Textbook Question
Chlorine reacts with molten sulfur to yield disulfur dichloride, a yellowish-red liquid. Propose a structure for disulfur dichloride.
Ch.22 - The Main Group Elements
Chapter 22, Problem 159
What is the electron-dot structure and geometry of XeO3?
Verified step by step guidance1
Step 1: Determine the total number of valence electrons available. Xenon (Xe) has 8 valence electrons, and each oxygen (O) has 6 valence electrons. Since there are three oxygen atoms, the total number of valence electrons is 8 + (3 * 6).
Step 2: Draw the skeletal structure of the molecule. Place the xenon (Xe) atom in the center and connect it to the three oxygen (O) atoms with single bonds.
Step 3: Distribute the remaining valence electrons to satisfy the octet rule for each oxygen atom. Start by placing lone pairs on the oxygen atoms until each has 8 electrons (including the bonding electrons).
Step 4: Check if the central xenon atom has a complete octet. If not, consider forming double bonds between xenon and oxygen atoms to ensure that xenon also satisfies the octet rule.
Step 5: Determine the molecular geometry using VSEPR theory. Count the number of bonding pairs and lone pairs around the central xenon atom to predict the shape of the molecule. XeO3 has three bonding pairs and one lone pair, leading to a trigonal pyramidal geometry.
Key Concepts
Here are the essential concepts you must grasp in order to answer the question correctly.
Electron-Dot Structure
The electron-dot structure, also known as the Lewis structure, represents the valence electrons of atoms within a molecule. It uses dots to depict the electrons and lines to indicate bonds between atoms. For XeO3, the structure helps visualize how xenon and oxygen atoms are bonded and the distribution of lone pairs, which is crucial for understanding molecular geometry.
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Molecular Geometry
Molecular geometry refers to the three-dimensional arrangement of atoms in a molecule. It is determined by the number of bonding pairs and lone pairs of electrons around the central atom, following the VSEPR (Valence Shell Electron Pair Repulsion) theory. For XeO3, the geometry can be predicted based on the arrangement of the bonded oxygen atoms and the lone pairs on xenon.
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VSEPR Theory
VSEPR theory is a model used to predict the shape of molecules based on the repulsion between electron pairs. According to this theory, electron pairs will arrange themselves to minimize repulsion, leading to specific geometries. In the case of XeO3, VSEPR theory helps determine that the molecule adopts a trigonal pyramidal shape due to the presence of lone pairs on the xenon atom.
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