Chemical Reactions and Equations Practice Flashcards

This set of vocabulary flashcards covers the fundamental concepts of chemical reactions, types of reactions, balancing equations, and everyday chemical phenomena as described in Chapter 1.

Chemical Reaction

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

Reactants

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

Products

The new substances formed during a chemical reaction, usually 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, indicating that the mass is not balanced.

Law of conservation of mass

A law stating that mass can neither be created nor destroyed in a chemical reaction; the total mass of elements in products must equal the total mass of elements in reactants.

Balanced chemical equation

A chemical equation in which the number of atoms of each element remains the same before and after a chemical reaction.

Hit-and-trial method

A method of balancing chemical equations by making trials to balance the equation using the smallest whole number coefficient.

Aqueous (aq)

A notation used in a chemical equation if the 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, given by the formula $CaO(s)$, used in industries like the manufacture of cement.

Slaked lime

The common name for calcium hydroxide, given by the formula $Ca(OH)_2(aq)$, produced by the reaction of quick lime with 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 body cells 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 in the form of heat, light, or electricity to break down reactants.

Displacement reaction

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

Precipitate

An insoluble substance formed during a chemical reaction.

Double displacement reaction

Reactions 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

Also known as oxidation-reduction reactions, these occur when one reactant gets oxidised while the other gets reduced during the process.

Corrosion

The process where a metal is attacked by substances in its environment such as moisture and acids, such as the rusting of iron or green coating on copper.

Rancidity

A condition occurring when fats and oils are oxidised, resulting in a change in their smell and taste.

Antioxidants

Substances added to foods containing fats and oils to prevent oxidation and slow down the process of becoming rancid.