The Nature of Chemical Bonds and Forming Covalent Bonds (VBT)
Start with the big picture
Atoms form bonds through their valence electrons, often attaining an octet or duet. In valence bond theory, covalent bonds arise from overlap of half-filled orbitals: head-on overlap forms σ bonds, while parallel p-orbital overlap forms π bonds. Hybridization helps describe carbon’s geometry in methane, ethene, and ethyne. Bond order, orbital s-character, and electronegativity are related to bond strength, length, polarity, and the acidity of attached hydrogen atoms. Formal charge, resonance, and bond cleavage provide further tools for understanding electron distribution and reaction mechanisms. The lesson also introduces Brønsted–Lowry and Lewis acid–base definitions, acid and base strength, and how conjugate-base stability influences acidity. Together, these concepts show how bonding and electron effects help explain molecular structure and reactivity.
What you'll learn
- Explain how valence electrons contribute to covalent bond formation.
- Distinguish σ and π bonds by their orbital overlap and properties.
- Relate carbon hybridization and s-character to geometry and bond behavior.
- Describe how resonance, induction, and conjugate-base stability affect acidity.
- Compare Brønsted–Lowry and Lewis definitions of acids and bases.
Continue your study
Work through the complete notes and reinforce the topic with the study tools available in the full lesson.
