Problem 184 - A Complete Resource Book in Chemistry for JEE Main

Question

Match the following Match the following Column-I (a) \(\mathrm{XeF}_{2}\) (b) \(\mathrm{XeF}_{4}\) (c) \(\mathrm{XeF}_{6}\) (d) \(\mathrm{XeOF}_{4}\) Column-II (p) One lone pair electron on Xe-atom (q) \(\mathrm{sp}^{3} \mathrm{~d}\) (r) \(\mathrm{sp}^{3} \mathrm{~d}^{2}\) (s) \(\mathrm{sp}^{3} \mathrm{~d}^{3}\) (t) \(+6\) oxidation state of xenon

Step-by-Step Solution

Answer

(a) matches (q); (b) matches (r); (c) matches (s); (d) matches (r) and (t).

Step 1: Analyze XeF2 Geometry

XeF2 has a linear geometry with the formula structure of AX2E3, which means there are 2 bonded pairs and 3 lone pairs of electrons. This corresponds to the following matches: XeF2 is sp3d hybridized and has 3 lone pairs.

Step 2: Analyze XeF4 Geometry

XeF4 has a square planar geometry with the formula structure of AX4E2, meaning it has 4 bonded pairs and 2 lone pairs. This corresponds to the following matches: XeF4 is sp3d2 hybridized and has 2 lone pairs.

Step 3: Analyze XeF6 Geometry

XeF6 has a distorted octahedral geometry with the formula structure of AX6E1, which means it has 6 bonded pairs and 1 lone pair. This corresponds to the following matches: XeF6 is sp3d3 hybridized and has 1 lone pair.

Step 4: Analyze XeOF4 Geometry and Oxidation State

XeOF4 has a square pyramidal geometry with the hybridization of sp3d2, indicated by 1 double bond with oxygen and 4 single bonds with fluorine atoms, leaving one lone pair. Also, the oxidation state of xenon in XeOF4 is +6.

Key Concepts

Chemical Bonding

Chemical bonding is the interaction that holds atoms together in molecules. In xenon fluoride compounds, xenon forms bonds with fluorine atoms. Xenon, a noble gas, has the ability to form stable compounds under specific conditions. It is not typical for noble gases to form bonds due to their full electron shells. However, xenon can do so because it has empty d-orbitals that can be utilized for bonding.

• Xenon and fluorine form covalent bonds in these compounds.
• Fluorine, being highly electronegative, strongly attracts electrons from xenon, leading to the formation of polar bonds.

Understanding chemical bonding in xenon fluorides helps explain how this normally inert element can create stable compounds.

Molecular Geometry

Molecular geometry is the three-dimensional arrangement of atoms in a molecule. For xenon fluoride compounds, the geometry varies according to the number of atoms bonded and lone pairs present.

• In \( \mathrm{XeF}_2 \), the geometry is linear with two bonded pairs and three lone pairs.
• \( \mathrm{XeF}_4 \) forms a square planar shape, with four bonded pairs and two lone pairs causing this arrangement.
• \( \mathrm{XeF}_6 \) features a distorted octahedral geometry, mainly due to six bonds and one lone pair.
• \( \mathrm{XeOF}_4 \) adopts a square pyramidal structure due to four bonds with fluorines and one bond with oxygen.

Each of these geometries arises from the need to minimize electron pair repulsions, according to VSEPR theory.

Hybridization

Hybridization is the concept explaining how atomic orbitals mix to form new hybrid orbitals, which accommodate the bonded electrons. In xenon fluoride compounds, hybridization allows xenon to form multiple bonds despite its full outer shell.

• In \( \mathrm{XeF}_2 \), hybridization of xenon's orbitals results in \( \mathrm{sp}^{3}d \), accounting for the linear arrangement.
• For \( \mathrm{XeF}_4 \), \( \mathrm{sp}^{3}d^2 \) hybridization explains its square planar shape.
• \( \mathrm{XeF}_6 \) involves \( \mathrm{sp}^{3}d^3 \) hybridization, which facilitates a distorted octahedral structure.
• The \( \mathrm{XeOF}_4 \) uses \( \mathrm{sp}^{3}d^2 \) hybridization, resulting in a square pyramidal form.

Hybridization provides insight into how electrons are distributed among atomic orbitals to form stable bonding arrangements.

Oxidation States of Xenon

Oxidation states denote the degree of oxidation of an atom, representing the number of electrons lost or gained. Xenon typically showcases a range of oxidation states in its compounds, contributing to its versatile chemistry.

• The oxidation state of xenon in \( \mathrm{XeF}_2 \), \( \mathrm{XeF}_4 \), and \( \mathrm{XeF}_6 \) is generally +2, +4, and +6, respectively.
• In \( \mathrm{XeOF}_4 \), xenon reaches its highest oxidation state of +6. This is due to bonding with more electronegative atoms like fluorine and oxygen.

Understanding oxidation states helps predict bonding patterns and reactivity of xenon compounds.