Unit 1C: Intermolecular Forces & Mixtures Study Guide (Honors)

This set of flashcards covers key concepts related to intermolecular forces, types of bonds, solutions, solubility, and laboratory procedures to prepare for the exam.

Intermolecular Forces

Forces of attraction or repulsion between neighboring particles (molecules or atoms).

Ionic Bond

A type of chemical bond formed through the electrostatic attraction between oppositely charged ions.

Polar Covalent Bond

A type of bond where two atoms share electrons unequally, resulting in a molecule with a slight dipole.

Nonpolar Covalent Bond

A bond formed between two atoms that share electrons equally, resulting in no charge separation.

Hydrogen Bonding

A strong type of dipole-dipole interaction that occurs between a hydrogen atom bonded to a highly electronegative atom and another electronegative atom.

Dipole-Dipole Interaction

The attractive force between the positive end of one polar molecule and the negative end of another polar molecule.

London Dispersion Forces

Weak intermolecular forces arising from temporary dipoles in molecules, present in all molecules.

Solubility

The ability of a substance to dissolve in a solvent at a given temperature and pressure.

Saturated Solution

A solution in which the maximum amount of solute has been dissolved at a given temperature.

Unsaturated Solution

A solution that has less solute than can be dissolved at a given temperature.

Supersaturated Solution

A solution that contains more dissolved solute than is required to reach equilibrium at a given temperature.

Colloid

A mixture where tiny particles are dispersed in a fluid but do not settle out or separate over time.

Suspension

A heterogeneous mixture in which solute-like particles settle out of a solvent-like phase after mixing.

Factors Increasing Solid Solubility

Temperature increase, stirring, and surface area increase solubility by increasing particle interactions.

Factors Increasing Gas Solubility

Higher pressure and lower temperature increase gas solubility due to decreased kinetic energy and fewer collisions.

Molarity

A measure of concentration representing the number of moles of solute per liter of solution.

Dilution

The process of reducing the concentration of a solute in a solution, usually by mixing with more solvent.