Question

Match the following: List I (Hydridization) 1\. \(\mathrm{sp}^{2}\) 2\. \(\mathrm{sp}^{3}\) 3\. \(\mathrm{sp}\) \(4 .\) List II (Geometry of the molecule) (i) trigonal bipyramidal (ii) planar trigonal (iii) octahedral (iv) tetrahedral (v) linear

Short answer

1.(ii), 2.(iv), 3.(v)

Step-by-step solution

Understanding Hybridization

Hybridization is a concept used to describe the geometry and bonding properties of molecules based on the combination of atomic orbitals. The three primary types of hybridization relevant to this problem are \(\mathrm{sp}^2\), \(\mathrm{sp}^3\), and \(\mathrm{sp}\). Each type predicts a particular molecular geometry driven by the number of hybrid orbitals.

Analyzing \(\mathrm{sp}^2\) Hybridization

Molecules with \(\mathrm{sp}^2\) hybridization typically have three hybridized orbitals. The electron pair arrangement around the central atom is trigonal planar, leading to a geometry described as planar trigonal. Therefore, \(\mathrm{sp}^2\) corresponds to (ii) in List II.

Analyzing \(\mathrm{sp}^3\) Hybridization

The \(\mathrm{sp}^3\) hybridized molecules involve four hybrid orbitals, arranging themselves in a way that minimizes repulsion, resulting in a tetrahedral geometry. Therefore, \(\mathrm{sp}^3\) matches with (iv) in List II.

Analyzing \(\mathrm{sp}\) Hybridization

In \(\mathrm{sp}\) hybridization, two hybrid orbitals are formed, leading the molecule to adopt a linear geometry as atoms arrange in a straight line. Hence, \(\mathrm{sp}\) matches with (v) in List II.

Match Each Item from Lists

After examining each type of hybridization, pair them with their corresponding molecular geometry: 1. \(\mathrm{sp}^2\) - (ii) Planar Trigonal 2. \(\mathrm{sp}^3\) - (iv) Tetrahedral 3. \(\mathrm{sp}\) - (v) Linear.

Key concepts

Molecular Geometry

Molecular geometry refers to the three-dimensional arrangement of atoms in a molecule. Understanding molecular geometry is crucial because it directly influences the physical and chemical properties of a substance. The shape of a molecule is determined by the hybridization of its central atom, which involves combining different types of atomic orbitals to form new hybrid orbitals. The goal of such an arrangement is to minimize repulsion between electron pairs surrounding the central atom, leading to a stable configuration.
For example:

• In a linear geometry, atoms are arranged in a straight line, providing a symmetrical shape that can affect polarity and reactivity.
• A trigonal planar configuration occurs when a central atom is bonded to three other atoms, lying on the same plane. This influences how the molecule interacts with other entities in its environment.
• Tetrahedral geometry, on the other hand, occurs when four bonded atoms situate themselves around a central atom in a three-dimensional space to minimize repulsion, which significantly affects bond angles and molecular interaction.

Overall, recognizing the geometry helps predict how molecules will behave in different chemical contexts.

sp2 Hybridization

In \(sp^{2} \)hybridization, one s orbital mixes with two p orbitals from the same atom to form three equivalent hybrid orbitals. These hybrid orbitals arrange themselves in a trigonal planar formation to minimize electron pair repulsion, providing (120^\circ)bond angles between them.
Let's consider ethylene (\(C_2H_4\)) as a classic example. In ethylene, each carbon atom is \(sp^{2}\)hybridized, forming a flat, planar structure which is essential for creating the double bond between carbon atoms due to the overlapping of \(p_z\)orbitals.
This hybridization is particularly common in molecules where double bonds are present. In the chemistry of organic compounds, \(sp^{2}\)configurations are significant because they contribute to the planarity and rigidity of molecules, which can influence both their chemical reactivity and how they interact with other molecules.

sp3 Hybridization

\(sp^{3}\)hybridization occurs when one s orbital combines with three p orbitals from the same atom to create four equivalent hybrid orbitals. These orbitals arrange in a tetrahedral shape to minimize repulsion between them, with each angle measuring approximately(109.5^\circ).
A classic representation of this hybridization is methane (\(CH_4\)). In methane, the central carbon atom is \(sp^{3}\)hybridized, creating a symmetrical structure that ensures each hydrogen atom is equidistant from the others, reinforcing the molecule’s stability.
This kind of hybridization is predominant in molecules where carbon is bonded exclusively by single bonds, making it critical in the structure of various organic substances. Understanding \(sp^{3}\)hybridization helps define characteristics like flexibility and the ability to undergo rotations around bonds, which extensively impacts the behavior of organic molecules.

sp Hybridization

The simplest form of hybridization, \(sp\)involves the combination of one s orbital and one p orbital, resulting in two linearly arranged hybrid orbitals. These orbitals align at (180^\circ)to each other, lending a linear geometry to molecules.
Take acetylene (\(C_2H_2\)) as an illustrative example. In acetylene, each carbon atom is \(sp\)hybridized, exhibiting a straight-line configuration. This linear shape is crucial for the existence and strength of the triple bond between the carbon atoms.
Moreover, \(sp\)hybridization is prevalent in molecules where triple bonds or molecules with two atoms are involved. These configurations are integral in determining properties such as bond strength and reactivity. Understanding this type of hybridization is essential for studying molecular shapes that are fundamental in different chemical processes.