Question

An element having the electronic configuration of its atom as \(\mathrm{ns}^{2} \mathrm{n} \mathrm{p}^{2}\) should have similar properties to those of (1) Sodium (2) Carbon (3) Magnesium (4) Oxygen

Short answer

Carbon

Step-by-step solution

Understand the Electronic Configuration

The given electronic configuration is \(s^{2} np^{2} \). This indicates that the element has two electrons in the s-orbital and two electrons in the p-orbital of the outermost shell.

Determine Group Classification

Elements with the electronic configuration of \(ns^{2} np^{2}\) belong to Group 14 of the periodic table, as they have four electrons in their outermost shell (2 from ns and 2 from np).

Identify Similar Element

Among the given options, Carbon is the element in Group 14 with an electronic configuration \(2s^{2} 2p^{2}\). Thus, an element with \(ns^{2} np^{2}\) configuration is similar to Carbon.

Key concepts

Group 14 Elements

Group 14 elements are also known as the carbon family. These elements include Carbon (C), Silicon (Si), Germanium (Ge), Tin (Sn), and Lead (Pb). They all share the same characteristic electronic configuration in their outermost shell, specifically \(ns^{2} np^{2}\).
This group exhibits a range of metallic to non-metallic properties, with carbon being a non-metal, silicon and germanium being metalloids, and tin and lead being metals.
The elements in this group have four electrons in their valence shell, which significantly affects their chemical behavior.
Understanding these elements is key to grasping their role in various chemical reactions and their wide range of applications, from organic chemistry to materials science.

Electronic Configuration

Electronic configuration describes the distribution of electrons in an atom's orbitals. For Group 14 elements, the configuration is \(ns^{2} np^{2}\). Here, 'n' represents the principal quantum number, which correlates with the period of the element on the periodic table.
The notation \(ns^{2} np^{2}\) indicates two electrons occupying the s orbital and two electrons occupying the p orbital of the outermost shell. This particular arrangement explains why Group 14 elements have similar chemical properties.
By knowing the electronic configuration, we can predict the reactivity of elements, their possible oxidation states, and their behavior in chemical bonding.
For instance, carbon with its \(2s^{2} 2p^{2}\) configuration is highly versatile and can form various compounds, ranging from simple hydrocarbons to complex biomolecules.

Chemical Properties Similarity

The chemical properties of elements are largely determined by the number and arrangement of electrons in their outermost shell. For Group 14 elements, the \(ns^{2} np^{2}\) configuration results in them sharing several similar properties:
They tend to form covalent bonds by sharing their four valence electrons.

• Carbon can form stable bonds with many elements, leading to an immense variety of organic compounds, including the basis of all known life.
• Silicon is crucial in the semiconductor industry, forming the backbone of electronic devices.

Their ability to form multiple oxidation states enables them to participate in a wide range of chemical reactions.
For instance, carbon can exhibit oxidation states from \(-4\) in methane (CH₄) to \(+4\) in carbon dioxide (CO₂), making it incredibly versatile.
Understanding the similar properties of Group 14 elements opens up insights into their reactivity patterns and applications in various fields, from organic chemistry to materials science.