IMF

Solids and liquids collectively characterized by strong intermolecular forces maintaining local order.

Condensed Matter

Substances with relatively weak intermolecular forces and high molecular motion.

Gases

Bonding forces within a molecule like covalent or ionic bonds.

Intramolecular Forces

Weaker interactions between molecules.

Intermolecular Forces

Measure of a liquid's resistance to flow influenced by IMF strength, molecular size/shape, and temperature.

Viscosity

IMF within a liquid aiming to minimize surface area.

Cohesive Forces

IMF between liquid molecules and the container.

Adhesive Forces

Spontaneous rising of a liquid in a narrow tube due to cohesive and adhesive forces.

Capillary Action

Resistance of a liquid to increase its surface area influenced by cohesive forces.

Surface Tension

Disordered structure with no lattice like cotton candy or glass.

Amorphous Solid

Regularly arranged components with a lattice structure like table salt.

Crystalline Solid

Crystalline solids with dipole-dipole or LDF forces between discrete molecules.

Molecular Solids

Crystalline solids with ionic bonds between ions.

Ionic Solids

Crystalline solids with metal atoms having delocalized covalent bonds or nonmetal atoms with directional covalent bonds.

Metallic Solids/Atomic Solids

forces in ionic and metallic substances

Interparticle forces

Types of IMF

1. Dipole-dipole (permanent) = polar

2. Hydrogen bonds = polar w/ H & F/O/N/S

3. van der Waals’ = induced (polar or not but

the only IMF in nonpolar)

the dipoles find the best compromise between attraction and repulsion, i.e, the molecules orient themselves to maximize the B,E interactions and to minimize B,B and E,E interactions

Dipole-dipole

Particularly strong dipole–dipole forces (H is bound to a highly EN atom: N, O, F)

Hydrogen Bond

forces that exist among noble gas atoms and nonpolar molecules

London Dispersion

Attraction between charge on anion and end of dipole with opposite charge

ion-dipole 35-400

Attraction between opposite partially chraged ends of polar molecules

Dipole-dipole 5-30

Attraction between partially positively charged H atom which attached to highly electronegative atom and a line pair on another atom

hydrogen bond 10-40

Attraction between an instantaneous dipole and a dipole induced in a neighboring atom or molecule

London dispersion

Liquids exhibit many characteristics that help us understand their nature: (3)

low compressibility, lack of rigidity, and high density compared with gases

liquid’s resistance to flowv

viscosity

determine viscosity: (3)

Strength of IMF, size/shape of molecule, temperature

IMF among the molecules of the liquid, aims to minimize surface

IMF between the liquid molecules & the container

Cohesive vs. adhesive

Liquid flow through material because of attraction between the liquid & the material

 CAPILLARY ACTION (adhesive + cohesive force > gravity)

depends on strength of cohesive forces

Surface tension

irregularly high surface tension (strong H bonds & size)

water

non metal atoms, directional covalent

network

crystalline solids determined by

X-ray diffraction