Intermolecular Forces: Hydrogen Bonds and More

Hydrogen Bonding

Strong dipole-dipole interaction involving H bonded to F, O, N.

Dipole-Dipole Forces

Attraction between polar molecules' positive and negative ends.

London Dispersion Forces

Weakest intermolecular force, present in all molecules.

Covalent Bond

Strong bond formed by sharing electron pairs between atoms.

Polar Molecule

Molecule with uneven distribution of charge, creating dipoles.

Non-Polar Molecule

Molecule with even charge distribution, no permanent dipoles.

Boiling Point (BP)

Temperature at which a liquid turns into vapor.

Melting Point (MP)

Temperature at which a solid turns into liquid.

Ionic Compound

Compound formed from ionic bonds between metals and nonmetals.

Electron Cloud

Region around an atom where electrons are likely found.

Induced Dipole

Temporary dipole created when a dipole distorts another's electron cloud.

Hydrogen Bond Example

NH3 has higher BP than PH3 due to hydrogen bonds.

Halogen Properties

Boiling/melting points increase down the group due to size.

Lattice Structure

Regular arrangement of ions in an ionic compound.

Solvation Shell

Layer of solvent molecules surrounding solute particles.

Attraction Strength

Depends on polarity and size of molecules involved.

Physical Change

Change affecting form but not chemical composition.

Chemical Change

Change resulting in the formation of new substances.

Intermolecular Forces

Forces between molecules affecting physical properties.

Ion-Dipole Forces

Attraction between ions and polar molecules, crucial in solutions.

Molecular Size Effect

Larger molecules have stronger London dispersion forces.

Electron Distribution

Constantly changing arrangement of electrons in a molecule.