Classification of Elements and Periodicity in Properties Set-2

Half the distance between two atoms when they are bound by a single covalent bond

The full internuclear distance between the atoms

Half the internuclear distance in a metallic crystal

Half the van der Waals radius

Twice the internuclear distance

Half the internuclear distance

Equal to the internuclear distance

$256\text{ pm}$

Effective nuclear charge decreases.

The principal quantum number ($n$) increases.

Effective nuclear charge increases, increasing attraction of electrons to the nucleus within the same valence shell

The number of core electrons increases drastically.

The nuclear charge decreases down the group.

The valence electrons are placed farther from the nucleus due to increased principal quantum number ($n$) and shielding

The electron gain enthalpy becomes more negative.

All inner energy levels are completely filled.

Smaller, due to increased effective nuclear charge

Larger, because the added electron increases repulsion and decreases effective nuclear charge

Smaller, because it has more protons

The same, as the nuclear charge is constant

The cation is larger because the remaining electrons are less attracted by the nucleus.

The cation is smaller because it has fewer electrons while the nuclear charge remains the same

The cation is the same size because only valence electrons are involved.

The cation's radius is half the atomic radius.

$\text{Mg}^{2+}$

$\text{Na}^{+}$

$\text{F}^{-}$

$\text{O}^{2-}$ (Anion with greater negative charge has larger radius due to net electron repulsion)

$\text{N}^{3-}$

$\text{O}^{2-}$

$\text{F}^{-}$

All are the same size

$\text{Mg}^{2+} < \text{Na}^{+} < \text{F}^{-}$

$\text{F}^{-} < \text{Na}^{+} < \text{Mg}^{2+}$

$\text{Na}^{+} < \text{Mg}^{2+} < \text{F}^{-}$

$\text{Mg}^{2+} < \text{F}^{-} < \text{Na}^{+}$

They are monoatomic, and their non-bonded (van der Waals) radii values are typically very large

They are highly reactive.

Their atomic numbers are too high.

They are located in the $p$-block.

$\text{Mg}$ (Largest parent atom)

$\text{Mg}^{2+}$

$\text{Al}$

$\text{Al}^{3+}$

Decrease in nuclear charge

Increased electron-electron repulsion and decrease in effective nuclear charge

The loss of the valence shell

The electron entering the $n=3$ quantum level

$\text{Rb}$

$\text{K}$

$\text{Cs}$

$\text{Li}$

$\text{Na}$

$\text{Si}$

$\text{Cl}$

$\text{Mg}$

$\text{Ar} < \text{K}^{+} < \text{Ca}^{2+}$

$\text{Ca}^{2+} < \text{K}^{+} < \text{Ar}$

$\text{K}^{+} < \text{Ar} < \text{Ca}^{2+}$

$\text{Ar} < \text{Ca}^{2+} < \text{K}^{+}$