SEM2

Pressure

The force exerted per unit area in a system.

Factors that increase pressure

Increasing temperature, decreasing volume, and increasing the number of moles of gas.

Kinetic Molecular Theory

Describes the behavior of gases in terms of particles in motion, explaining gas laws.

Ideal Gas Constant (R)

The constant used in the ideal gas law, given in units of $0.0821 \frac{L \times atm}{K \times mol}$.

STP (Standard Temperature and Pressure)

Conditions of 0°C (273.15 K) and 1 atm pressure, used as reference points.

Stoichiometry

The calculation of reactants and products in chemical reactions.

Solubility

The ability of a substance to dissolve in a solvent.

Suspension

A heterogeneous mixture in which solid particles are suspended in a liquid.

Colloid

A mixture where microscopic particles are dispersed throughout but not settled.

Electrolyte

A substance that produces an electrically conducting solution when dissolved.

Catalyst

A substance that increases the rate of a chemical reaction without being consumed.

Arrhenius acid

A substance that increases the concentration of H+ ions in aqueous solution.

Bronsted-Lowry acid

A substance that donates a proton (H+) in a chemical reaction.

Lewis acid

A substance that accepts an electron pair to form a covalent bond.

pH

A measure of the acidity or alkalinity of a solution, based on H3O+ concentration.

Specific heat

The amount of heat required to raise the temperature of one gram of a substance by one degree Celsius.

Enthalpy change (ΔH)

The heat content change during a reaction at constant pressure.

Exothermic reaction

A reaction that releases heat, resulting in a decrease in enthalpy.

Endothermic reaction

A reaction that absorbs heat, resulting in an increase in enthalpy.

Collisions theory

The theory that reaction rates depend on the collisions between molecules.

Rate law

An equation that relates the reaction rate to the concentration of reactants.

Equilibrium expression

A mathematical expression that relates the concentrations of reactants and products at equilibrium.

Common ion effect

The decrease in solubility of an ionic compound caused by the presence of a common ion.

Ksp (Solubility Product Constant)

An equilibrium constant for the dissolution of a sparingly soluble compound.

oxidation number

A measure of the degree of oxidation of an atom in a compound.

Redox reaction

A reaction involving the transfer of electrons between two species.

Voltaic cell

A device that converts chemical energy into electrical energy through a spontaneous reaction.

Electrolytic cell

A device that uses electrical energy to drive a non-spontaneous chemical reaction.

Anode

The electrode where oxidation occurs in a cell.

Cathode

The electrode where reduction occurs in a cell.