Chapter 1 Summary & Key Takeaways

Chapter 1 lays the foundation for everything that follows in organic chemistry. Use this page as a quick refresher before diving into mechanisms and synthesis.

Core Concepts

• Structure & bonding: Carbon’s tetravalency and hybridization (sp, sp², sp³) explain molecular shapes and bond angles; formal charge keeps Lewis structures honest.
• Resonance: Electron delocalization stabilizes ions and intermediates; only electrons move, not atoms.
• Geometry & polarity: VSEPR predicts 3D shapes; polarity depends on both bond dipoles and symmetry.
• Acid–base basics: pKₐ sets equilibrium direction; ARIO (atom, resonance, induction, orbital) explains conjugate-base stability.
• Functional groups: Recognizing –OH, –NH₂, carbonyls, halides, etc., lets you predict reactivity and physical properties.
• Nomenclature & isomerism: IUPAC rules name the parent, substituents, and functional group priority; distinguish constitutional vs stereoisomers (enantiomers, diastereomers, meso).

Quick Checks

• Can you assign hybridization and predict geometry for any atom in a small molecule?
• Can you draw major resonance contributors and identify the resonance hybrid?
• Do you know which conjugate base is most stabilized (and why) using ARIO?
• Can you name a branched chain and spot its functional groups?
• Can you label a pair as enantiomers, diastereomers, or identical?

Summary

• Hybridization drives shape; formal charge and resonance keep structures chemically reasonable.
• pKₐ differences drive acid–base equilibria toward the weaker acid/base pair.
• Functional groups are reactivity shortcuts—learn their signatures early.
• Clear naming and isomer classification prevent miscommunication and mistakes later.