Question

Two elements \(\Lambda\) and \(\mathrm{B}\) of carbon family have very close atomic radii. The clements \(\Lambda\) and \(B\) arc (1) \(\mathrm{Pb}\) and \(\mathrm{Sn}\) (2) \(\mathrm{C}\) and \(\mathrm{Si}\) (3) Ge and Sn (4) \(\mathrm{Si}\) and \(\mathrm{Gc}\)

Short answer

Si and Ge (Option 4)

Step-by-step solution

Identify the Carbon Family Elements

The carbon family elements belong to Group 14 of the periodic table. These elements include Carbon (C), Silicon (Si), Germanium (Ge), Tin (Sn), and Lead (Pb).

Consider Atomic Radii Trends

Within a group in the periodic table, the atomic radius increases as you move down the group. This increase happens because additional electron shells are being added.

Compare Given Options

Now, compare the atomic radii of the given pairs:- (1) Pb and Sn: These elements are at the bottom of the group, so they have larger atomic radii compared to other elements in the group.- (2) C and Si: These elements are at the top of the group, with smaller atomic radii compared to other elements.- (3) Ge and Sn: These two elements are positioned close to each other on the periodic table, between Si and Pb.- (4) Si and Ge: These elements are adjacent in the periodic table, just below Carbon and above Tin.

Select Elements with Closest Atomic Radii

From the analysis, we can infer that pairs (3) Ge and Sn, and (4) Si and Ge have relatively close atomic radii. Since Si and Ge are directly adjacent, they will have the closest atomic radii.

Key concepts

Carbon family elements

The Carbon family, also known as Group 14 elements, is a fascinating set of elements in the periodic table. These elements include Carbon (C), Silicon (Si), Germanium (Ge), Tin (Sn), and Lead (Pb). Each of these elements plays a crucial role in both natural and industrial processes. This family is unique due to their varied properties that change gradually across the group.

For instance, carbon is a nonmetal, silicon and germanium are metalloids, while tin and lead are metals. This variation results in a wide range of bonding types and chemical behaviors. Understanding the atomic radii of these elements helps us comprehend how these properties change, aiding in predicting their reactivity and compatibility in different reactions.

Group 14 elements

Group 14 elements, which belong to the p-block of the periodic table, share some common traits yet exhibit distinct differences due to their atomic size and electronic configuration. These elements have four electrons in their outermost shell, leading to a common oxidation state of +4. However, as you move down the group from Carbon to Lead, atomic size and metallic behavior increase.

Silicon (Si), Germanium (Ge), Tin (Sn), and Lead (Pb) display an trend towards metallic properties, with Lead being the most metallic. Germanium and Silicon, however, are known for their semiconductor properties, making them invaluable in electronics. The ability to compare their atomic radii gives insight into their bonding capabilities and placements in various chemical environments.

Periodic table trends

The periodic table is a powerful tool for understanding the properties and behaviors of elements. One essential trend is the atomic radius trend. Within a group like Group 14, the atomic radius increases as you move down the group. This is because each successive element adds a shell of electrons, making the atoms larger overall.

This trend helps us predict not only the size of atoms but also their reactivity and other chemical properties. Elements like Si and Ge, being adjacent to each other, have very similar atomic radii, making them closely comparable. This similarity often means they can substitute for one another in various chemical compounds, which is vital in fields like material science and chemistry.