Chemical Reactions and Equations

A process where new substances with different properties are formed due to the rearrangement of atoms.

A change that does not produce new substances and is temporary. Examples include melting ice or boiling water.

A change that results in the formation of new substances with different properties. It is usually permanent. Examples include burning wood or rusting iron.

A chemical reaction where the number of atoms of each element on the reactant side is equal to the number of atoms of that element on the product side. It follows the law of conservation of mass.

A chemical reaction where the number of atoms of each element on the reactant side is not equal to the number of atoms of that element on the product side. It does not follow the law of conservation of mass.

A reaction where a single substance breaks down into two or more simpler substances. Example: Decomposition of hydrogen peroxide into water and oxygen.

A reaction where two or more substances combine to form a single, more complex substance. Example: Formation of water from hydrogen and oxygen.

A reaction where one element replaces another element in a compound. Example: Iron reacting with copper sulfate to form iron sulfate and copper.

A reaction where two compounds exchange their ions to form two new compounds, one of which is usually a precipitate. Example: Lead nitrate reacting with potassium iodide to form lead iodide and potassium nitrate.

A reaction where a substance reacts with oxygen, producing heat and light. Example: Burning of magnesium ribbon in air.

An insoluble solid formed during a chemical reaction in a solution. Example: The yellow precipitate formed when lead nitrate reacts with potassium iodide.

A chemical reaction that releases energy into the surroundings, usually as heat. Example: Burning of magnesium ribbon, which produces heat and light.

A chemical reaction that absorbs energy from the surroundings, usually as heat. Example: Dissolving ammonium chloride in water.

The substance that is being changed in a chemical reaction. Example: Magnesium ribbon in the burning of magnesium ribbon.

The new substance formed in a chemical reaction. Example: Magnesium oxide in the burning of magnesium ribbon.

A substance that speeds up a chemical reaction without being consumed in the process. Example: Enzymes in biological reactions.

A substance that slows down a chemical reaction. Example: Antioxidants in food.

A chemical reaction where the forward and reverse reactions occur at the same rate, resulting in no net change in the concentrations of reactants and products. Example: The reaction between hydrogen and iodine to form hydrogen iodide.

A type of reaction where a compound reacts with oxygen, producing heat and light. Example: Burning wood, burning natural gas.

The process of separating a metal from its ore by oxidation followed by reduction. Example: Extraction of iron from iron oxide.

The process of reacting a metal with oxygen to form its oxide. Example: Rusting of iron.

The process of removing oxygen from a compound. Example: Heating copper oxide in the presence of hydrogen to form copper.

A substance that gains electrons during a chemical reaction. Example: Oxygen in the reaction of magnesium with oxygen.

A substance that loses electrons during a chemical reaction. Example: Magnesium in the reaction of magnesium with oxygen.

The minimum amount of energy needed for a reaction to start.

The measure of the rate of a chemical reaction. It is influenced by factors such as temperature, concentration, and catalysts.

The study of the relationships between the chemical and physical properties of substances and the rates and extent of chemical reactions.

The study of the energy changes that accompany chemical reactions.

The rate of a chemical reaction can be determined by monitoring the change in concentration of a reactant or product over time.