Chemical Reactions and Equations Vocabulary

A set of vocabulary flashcards covering the fundamental concepts of chemical reactions, equations, types of reactions, and oxidation effects based on Chapter 1.

Chemical Reaction

A process where the nature and the identity of the initial substance have changed, signaling that a chemical change has occurred.

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 mass is not the same on both sides because the number of atoms of each element is not equal.

Balanced chemical equation

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

Hit-and-trial method

A method of balancing chemical equations by using the smallest whole number coefficient to make the number of atoms of each element equal on both sides.

Aqueous (aq)

A notation used in chemical equations to indicate 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, with the chemical formula $CaO(s)$.

Slaked lime

The common name for calcium hydroxide, with the chemical formula $Ca(OH)_2(aq)$, produced by the reaction of calcium oxide and water.

Exothermic chemical reactions

Reactions in which heat is released along with the formation of products.

Respiration

An exothermic process where glucose ($C_6H_{12}O_6(aq)$) combines with oxygen in the cells of our body to provide energy.

Decomposition reaction

A reaction where a single reactant breaks down to give simpler products.

Thermal decomposition

A decomposition reaction that is carried out by heating the reactant.

Endothermic reactions

Reactions in which energy is absorbed, either in the form of heat, light, or electricity, to break down the reactants.

Displacement reaction

A chemical reaction in which a more reactive element displaces or removes another element from its compound.

Precipitate

An insoluble substance formed during a chemical reaction in a solution.

Precipitation reaction

Any reaction that produces a 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 reaction.

Reduction

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

Redox reactions

Reactions in which one reactant gets oxidised while the other gets reduced; also known as oxidation-reduction reactions.

Corrosion

The process where a metal is attacked by substances in its environment, such as moisture and acids, leading to damage (e.g., rusting of iron).

Rancidity

A condition produced by the oxidation of fats and oils in food, resulting in a change in smell and taste.