Fill in the blank spaces in the following chart. If the molecule column is blank, find an example that fulfills the conditions of the rest of the row. Molecule Electron-Domain Hybridization Dipole Geometry of Central Atom Moment? Yes or No CO2 sp3 Yes sp3 No Trigonal planar No SF4 Octahedral No sp2 Yes Trigonal bipyramidal No XeF2 Complete the first row of the table.

Verified step by step guidance

1. Identify the missing information in the first row of the table: the molecule and the geometry of the central atom.
2. The given electron-domain hybridization is \( \text{sp}^3 \), which typically corresponds to a tetrahedral geometry.
3. The dipole moment is 'Yes', indicating that the molecule is polar.
4. A common molecule with \( \text{sp}^3 \) hybridization and a polar nature is \( \text{CH}_3\text{Cl} \) (chloromethane).
5. Thus, the first row can be completed with the molecule \( \text{CH}_3\text{Cl} \) and the geometry of the central atom as tetrahedral.

Key Concepts

Electron-Domain Hybridization

Electron-domain hybridization is the process by which atomic orbitals mix to form new hybrid orbitals that can accommodate the electron pairs around a central atom. The type of hybridization (e.g., sp, sp2, sp3) depends on the number of electron domains, which include bonding pairs and lone pairs. Understanding this concept is crucial for predicting molecular geometry and the arrangement of atoms in a molecule.

Molecular Geometry

Molecular geometry refers to the three-dimensional arrangement of atoms in a molecule, which is determined by the repulsion between electron pairs surrounding the central atom. The VSEPR (Valence Shell Electron Pair Repulsion) theory helps predict the geometry based on the number of bonding and lone pairs. This concept is essential for understanding the shape and polarity of molecules, which influences their chemical behavior.

Dipole Moment

A dipole moment is a measure of the separation of positive and negative charges in a molecule, indicating its polarity. It arises when there is an uneven distribution of electron density, often due to differences in electronegativity between bonded atoms. Understanding dipole moments is important for predicting molecular interactions, solubility, and reactivity, as polar molecules behave differently than nonpolar ones.