Question

The element that has the least tendency to show the inert-pair effect is (a) Bi (b) \(\bar{P}\) (c) \(\mathrm{Sb}\) (d) \(\mathrm{N}\)

Short answer

Nitrogen ( N ) has the least tendency to show the inert-pair effect.

Step-by-step solution

Understand the Inert-Pair Effect

The inert-pair effect refers to the tendency of the ns^2 electrons in the outermost electron shell to remain non-bonding or inert as you move down a group in the periodic table. This typically affects heavier p-block elements.

Analyze the Elements

We have the elements Bismuth (Bi), Phosphorus ( P ), Antimony ( Sb ), and Nitrogen ( N ). These elements are in Group 15 of the periodic table. We need to compare their tendency to exhibit the inert-pair effect.

Consider the Position in the Periodic Table

As you move down the group from N to Bi , the tendency to exhibit the inert-pair effect generally increases due to increased atomic size and electron shielding. Consequently, elements higher up in the group tend to have a lesser tendency to display the inert-pair effect.

Identify the Element

Since Nitrogen ( N ) is the highest in the group among the options, it has the least fullness of the inert-pair effect. The effect is more pronounced in heavier elements like Bismuth.

Key concepts

p-block elements

The p-block elements are a fascinating group of elements found on the right side of the periodic table. They encompass a wide range of elements from various groups, specifically Groups 13 to 18. This diversity is reflected in their properties and applications. These elements include non-metals, metalloids, and metals.
One interesting feature of p-block elements is their electron configuration, which terminates in the p shell. This means their outermost electron configuration can end in one to six p electrons, leading to intricate chemical behavior and bonding capabilities.

• Metalloids, like Silicon, exhibit properties that are intermediate between metals and non-metals.
• The non-metals, such as Nitrogen (N) and Oxygen (O), are essential for life and exist as gases in their elemental forms.

Overall, the p-block elements are crucial for various biological, chemical, and industrial processes.

periodic table

The periodic table is an iconic representation of chemical elements arranged in an array by atomic number, electron configuration, and recurring chemical properties. Each element on the table sits in a specific place, reflecting its atomic structure and properties.
The table is structured in rows called periods and columns referred to as groups or families. Each of these groups has elements with similar properties. For example, Group 15 where Nitrogen (N), Phosphorus (P), and Bismuth (Bi) reside, is known for elements having five electrons in their outermost p orbitals, hence tending to form triple bonds or oxidation states of +3 and +5.

• Periods represent the number of electron shells an element possesses.
• Groups have elements with the same number of electrons in their outer shell, indicating similar chemical behavior.

This arrangement allows us to predict the chemical reactions the element might undergo, as well as its likely electron gain or loss tendencies.

electron configuration

Electron configuration is like the blueprint of an element's electrons around the nucleus. The way these electrons are arranged determines the element's chemical properties and reactivity. The electrons fill up various shells or energy levels defined by quantum mechanics, indicated by the principal quantum number, followed by the type of orbital (s, p, d, f) they inhabit.
In the case of p-block elements, their outermost electrons enter the p orbitals. Therefore, the group number in the periodic table often gives insight into the number of electrons present in these p orbitals. For example, elements in Group 15 typically have an outer electron configuration ending in ns²np³.

• The electrons follow the Pauli Exclusion Principle and Hund's Rule as they occupy orbitals.
• This filling order leads to distinct electron configuration patterns that provide insight into bonding and chemical properties.

Understanding electron configuration is fundamental to grasping why certain elements exhibit specific reactions, such as why Nitrogen has limited participation in the inert-pair effect compared to Bismuth.

elemental properties

Elemental properties are the inherent characteristics that dictate how an element behaves chemically and physically. These properties are derived from the element's atomic structure and electron configuration. Among these properties, atomic size and electron affinity are particularly important.
As we move down a group in the periodic table, atomic size increases. This happens due to the addition of electron shells. Elements lower in a group, like Bismuth, have larger atomic radii compared to those higher up, such as Nitrogen. This increase in size and electron shielding in heavier elements leads to phenomena like the inert-pair effect.
Moreover, electron affinity and electronegativity tend to decrease down the group, affecting how elements bond with others. For instance, Nitrogen is more electronegative than Bismuth and engages differently in chemical reactions. These properties help understand why Bi might exhibit more pronounced inert-pair effect than N due to its electron configuration and size.