The correct order of stability is (a) SnF2>PbF2>GeF2 (b) GeF2>SnF2>PbF2^2 (c) GeF2>PbF2^2>SnF2 (

step 1 The stability of fluorides increases as the size of central atom of central atom increases. So c

The correct order of stability is (a) SnF2>PbF2>GeF2 (b)...

The correct order of stability is
(a) $\mathrm{SnF}_{2}>\mathrm{PbF}_{2}>\mathrm{GeF}_{2}$
(b) $\mathrm{GeF}_{2}>\mathrm{SnF}_{2}>\mathrm{PbF}_{2}^{2}$
(c) $\mathrm{GeF}_{2}>\mathrm{PbF}_{2}^{2}>\mathrm{SnF}_{2}$
(d) $\mathrm{PbF}_{2}>\mathrm{SnF}_{2}>\mathrm{GeF}_{2}$

Key Concepts

Periodic Trends

Periodic trends refer to the recurring patterns observed in the properties of elements, such as atomic radius, ionization energy, and electronegativity, as one moves across or down the periodic table. These trends influence the behavior of elements in chemical compounds, including how they bond with other atoms and the stability of the compounds they form.

Inert Pair Effect

The inert pair effect is the tendency of the s-electrons in the outermost electron shell of heavy p-block elements to remain non-bonding or inert in chemical reactions, leading to lower oxidation states than might be expected. This effect significantly influences the stability of compounds formed by these elements, particularly in cases where multiple oxidation states are possible.

Oxidation States and Compound Stability

The oxidation state of an element in a compound determines the number of electrons lost, gained, or shared during bonding, which in turn affects the compound’s overall stability. For main group elements, especially those in the heavier part of the group, lower oxidation states can be favored due to factors like the inert pair effect, which stabilizes compounds that might otherwise be less common.

Bonding and Lattice/Energy Considerations

Bond strength and lattice energy play crucial roles in determining the stability of compounds. In ionic compounds, the lattice energy, which arises from the electrostatic interactions between charged ions, can greatly influence the stability. For covalent compounds, bond energies and the effectiveness of orbital overlap impact how strongly atoms are held together, thereby affecting the compound's persistence under various conditions.

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