A covalent bond is a chemical bond formed by the sharing of one or more pairs of electrons between two atoms. This type of bond is responsible for the stability and structure of many molecules and is a fundamental concept in understanding the topics of 7.2 Covalent Bonding, 7.3 Lewis Symbols and Structures, 7.4 Formal Charges and Resonance, 7.5 Strengths of Ionic and Covalent Bonds, 7.6 Molecular Structure and Polarity, and 8.1 Valence Bond Theory.
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The strength of a covalent bond is determined by the electronegativity difference between the bonded atoms, with a larger difference resulting in a stronger bond.
Covalent bonds can be classified as either polar or nonpolar, depending on the electronegativity difference between the atoms involved.
The Lewis structure of a molecule represents the arrangement of atoms and the sharing of electrons in covalent bonds, providing information about the formal charges and resonance structures.
The strength of a covalent bond is directly related to the bond length, with shorter bond lengths indicating stronger bonds.
Valence bond theory explains the formation of covalent bonds by the overlap of atomic orbitals, leading to the creation of sigma (σ) and pi (π) bonds.
Review Questions
Explain how the concept of covalent bonding is related to the topics of 7.2 Covalent Bonding and 7.3 Lewis Symbols and Structures.
Covalent bonding is the central focus of 7.2 Covalent Bonding, where the formation of covalent bonds between atoms is discussed in detail. The sharing of electrons between atoms is the basis for covalent bond formation, and the Lewis symbols and structures introduced in 7.3 provide a visual representation of these bonds, showing how atoms share electrons to achieve stable configurations.
Describe the relationship between covalent bonds, formal charges, and resonance structures, as covered in 7.4 Formal Charges and Resonance.
Covalent bonds play a crucial role in the concept of formal charges, as the sharing of electrons between atoms can result in unequal distributions of charge. This understanding of formal charges is then extended to the discussion of resonance structures in 7.4, where multiple valid Lewis structures for a molecule are considered, and the covalent bonds are rearranged to minimize formal charges and maximize the stability of the molecule.
Analyze how the strength and polarity of covalent bonds, as discussed in 7.5 Strengths of Ionic and Covalent Bonds and 7.6 Molecular Structure and Polarity, influence the overall properties and behavior of chemical compounds.
The strength of a covalent bond, which is determined by the electronegativity difference between the bonded atoms, directly impacts the stability and reactivity of the molecule. Additionally, the polarity of covalent bonds, ranging from nonpolar to polar, influences the overall molecular structure and polarity, which in turn affects the intermolecular forces and physical properties of the compound. These concepts are crucial in understanding the relationships between covalent bonding and the macroscopic behavior of chemical systems.
A covalent bond in which the shared electrons are not equally shared, resulting in a partial positive and partial negative charge.
Sigma (σ) and Pi (π) Bonds: The two types of covalent bonds formed by the overlap of atomic orbitals, with sigma bonds being stronger and more stable than pi bonds.