Chapter 16: Problem 180
The structure of \(\mathrm{XeO}_{3}\) is (a) linear (b) planar (c) pyramidal (d) T-shaped
Short Answer
Expert verified
The structure of XeO₃ is pyramidal.
Step by step solution
01
Identify the central atom and its valence electrons
The molecule is XeO₃, with xenon (Xe) as the central atom. Xe is a noble gas with 8 valence electrons.
02
Determine the number of oxygen atoms bonded to the central atom
XeO₃ has 3 oxygen atoms bonded to the central xenon atom. Each oxygen atom will form a single bond with xenon, using 3 of xenon's valence electrons.
03
Calculate remaining valence electrons as lone pairs
After bonding with 3 oxygen atoms, xenon still has 5 valence electrons to account for. These electrons will form lone pairs. Since each bond uses one electron but two electrons are needed from Xe for bonding to O₂, there are a total of 3 lone pairs remaining.
04
Predict molecular geometry using VSEPR theory
The molecule has 3 bonded pairs and 1 lone pair on the central atom. According to VSEPR (Valence Shell Electron Pair Repulsion) theory, the shape with 3 bonds and 1 lone pair is pyramidal.
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Key Concepts
These are the key concepts you need to understand to accurately answer the question.
VSEPR Theory
The VSEPR (Valence Shell Electron Pair Repulsion) theory is essential for understanding the shape of molecules. It is based on the principle that electron pairs around a central atom will arrange themselves to minimize repulsion. This is because electron pairs repel each other, causing them to spread out as much as possible to achieve a stable structure.
VSEPR theory helps predict the geometry of a molecule based on the number of bonding pairs and lone pairs of electrons surrounding the central atom. The key idea is that different arrangements of electrons lead to different molecular shapes. The theory considers both bonded pairs and lone pairs to determine the overall shape of the molecule.
In the case of \( ext{XeO}_3\), VSEPR theory tells us that the arrangement of three oxygen atoms bonded to the central xenon atom, along with any lone pairs, will define its shape. Understanding how electron pairs interact is crucial for determining molecular geometry. It allows chemists to predict shapes like linear, planar, pyramidal, and others.
VSEPR theory helps predict the geometry of a molecule based on the number of bonding pairs and lone pairs of electrons surrounding the central atom. The key idea is that different arrangements of electrons lead to different molecular shapes. The theory considers both bonded pairs and lone pairs to determine the overall shape of the molecule.
In the case of \( ext{XeO}_3\), VSEPR theory tells us that the arrangement of three oxygen atoms bonded to the central xenon atom, along with any lone pairs, will define its shape. Understanding how electron pairs interact is crucial for determining molecular geometry. It allows chemists to predict shapes like linear, planar, pyramidal, and others.
Valence Electrons
Valence electrons are the outermost electrons of an atom, occupying the highest energy levels. They play a crucial role in bonding because they are the electrons involved in forming chemical bonds.
For xenon, which is found in group 18 of the periodic table, valence electrons are particularly important. Xenon has 8 valence electrons, typical of noble gases, which are generally inert. However, in compounds like \(\mathrm{XeO}_3\), these electrons can participate in bonding.
Valence electrons determine how an atom will interact with other atoms. When forming bonds, an atom will share, gain, or lose electrons to reach a stable configuration similar to the nearest noble gas. For xenon, utilizing its valence electrons means it can form stable compounds despite being a noble gas. Identifying the number of valence electrons is often the first step in predicting how atoms bond and the shapes they form.
For xenon, which is found in group 18 of the periodic table, valence electrons are particularly important. Xenon has 8 valence electrons, typical of noble gases, which are generally inert. However, in compounds like \(\mathrm{XeO}_3\), these electrons can participate in bonding.
Valence electrons determine how an atom will interact with other atoms. When forming bonds, an atom will share, gain, or lose electrons to reach a stable configuration similar to the nearest noble gas. For xenon, utilizing its valence electrons means it can form stable compounds despite being a noble gas. Identifying the number of valence electrons is often the first step in predicting how atoms bond and the shapes they form.
Lone Pairs
Lone pairs denote pairs of valence electrons that are not involved in bonding but still occupy space around the central atom. These pairs influence the shape and properties of a molecule by occupying regions of space and exerting repulsion forces.
In \(\mathrm{XeO}_3\), xenon forms bonds with three oxygen atoms using its valence electrons. After forming these bonds, xenon still possesses electrons that are not used in bonding, leaving three lone pairs. These also need to be arranged around the xenon to minimize repulsion, which influences the molecule's structure.
Lone pairs are significant because they take up more space than bonding pairs. They can also have a profound effect on the molecular geometry by causing bond angles to adjust. For example, the presence of one lone pair on xenon in \(\mathrm{XeO}_3\) results in a pyramidal shape, as they repel the bonding pairs to modify the overall geometry.
In \(\mathrm{XeO}_3\), xenon forms bonds with three oxygen atoms using its valence electrons. After forming these bonds, xenon still possesses electrons that are not used in bonding, leaving three lone pairs. These also need to be arranged around the xenon to minimize repulsion, which influences the molecule's structure.
Lone pairs are significant because they take up more space than bonding pairs. They can also have a profound effect on the molecular geometry by causing bond angles to adjust. For example, the presence of one lone pair on xenon in \(\mathrm{XeO}_3\) results in a pyramidal shape, as they repel the bonding pairs to modify the overall geometry.
Bonding in Xenon Compounds
Bonding in xenon compounds, like \(\mathrm{XeO}_3\), is fascinating because it challenges the general behavior expected from noble gases. Typically, noble gases like xenon are chemically inert because they have a complete set of valence electrons. However, under certain conditions, xenon can form compounds by sharing its valence electrons.
In \(\mathrm{XeO}_3\), xenon forms three sigma bonds with oxygen atoms. Each oxygen atom receives two electrons from xenon, which allows them to fill their outer shell. Xenon's ability to form such bonds is attributed to the availability of empty \(d\) orbitals that can participate in bonding. This expands xenon's bonding capability beyond the typical limitations of noble gases.
Understanding xenon bonds requires considering the atomic structure and electron configuration, which venture beyond simple octet rules. Xenon's versatility in bonding is linked to its ability to mix available orbitals to accommodate additional electrons and achieve diverse molecular geometries.
In \(\mathrm{XeO}_3\), xenon forms three sigma bonds with oxygen atoms. Each oxygen atom receives two electrons from xenon, which allows them to fill their outer shell. Xenon's ability to form such bonds is attributed to the availability of empty \(d\) orbitals that can participate in bonding. This expands xenon's bonding capability beyond the typical limitations of noble gases.
Understanding xenon bonds requires considering the atomic structure and electron configuration, which venture beyond simple octet rules. Xenon's versatility in bonding is linked to its ability to mix available orbitals to accommodate additional electrons and achieve diverse molecular geometries.
