Question

The xenon halides and oxides are isoelectronic with many other compounds and ions containing halogens. Give a molecule or ion in which iodine is the central atom that is isoelectronic with each of the following. \(\begin{array}{ll}{\text { a. xenon tetroxide }} & {\text { d. xenon tetrafluoride }} \\ {\text { b. xenon trioxide }} & {\text { e. xenon hexafluoride }} \\ {\text {c. xenon difluoride}}\end{array}\)

Short answer

The iodine-containing species isoelectronic with the given xenon compounds are: a. \(\text{IO}_4^-\). b. \(\text{IO}_3^-\). c. \(\text{IF}_2^+\). d. \(\text{IF}_4^+\). e. \(\text{IF}_6^+\).

Step-by-step solution

Determine the total number of electrons in the given xenon compounds

The known xenon compounds are given below, and their corresponding total electrons are calculated. a. Xenon tetroxide (XeO4): Xe(54 electrons) + 4 * O(8 electrons each) = 54 + 4 * 8 = 86 electrons. b. Xenon trioxide (XeO3): Xe(54 electrons) + 3 * O(8 electrons each) = 54 + 3 * 8 = 78 electrons. c. Xenon difluoride (XeF2): Xe(54 electrons) + 2 * F(9 electrons each) = 54 + 2 * 9 = 72 electrons. d. Xenon tetrafluoride (XeF4): Xe(54 electrons) + 4 * F(9 electrons each) = 54 + 4 * 9 = 90 electrons. e. Xenon hexafluoride (XeF6): Xe(54 electrons) + 6 * F(9 electrons each) = 54 + 6 * 9 = 108 electrons.

Find iodine compounds with the same total electrons

To find isoelectronic iodine compounds, we will identify the species with the required number of electrons by adjusting the number and type of ligands (atoms surrounding iodine). a. For 86 electrons, we need iodine (53 electrons) plus an additional 33 electrons from ligands. Four oxygen atoms can provide this (4 * 8 = 32 electrons), and we have a negative charge: \(\text{IO}_4^-\). b. For 78 electrons, we need iodine (53 electrons) plus an additional 25 electrons from ligands. Three oxygen atoms can provide this (3 * 8 = 24 electrons), and additionally we have a negative charge: \(\text{IO}_3^-\). c. For 72 electrons, we need iodine (53 electrons) plus an additional 19 electrons from ligands. Two fluorine atoms can provide this (2 * 9 = 18 electrons), and additionally we have a positive charge: \(\text{IF}_2^+\). d. For 90 electrons, we need iodine (53 electrons) plus an additional 37 electrons from ligands. Four fluorine atoms can provide this (4 * 9 = 36 electrons), and we have a positive charge: \(\text{IF}_4^+\). e. For 108 electrons, we need iodine (53 electrons) plus an additional 55 electrons from ligands. Six fluorine atoms can provide this (6 * 9 = 54 electrons), and we have a positive charge: \(\text{IF}_6^+\).

Write down the isoelectronic iodine-containing species

The iodine-containing species isoelectronic with the given xenon compounds are as follows: a. \(\text{IO}_4^-\). b. \(\text{IO}_3^-\). c. \(\text{IF}_2^+\). d. \(\text{IF}_4^+\). e. \(\text{IF}_6^+\).

Key concepts

Xenon Compounds

Xenon, a member of the noble gases, forms fascinating compounds despite its inert nature. These include various halides and oxides. Prime examples of xenon compounds include xenon tetroxide (XeO₄), xenon trioxide (XeO₃), and xenon difluoride (XeF₂).
Xeno xenon compounds are interesting as they deviate from the typical inertness of noble gases due to xenon's ability to form stable bonds with highly electronegative elements like oxygen and fluorine.
Understanding these compounds is crucial as they serve as benchmarks for exploring similar structures containing other central atoms, such as iodine, in the quest for isoelectronic counterparts.

Valence Electrons

Valence electrons are pivotal in determining how an atom bonds with others. For xenon, its valence electrons are responsible for the formation of its stable compounds despite being a noble gas.
In xenon compounds, xenon contributes 54 electrons while ligands, like oxygen or fluorine, contribute additional electrons. For example:

• Xenon tetroxide (XeO₄) has 86 electrons in total - which includes xenon's electrons and those from four oxygen atoms.
• Xenon hexafluoride (XeF₆) contains a whopping 108 total electrons, thanks to the contributions from six fluorine atoms.

Recognizing these electrons helps in deducing isoelectronic species, which share the same total number of electrons, and are useful in comparing molecular properties.

Halides and Oxides

The xenon halides (such as XeF₂, XeF₄, and XeF₆) and oxides (such as XeO₃ and XeO₄) showcase the versatility of xenon in forming compounds. Each type of compound involves different non-metal elements bonding with xenon, which is rare for noble gases.
Halides like XeF₂ involve xenon sharing electrons with fluorine, a highly electronegative element. Oxides like XeO₄ involve bonds with oxygen that strongly stabilize the compound.

• These halides and oxides are comparably stable due to the electronegative elements involved.
• In forming these molecules, xenon departs from its usual non-reactive self, showing its potential to form numerous isoelectronic species with other elements, such as iodine.

This comparison highlights how iodine can form similar compounds, often leading us to understand advances in chemical bonding and molecular stability.

Molecular Structure

The molecular structure of xenon compounds provides insights into the geometric and electronic arrangement of atoms within a molecule. The spatial arrangement of atoms, particularly in complex molecules, impacts their chemical properties.
Xenon halides like XeF₄ have a square planar structure due to the hybridization of xenon's orbitals. The linear structure of XeF₂ displays the influence of fluorine's electronegativity tightly binding the electrons.
The various structures are determined by the central xenon atom, and influence is enhanced by the surrounding electronegative ligands. Moreover:

• In terms of electron pairs, xenon tetroxide (XeO₄) is structured tetrahedrally, giving it a symmetrical geometric configuration.
• Understanding these structures, including those like IF₄⁺ isoelectronic to XeF₄, aids in predicting behavior and properties for advanced chemical studies.

Overall, these structures play a pivotal role in chemical bonding theories and molecular geometry understanding, offering a window into the nature of other complex compounds.