Untitled Flashcards Set

Kinetic Energy - The energy of motion; particles in gases have the most kinetic energy, while particles in solids have the least.

Intermolecular Forces (IMFs) - Forces between molecules; strongest in solids, medium in liquids, and weakest in gases.

Vapor Pressure - The pressure exerted by gas particles above a liquid in a closed container; increases with temperature.

Boiling Point - The temperature at which a liquid’s vapor pressure equals the external pressure.

Normal Boiling Point - The boiling point of a liquid at standard pressure (101.3 kPa).

Surface Tension - The inward force that minimizes the surface area of a liquid, caused by cohesive forces.

Capillary Action - The ability of a liquid to flow in narrow spaces without external forces, due to adhesive and cohesive forces.

Viscosity - A liquid’s resistance to flow; increases with stronger intermolecular forces.

Polar Molecule - A molecule with an uneven distribution of charge, like water.

Hydrogen Bonding - A strong type of dipole-dipole interaction between a hydrogen atom and an electronegative atom (e.g., oxygen).

Universal Solvent - Water’s ability to dissolve more substances than any other liquid.

Solution - A homogeneous mixture of two or more substances.

Solute - The substance that dissolves in a solution.

Solvent - The substance in which the solute dissolves.

Aqueous Solution - A solution where water is the solvent.

Soluble - A substance that can dissolve in a particular solvent.

Insoluble - A substance that cannot dissolve in a particular solvent.

Dissociation - The separation of ions in an ionic compound when dissolved in water.

Solvation - The process of solvent particles surrounding and separating solute particles.

Hydration - Solvation when the solvent is water.

Heterogeneous Mixture - A mixture where components are not uniformly distributed (e.g., salt and pepper).

Suspension - A heterogeneous mixture where particles settle out over time.

Colloid - A heterogeneous mixture with particles larger than in solutions but smaller than in suspensions; does not settle out.

Tyndall Effect - The scattering of light by particles in a colloid.

Brownian Motion - The random movement of particles in a colloid due to collisions with solvent molecules.

Coagulation - The clumping together of colloid particles, often due to the addition of an electrolyte.

Emulsion - A colloidal dispersion of one liquid in another, stabilized by an emulsifying agent.

Saturated Solution - A solution that contains the maximum amount of solute that can dissolve at a given temperature.

Unsaturated Solution - A solution that contains less solute than the maximum amount that can dissolve.

Supersaturated Solution - A solution that contains more solute than it should at a given temperature; unstable.

Solubility - The maximum amount of solute that can dissolve in a given amount of solvent at a specific temperature.

Solubility Curve - A graph showing the relationship between solubility and temperature for different substances.

Rate of Dissolving - The speed at which a solute dissolves in a solvent; influenced by agitation, surface area, and temperature.

Molarity (M) - The concentration of a solution, expressed as moles of solute per liter of solution.

Dilution - The process of reducing the concentration of a solution by adding more solvent.

Percent by Mass - The ratio of the mass of the solute to the mass of the solution, expressed as a percentage.

Percent by Volume - The ratio of the volume of the solute to the volume of the solution, expressed as a percentage.

Colligative Properties - Properties of solutions that depend on the number of solute particles, not their identity (e.g., vapor pressure lowering, boiling point elevation, freezing point depression).

Vapor Pressure Lowering - The decrease in vapor pressure of a solvent when a solute is added.

Boiling Point Elevation - The increase in a solution’s boiling point compared to the pure solvent.

Freezing Point Depression - The decrease in a solution’s freezing point compared to the pure solvent.

Electrolyte - A substance that conducts electricity when dissolved in water, due to the presence of ions.

Non-electrolyte - A substance that does not conduct electricity when dissolved in water.

Ion-dipole Force - An intermolecular force between an ion and a polar molecule.

Dipole-dipole Force - An intermolecular force between two polar molecules.

London Dispersion Forces (LDF) - Weak intermolecular forces caused by temporary dipoles in nonpolar molecules.

Dipole-induced Dipole - An intermolecular force where a polar molecule induces a dipole in a nonpolar molecule.

Recrystallization - The process of solute particles returning to the solid state from a solution.

Solubility Product (Ksp) - The equilibrium constant for the dissolution of a solid in a solution.

Molar Mass - The mass of one mole of a substance, expressed in grams per mole (g/mol).