Covalent molecules are built through the sharing of electron pairs between non-metal atoms, aiming for a stable electronic configuration. Key examples include H2O, CO2, and CH4, each showcasing different covalent bonds and molecular geometries. Physical properties like low melting points and poor electrical conductivity are characteristic of these molecules, influenced by intermolecular forces and molecular shapes as explained by VSEPR theory.
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Non-metal atoms share pairs of electrons to form covalent bonds, resulting in stable electronic configurations
Dot and Cross Diagrams
Lewis structures, also known as dot and cross diagrams, illustrate the shared electron pairs in covalent molecules
Diatomic molecules and simple compounds, such as hydrogen, oxygen, and water, serve as prime examples of covalent bonding
Covalent molecules have low melting and boiling points due to weak intermolecular forces between separate molecules
Covalent molecules are typically poor conductors of electricity due to the lack of free-moving charged particles
The Valence Shell Electron Pair Repulsion (VSEPR) theory explains the three-dimensional shapes of covalent molecules based on the arrangement of electron pairs around a central atom
Covalent molecules play critical roles in various physical processes, such as phase transitions, due to their distinct properties
Covalent molecules are essential components of biological systems, contributing to the structure and function of living organisms
A thorough understanding of covalent molecules and their properties is crucial for students of chemistry and serves as a foundation for further study in the field
00
______ molecules occur when non-metal atoms share electron pairs, creating ______ bonds for stability.
Covalent
covalent
01
Define Lewis structures.
Lewis structures are diagrams that show the bonding between atoms of a molecule and the lone pairs of electrons that may exist.
02
What is a single covalent bond?
A single covalent bond is formed when two atoms share one pair of electrons.
