Question

Which of the following is a correct pair with respect to molecular formula of a xenon compound and the hybridization state of xenon in it? (a) \(\mathrm{XeF}_{2}, \mathrm{sp}\) (b) \(\mathrm{XeF}_{4}, \mathrm{sp}^{2}\) (c) \(\mathrm{XeF}_{4}, \mathrm{sp}^{3}\) (d) \(\mathrm{XeF}_{2}, \mathrm{sp}^{3} \mathrm{~d}\)

Short answer

Option (d): \( \mathrm{XeF}_{2}, \mathrm{sp}^3\mathrm{d} \) is correct.

Step-by-step solution

Identify the Molecular Formula

We need to examine each option to identify the molecular formula of the xenon compound and compare it with the hybridization state provided. Let's start with the formula and its corresponding structure.

Analyze the XeF2 Molecule

- \(\mathrm{XeF}_{2}\) has a linear structure.- The hybridization state of xenon in \(\mathrm{XeF}_2\) is \(\mathrm{sp}^{3}\mathrm{d}\), forming a linear shape with 3 lone pairs and 2 bond pairs.

Evaluate the XeF4 Molecule Options

- \(\mathrm{XeF}_{4}\) requires analysis as well.- It has a square planar geometry, and the hybridization state of xenon is \(\mathrm{sp}^{3}\mathrm{d}^{2}\), with 2 lone pairs and 4 bond pairs.

Check Each Given Option

Compare the correct hybridization states with the options.- Option (a) \(\mathrm{XeF}_{2}, \mathrm{sp}\)- Option (b) \(\mathrm{XeF}_{4}, \mathrm{sp}^{2}\)- Option (c) \(\mathrm{XeF}_{4}, \mathrm{sp}^{3}\)- Option (d) \(\mathrm{XeF}_{2}, \mathrm{sp}^{3}\mathrm{d}\) Only option (d) correctly pairs the molecular formula with the hybridization state.

Key concepts

Hybridization

Hybridization is a key concept in understanding how different elements form chemical bonds in molecules. It's a model that describes the mixing of atomic orbitals to create equivalent hybrid orbitals, which can then form bonds to other atoms. In the case of xenon compounds, we often look at xenon fluoride structures, like \( \text{XeF}_2 \) and \( \text{XeF}_4 \).

For example, in \( \text{XeF}_2 \), xenon undergoes \( \text{sp}^3\text{d} \) hybridization. This involves the mixing of one \( s \), three \( p \), and one \( d \) orbital to create five hybrid orbitals. This hybridization allows xenon to form bonds with two fluorine atoms and accommodate three lone pairs, resulting in a linear structure.

Meanwhile, \( \text{XeF}_4 \) uses \( \text{sp}^3\text{d}^2 \) hybridization. In this case, xenon's one \( s \), three \( p \), and two \( d \) orbitals combine to allow bonding with four fluorine atoms and holding two lone pairs, giving a square planar shape. Understanding these hybridizations is crucial for predicting the molecular shapes and properties of xenon compounds.

Molecular Geometry

Molecular geometry focuses on the 3-dimensional arrangement of atoms within a molecule. It's significant because the shape of a molecule greatly influences its properties and reactivity. In xenon compounds like \( \text{XeF}_2 \) and \( \text{XeF}_4 \), molecular geometry is determined by both bonding and lone pairs of electrons.

For \( \text{XeF}_2 \), the geometry is linear due to the arrangement of three lone pairs and two bonded pairs around xenon. The electron repulsion theory explains this linear shape, with the 180-degree bond angle minimizing electronic repulsions.

On the other hand, \( \text{XeF}_4 \) presents a square planar geometry. The logical arrangement of four bonded pairs and two lone pairs around xenon allows for a symmetric distribution, resulting in 90-degree angles in the plane of the molecule. Such shapes are easier to predict through understanding hybridization and electron arrangements, making molecular geometry a useful tool in chemical structure analysis.

Chemical Structure Analysis

Chemical structure analysis is the study of how atoms are connected in a molecule and their spatial configuration. It's essential for identifying molecular features that affect behavior and interactions. In analyzing xenon compounds like \( \text{XeF}_2 \) and \( \text{XeF}_4 \), consideration of electron pairs (both bonded and lone) helps to elucidate their structure.

In \( \text{XeF}_2 \), chemical structure determination reveals that its linear form is due to the positioning of lone pairs, which shield each other and the bonded pairs effectively. This shielding is fundamental in maintaining a stable molecular configuration.

In \( \text{XeF}_4 \), the configuration analysis shows a square planar shape where the four fluorine atoms form a symmetric square around xenon. The lone pairs are positioned opposite each other above and below the plane, preventing any distortion in the structure and thereby affecting how the molecule interacts with other substances.

Understanding chemical structures is crucial in fields like material science and pharmaceuticals, where molecular interactions dictate functionality and efficacy.