}, Mg^{2+}, Al^{3+}, Si^{4+}$ are isoelectronic with $10$ electrons each. For isoelectronic species, the ionic radius decreases as

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$Al^{3+}, Mg^{2+}, Si^{4+}, Na^{+}$

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(D) The ions $Na^{+}, Mg^{2+}, Al^{3+}, Si^{4+}$ are isoelectronic with $10$ electrons each. For isoelectronic species, the ionic radius decreases as the nuclear charge (atomic number) increases. The atomic numbers are: $Na (11), Mg (12), Al (13), Si (14)$. Ordering by increasing atomic number: $Na^{+} Therefore, the order of decreasing ionic radius is: $Na^{+} (100 \ pm) > Mg^{2+} (72 \ pm) > Al^{3+} (53 \ pm) > Si^{4+} (40 \ pm)$. Matching the given radii: $Y^{c+} = 40 \ pm = Si^{4+}$ $Q^{a+} = 53 \ pm = Al^{3+}$ $X^{b+} = 66 \ pm = Mg^{2+}$ $Z^{d+} = 100 \ pm = Na^{+}$ Thus, $Q^{a+}, X^{b+}, Y^{c+}, Z^{d+}$ are $Al^{3+}, Mg^{2+}, Si^{4+}, Na^{+}$.

Ion	Radius $(pm)$
$Q^{a+}$	$53$
$X^{b+}$	$66$
$Y^{c+}$	$40$
$Z^{d+}$	$100$

Observe the following data.
Ion Radius $(pm)$
$Q^{a+}$ $53$
$X^{b+}$ $66$
$Y^{c+}$ $40$
$Z^{d+}$ $100$
$Q^{a+}, X^{b+}, Y^{c+}, Z^{d+}$ are respectively

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Observe the following data. IonRadius $(pm)$$Q^{a+}$$53$$X^{b+}$$66$$Y^{c+}$$40$$Z^{d+}$$100$ $Q^{a+}, X^{b+}, Y^{c+}, Z^{d+}$ are respectively