Chp 2—IMFs, Acid-Base

vector quantity that measures polarity of covalent bond

μ = d(δ) μ = dipole moment d = distance between atoms δ = charge

dipole moment of entire molecule

temperature at which equilibrium exists between crystalline solid state and liquid state

temperature at which vapor pressure of a liquid equals pressure of the atmosphere around the liquid

electrostatic attraction results in ionic bonds BP, MP is very high

ion-ion force

dipole dipole london dispersion hydrogen bonding

• polarizability — related to size — atoms with larger atomic radii have greater dispersion forces, as e- are further from nucleus • surface area — linear molecules have more dispersion forces than branced/spherical molecules

highly positive H + lone pairs on N, O, F of other molecules

HF > HO > HN

Acid: produces H+ in water Base: produces OH- in water

Acid: proton donor Base: proton acceptor

Acid: e- acceptor Base: e- donor

acids

• EN of atom connected to H (higher = more acidic) • size of atom connected to H (larger = more acidic) • orbital character of atom connected to H (more s character = more acidic) • delocalization of charge in conj. anion base (more resonance structure in conj base = more acidic) • inductive effects (higher EN of inductive group, shorter distance, higher number of inductive groups = more acidic)

higher pKa weaker acid

right and down

electron poor cations seek e- Lewis acids

electron rich anions seek to donate e- Lewis bases

nucleophiles attack electrophiles start arrow from nucleophile