Chemical Reactions, Stoichiometry, Solutions, Thermochemistry, Acids and Bases, Gas Laws

Flashcards for vocabulary review

Chemical Equation

A representation of a chemical reaction using chemical formulas and symbols.

Balancing Equations

Adjusting the coefficients in a chemical equation to ensure that the number of atoms of each element is the same on both sides of the equation.

Synthesis (Combination) Reaction

A reaction in which two or more substances combine to form a single product.

Decomposition Reaction

A reaction in which a single compound breaks down into two or more simpler substances.

Single Replacement Reaction

A reaction in which one element replaces another element in a compound.

Double Replacement Reaction

A reaction in which the cations of two ionic compounds switch places.

Combustion Reaction

A reaction in which a substance reacts rapidly with oxygen, producing heat and light.

Endothermic Reaction

A reaction that absorbs energy from its surroundings.

Change in Color

A visual indication that a chemical reaction has occurred.

Energy Change

A temperature change or the production of light indicating a chemical reaction.

Gas Production

The release of a gas as evidence of a chemical reaction.

Formation of a Precipitate

The formation of a solid from a solution during a chemical reaction.

Change in Odor

A change in scent indicating a chemical reaction.

Precipitate

A solid that forms out of solution during a chemical reaction.

Net Ionic Equation

A chemical equation that shows only the species that participate in the reaction.

Spectator Ions

Ions that are present in a reaction mixture but do not participate in the reaction.

Collision Theory

The theory that chemical reactions occur when reactant particles collide with sufficient energy and proper orientation.

Activation Energy

The minimum energy required for a chemical reaction to occur.

Catalyst

A substance that speeds up a chemical reaction without being consumed in the reaction.

Molar Mass

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

Mole

A unit of measurement used to express amounts of a chemical substance.

Stoichiometry

The quantitative relationship between reactants and products in a chemical reaction.

Limiting Reactant

The reactant that is completely consumed in a chemical reaction and determines the amount of product formed.

Excess Reactant

The reactant that remains after the limiting reactant is completely consumed in a chemical reaction.

Percent Yield

he ratio of the actual yield to the theoretical yield, expressed as a percentage.

Human Error

Mistakes made by the person conducting the experiment.

Systematic Error

Error due to issues with equipment or experiment design.

Random Error

Error due to unpredictable variations in measurement.

Solute

The substance that is dissolved in a solution.

Solvent

The substance that dissolves the solute in a solution; typically present in a larger amount.

Solution

A homogeneous mixture of solute and solvent.

Concentration

The amount of solute present in a solution.

Molarity

Moles of solute per liter of solution (M = mol/L).

Heat (q)

The transfer of thermal energy from one object to another.

Specific Heat Capacity

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

Calorimetry

The measurement of the quantity of heat exchanged in a chemical reaction.

Calorimeter

A device used to measure the heat transferred during a chemical reaction.

Temperature

A measure of the average kinetic energy of the particles in a substance.

System

The portion of the universe that is singled out for study.

Surroundings

Everything outside the system.

State Function

A property whose value does not depend on the path taken to reach that specific value. Examples enthalpy, energy, and entropy.

Enthalpy (H)

The total energy of a system.

Change in Enthalpy (ΔH)

The amount of energy transferred during a chemical reaction.

Activation Energy

The energy needed to start a chemical reaction.

Bond Enthalpy

The energy stored while holding elements together in a compound.

Enthalpy of Formation (ΔHf o)

The change in enthalpy associated with the formation of one mole of a compound from its elements in their standard states.

Entropy (S)

A measure of how dispersed the energy of a system is at a specific temperature.

Spontaneous Reaction

A reaction that favors the formation of products.

Non-spontaneous Reaction

A reaction that favors the formation of reactants.

Gibbs Free Energy (ΔGº)

The amount of energy that is available to do useful work.

Acids

Substances that have the potential to donate a proton.

Bases

Substances that can accept protons.

Titration

A lab technique used to determine the unknown concentration of a solution.

Titrant

A solution of a known concentration, which is added to another solution whose concentration has to be determined.

Analyte

The solution whose concentration has to be determined.

Equivalence Point

The point in a titration at which the amount of titrant added is just enough to completely neutralize the analyte solution.

Half-Equivalence Point

The point in a titration where the conjugate base and acid (or conjugate acid and base) are equal in concentration.

Kinetic Molecular Theory

The theory that all matter is made up of particles that are always moving.

Thermal Energy

The kinetic energy of particles.

Pressure

A force exerted on an object.

Boyle’s Law

The principle that at constant temperature, the volume and pressure of a gas are inversely proportional.

Charles’ Law

The principle that at constant pressure, the volume and the temperature of a gas are directly proportional.

Gay-Lussac’s Law

The principle that at constant volume, the temperature and pressure of a gas are directly proportional.