Chemical Reactions and Equations

This set of flashcards covers the vocabulary and key conceptual definitions from the first chapter on chemical reactions and equations, including types of reactions, balancing methods, and everyday oxidation effects.

Chemical Reaction

A process in which the nature and identity of the initial substance change, resulting in a chemical change.

Reactants

The substances that undergo chemical change in a reaction, written on the left-hand side (LHS) of a chemical equation.

Product

The new substance formed during a chemical reaction, written on the right-hand side (RHS) of a chemical equation.

Skeletal Chemical Equation

A chemical equation where the number of atoms of each element is not the same on both sides, making the mass unbalanced.

Balanced Chemical Equation

An equation in which the number of atoms of each element remains the same before and after a chemical reaction, adhering to the law of conservation of mass.

Law of Conservation of Mass

A principle stating that mass can neither be created nor destroyed in a chemical reaction; thus, total product mass must equal total reactant mass.

Hit-and-Trial Method

A method of balancing chemical equations by using the smallest whole number coefficients to ensure equal numbers of atoms on both sides.

Aqueous $(aq)$

A notation indicating that a reactant or product is present as a solution in water.

Combination Reaction

A reaction in which a single product is formed from two or more reactants.

Quick Lime

The common name for Calcium oxide ($CaO$), which reacts vigorously with water to produce slaked lime.

Slaked Lime

The common name for Calcium hydroxide ($Ca(OH)_2$), which is used for whitewashing walls.

Exothermic Chemical Reaction

A reaction in which heat is released along with the formation of products, such as respiration or the burning of natural gas.

Decomposition Reaction

A reaction in which a single reactant breaks down into two or more simpler products.

Thermal Decomposition

A decomposition reaction that is carried out by heating common substances like magnesium carbonate or lead nitrate.

Endothermic Reaction

A reaction in which energy is absorbed from the surroundings in the form of heat, light, or electricity.

Displacement Reaction

A reaction where a more reactive element displaces or removes another element from its compound.

Precipitate

An insoluble substance that settles out of a solution during a chemical reaction.

Precipitation Reaction

Any chemical reaction that produces an insoluble substance (precipitate).

Double Displacement Reaction

A reaction in which there is an exchange of ions between the reactants to form new compounds.

Oxidation

The gain of oxygen or the loss of hydrogen by a substance during a chemical reaction.

Reduction

The loss of oxygen or the gain of hydrogen by a substance during a chemical reaction.

Redox Reactions

Chemical reactions involving both oxidation and reduction, where one reactant is oxidized while the other is reduced.

Corrosion

The process where a metal is gradually attacked and worn away by substances in the environment such as moisture, acids, and oxygen.

Rancidity

A condition where fats and oils in food are oxidized, leading to a noticeable change in their smell and taste.

Antioxidants

Substances added to foods containing fats and oils to prevent oxidation and maintain freshness.