Chemical Reactions and Equations

A set of vocabulary flashcards based on chemical reactions and equations.

Chemical Reaction

A process that leads to the transformation of one set of chemical substances to another.

Reactants

The starting materials in a chemical reaction, found on the left side of the equation.

Products

The substances formed as a result of a chemical reaction, found on the right side of the equation.

Word Equation

A method of expressing a chemical reaction using the names of the reactants and products.

Chemical Equation

A representation of a chemical reaction using symbols and formulas of the substances involved.

Balanced Equation

An equation with equal numbers of each type of atom on both sides, respecting the law of conservation of mass.

Combination Reaction

A reaction where two or more reactants combine to form a single product.

Decomposition Reaction

A reaction where a single compound breaks down into two or more simpler products.

Displacement Reaction

A reaction where one element displaces another in a compound.

Double Displacement Reaction

A reaction where two compounds exchange ions to form two new compounds.

Exothermic Reaction

A reaction that releases heat energy to the surroundings.

Endothermic Reaction

A reaction that absorbs heat energy from the surroundings.

Skeletal Equation

An unbalanced chemical equation that shows the reactants and products but not their quantities.

Corrosion

The gradual destruction of materials, usually metals, by chemical reactions with the environment.

Rancidity

The oxidation of fats and oils in food that leads to off-flavors and odors.

Oxidation

A chemical process in which a substance gains oxygen or loses hydrogen.

Reduction

A chemical process in which a substance loses oxygen or gains hydrogen.

Precipitate

An insoluble solid that forms when two solutions are mixed.

Physical State Notation

Symbols used in equations to indicate the physical states of reactants and products: (s) for solid, (l) for liquid, (g) for gas, (aq) for aqueous.

Catalyst

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

Hydrolysis

A reaction involving the breaking of a bond in a molecule using water.

Ammonium Chloride

An inorganic compound with the formula NH4Cl, used in various chemical reactions.

Sulphuric Acid

A strong acid with the formula H2SO4, used in various chemical reactions.

Zinc Oxide

A white powder with the formula ZnO, used in various applications including sunscreens.

Acid-Base Reaction

A reaction in which an acid and a base react to form water and a salt.

Carbon Dioxide

A colorless gas produced by respiration and combustion, with the formula CO2.

Chemical Bond

The lasting attraction between atoms that enables the formation of chemical compounds.

Symbolic Representation

The use of chemical symbols to represent elements and compounds in a chemical equation.

Mass Conservation Law

A principle stating that mass is neither created nor destroyed in a chemical reaction.

Heat Release

The energy given off during an exothermic reaction.

Hydrogen Gas

A colorless and odorless gas, represented by H2, that is often produced during chemical reactions.

Nitrogen Dioxide

A reddish-brown gas produced by combustion processes, with the formula NO2.

Copper Sulphate

A bright blue crystalline solid with the formula CuSO4, commonly used in displacement reactions.

Ferrous Sulphate

A green crystalline solid with the formula FeSO4, used in various applications.

Calcium Hydroxide

A white powder with the formula Ca(OH)2, also known as slaked lime.

Calcium Carbonate

A compound with the formula CaCO3, commonly found in rocks and used as a calcium supplement.

Sodium Hydroxide

A strong base with the formula NaOH, used in various chemical reactions.

Barium Sulphate

A white solid with the formula BaSO4, used as a contrast agent in medical imaging.

Electrolysis

A process that uses electricity to drive a chemical reaction.

Aqueous Solution

A solution in which water is the solvent.

Magnesium Oxide

A white solid with the formula MgO, produced by the burning of magnesium.

Calcium Oxide

A white powder known as quick lime, with the formula CaO.

Copper Chloride

A blue-green crystalline compound with the formula CuCl2, used in various chemical reactions.

Heat of Reaction

The difference in energy between reactants and products during a chemical reaction.

Element Displacement

The process where one element replaces another in a compound during a chemical reaction.

Ozone Layer

A region of Earth's stratosphere that contains a high concentration of ozone (O3) and absorbs most of the sun's UV radiation.

Ferrous Oxide

A black solid with the formula FeO, formed from iron.

Cation

A positively charged ion that results from the loss of one or more electrons.

Anion

A negatively charged ion that results from the gain of one or more electrons.

Photodecomposition

A chemical decomposition reaction caused by light.

Thermal Decomposition

The breakdown of a compound into simpler substances by heating.

Chemical Stability

The tendency of a substance to maintain its chemical structure under given conditions.

Flame Test

A qualitative analysis technique used to identify the presence of certain metal ions based on the color of the flame.

Hydration

The process of adding water to a substance.

Precipitation Reaction

A reaction that results in the formation of an insoluble product from soluble reactants.

Bimetallic Reaction

A type of redox reaction involving two metals.

Heavy and Light Metals

Terms used to describe metals based on their density and specific gravity.

Galvanization

The process of applying a protective zinc coating to iron or steel to prevent rusting.

Combustion Reaction

A reaction that occurs when a substance reacts rapidly with oxygen to produce heat and light.

Chemical Safety

The practices put in place to minimize the risks associated with chemical substances.

Environmental Impact

The effect that human activities, including chemical reactions, have on the environment.