Problem 28 - A Complete Resource Book in Chemistry for JEE Main

Question

The electronic configuration of group III elements is (a) \(\mathrm{ns}^{1} \mathrm{np}^{2}\) (b) \(\mathrm{ns}^{1} \mathrm{np}^{3}\) (c) \(\mathrm{ns}^{2} \mathrm{np}^{1}\) (d) \(\mathrm{ns}^{2} \mathrm{np}^{2}\)

Step-by-Step Solution

Answer

The correct electronic configuration of group III elements is (c) \(\mathrm{ns}^{2} \mathrm{np}^{1}\).

Step 1: Understanding the question

We are asked to find the electronic configuration of group III elements. Group III elements in the periodic table are typically associated with the boron family.

Step 2: Analyzing Group III Electronic Configuration

The group III elements, also known as the boron group, start with Boron (B) and continue with Aluminum (Al), Gallium (Ga), Indium (In), and Thallium (Tl). All these elements have one electron in the p orbital in their outermost shell. This leads to an electronic configuration pattern of \(s^{2}np^{1}\).

Step 3: Choosing the correct option

Now we compare the given options with the established electronic configuration pattern for group III elements, which is \(s^{2}np^{1}\). The correct answer matches option (c) \(s^{2} p^{1}\).

Key Concepts

Group III Elements

The term "group III elements" refers to a specific set of elements found in the periodic table. These elements are located in the same column, which indicates that they share similar properties.
The group is known as the "boron group," and it includes the elements Boron (B), Aluminum (Al), Gallium (Ga), Indium (In), and Thallium (Tl).
These elements are characterized by having three electrons in their outermost shell, with a typical electronic configuration of \( ext{ns}^2 ext{np}^1 \).

• Boron is the first element in this group and is a non-metal.
• The other elements, like Aluminum and Indium, are metals.

These elements have an important role in chemistry due to their unique properties and widespread applications, ranging from fuel catalysts with Boron to the ubiquitous use of Aluminum in consumer products.

Boron Group

The boron group is a fascinating collection of elements within the periodic table. This group consists of five elements, all sharing similar properties due to their group positioning.

• Boron, the first member, is a metalloid, demonstrating properties of both metals and non-metals.
• Aluminum is the next in line, and it is widely known for its lightweight and strength, making it useful in packaging and construction.
• Gallium can melt easily and is often used in electronics and semiconductors.

Across this group, these elements demonstrate a gradual transition from non-metallic to metallic properties as you move down the periodic table. This trend is particularly interesting in the study of chemical behaviors and compound formation.

Periodic Table

The periodic table is a fundamental tool in chemistry that organizes all known elements into a systematic layout. It is organized by increasing atomic number and groups elements with similar properties together.

• Groups are the vertical columns, and they indicate elements with similar valence electron configurations.
• The names of groups provide valuable information about their chemical behavior.

The periodic table not only helps predict the properties and reactivity of the elements, but also makes understanding and memorizing them more structured. For anyone studying chemistry, mastering the periodic table is essential for navigating and linking the vast information it contains.

P Orbital

The p orbital is one of the major types of atomic orbitals within an atom, responsible for the shape and distribution of electrons.

• In the context of the electronic configuration, p orbitals can hold a maximum of six electrons, divided across three sub-orbitals.
• In the case of group III elements, there is typically one electron in the p orbital, giving rise to the configuration \( ext{ns}^2 ext{np}^1 \).

P orbitals have a dumbbell shape, with three orientations in space (px, py, pz), that allow them to form covalent chemical bonds.
This understanding is crucial when predicting how an element within a specific group will react in various chemical environments.