Electron Displacement in Organic Molecules

Explore how electrons are displaced in organic reactions by the inductive effect, the mesmeric effect, and the electromagnet effect, and how plus and minus I groups influence electron flow.

The inductive effect transmits along a carbon chain from an electronegative atom through sigma bonds, diminishing with distance, and is influenced by electron-donating groups that alter acidity and conjugate-base stability.

Explore the mesomeric (resonance) effect as a pi-bond interaction that redistributes electron density in conjugated systems, highlighting donor and withdrawing groups.

Explore the mesomeric effect with bromine as an electron donating group and nitro as an electron withdrawing group on benzene, illustrating resonance structures and the resonance hybrid.

Explore the electromeric effect, a reagent-dependent, temporary electron displacement in a molecule's bonds, initiated by electrophiles or nucleophiles, illustrated with carbonyl-driven shifts.

Practice problems illustrate how inductive effects alter acidity, with electron withdrawing groups stabilizing the conjugate base and donating groups increasing basic character. Methylamine is a stronger base than ammonia.

Explore Arrhenius, Bronsted–Lowry, and Lewis acid-base concepts with definitions, examples, and how acids donate or accept protons and electrons in organic chemistry.

Explore common organic acids and bases, from carboxylic acids and phenols to amines and sodium alkoxides, and contrast Brønsted and Lewis concepts with electron donation.

Compute the strength of acids and bases by their extent of ionization and dissociation constants, relating Ka, Kb, and pKa, pKb to distinguish strong from weak acids and bases.

Explore how acid strength is determined by structural aspects and periodic trends, driven by electronegativity of the atom attached to the acidic hydrogen and conjugate base stability.

Explore how conjugate base stability, especially resonance stabilization, increases acid strength; compare acetic acid and ethanol, and note that strong conjugate bases accompany weak acids.

This lecture explains how acid strength varies across a period and down a group, showing that electronegativity increases acidity across a period and larger size stabilizes conjugate bases.

this lecture outlines the acidity order based on BK values, from strong inorganic acids to carboxylic acids, phenol, alcohol, then substituted hydrocarbons, ending with the least acidic hydrocarbons.

Explore how resonance stabilizes phenol's conjugate base via delocalization onto oxygen and the benzene ring, making phenol stronger than acetic acid, and note aluminum chloride as a Lewis acid.

Analyze acid strength among alkenes, acetylene, and benzene using sp hybridization and electronegativity, showing how s-character and electron-withdrawing groups influence acidity.

Compare cyclohexylamine and aniline: aniline's resonance delocalizes its nitrogen, lowering basicity; rank by nitrogen hybridization from sp3 to sp, with nitrile least basic and amines most basic.

Explore upcoming topics on organic reagents, electrophiles and nucleophiles, reactive intermediates, and arrow notation, and learn their importance and correct usage in organic reactions.