Chapter 5: Covalent Bonding
- Page ID
- 22831
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- Chapter 5.1: Representing Covalent Bonds
- This page explores the distinctions between covalent and ionic bonding, focusing on the role of electrostatic attractions and the characteristics of ionic versus covalent compounds. It details how to write molecular formulas for both organic and inorganic compounds, emphasizing elemental composition and providing examples like nitrous oxide.
- Chapter 5.2: Lewis Electron Dot Symbols
- This page explains Lewis electron dot symbols, created by G. N. Lewis, for predicting bond formation based on valence electrons. It illustrates how these symbols represent valence electrons and relate to the octet rule, with mentions of exceptions. The page highlights the importance of Lewis dot symbols in understanding chemical bonding, compound properties, and stoichiometry.
- Chapter 5.3: Lewis Structures
- This page explores covalent bonding and the use of Lewis dot symbols for molecular structures, emphasizing the balance of attractive and repulsive forces in bond formation. It covers the construction of Lewis structures while accounting for valence electrons, formal charges, and resonance structures for various compounds, including ozone and carbon dioxide.
- Chapter 5.4: Exceptions to the Octet Rule
- This page explores exceptions to the octet rule in Lewis dot structures, highlighting cases of odd electron counts, expanded valence shells with d orbital involvement, and electron-deficient species. Notable examples include nitric oxide (NO) and SF6, as well as BCl3. The content emphasizes the significance of these exceptions in understanding molecular structures and bonding, supplemented with exercises and conceptual problems to deepen comprehension.
- Chapter 5.5: Properties of Covalent Bonds
- This page covers covalent bonding, detailing bond order, length, and energy. It explains bond order as the number of electron pairs, identifying trends where bond length decreases with increasing order and energy is highest in triple bonds. The page also examines bond strength among periodic elements, noting exceptions in period 2 (N, O, F) and trends of weaker bonds down groups.
- Chapter 5.6: Properties of Polar Covalent Bonds
- This page covers bond polarity and ionic character, linking them to electronegativity differences and bond types (ionic, covalent, polar covalent). It defines polar bonds as those with unequal electron sharing and introduces dipole moments for charge distribution illustration. The page mentions examples like HCl and NaCl, noting that even highly electronegative differences yield less than complete ionic character in gas phase, and discusses dipole interactions in solids.
- Chapter 5.7: Metallic Bonding
- This page covers metallic bonding and its properties like conductivity and malleability, explained through Drude's model of delocalized electrons. It examines sodium and magnesium, emphasizing the role of delocalization and ionic charge in bond strength. Additionally, it introduces Band Theory, detailing conduction and valence bands.
- Chapter 5.8: Molecular Representations
- This page covers the distinctions between ionic and covalent bonding, including their formation through electrostatic interactions. It explains molecular and structural formulas, deriving them from elemental compositions, and emphasizes Lewis structures for depicting bonding. The properties of these compounds are discussed, highlighting differences like melting points and structural models.