Chemical Reactions and Equations - Vocabulary Flashcards

Vocabulary flashcards covering key terms and concepts from the notes on chemical reactions and equations.

Chemical change

A change in which the chemical identity of a substance is altered due to a chemical reaction.

Chemical reaction

The process that leads to chemical change, transforming reactants into products.

Reactants

Starting substances on the left side of a chemical equation.

Products

Substances formed on the right side of a chemical equation.

Word equation

A verbal description of a reaction using names of reactants and products.

Skeletal equation

A chemical equation that shows formulas but is not balanced in terms of atom counts.

Balanced equation

A chemical equation with equal numbers of each type of atom on both sides.

Law of conservation of mass

Mass is conserved in a closed system; atoms are rearranged, not created or destroyed.

Coefficient

The number placed before a formula to balance atoms in an equation.

Balance (Hit and Trial method)

A method to balance equations by tallying atoms and adjusting coefficients until equal on both sides.

Boxing method

A balancing approach where each chemical formula is enclosed in a box and coefficients are adjusted without altering the contents.

Physical states notation

Symbols like G, L, AQ, S indicating gas, liquid, aqueous, solid in a chemical equation.

Combination reaction

Two or more reactants combine to form a single product.

Decomposition reaction

A single compound breaks down into two or more simpler substances.

Exothermic reaction

A reaction that releases heat.

Endothermic reaction

A reaction that absorbs heat.

Electrolytic decomposition

Decomposition of a compound by passing electricity (electrolysis).

Photolytic decomposition

Decomposition caused by exposure to light.

Displacement reaction

A reaction where a more reactive element displaces a less reactive element from a compound.

Double displacement reaction

Two compounds exchange ions to form two new compounds; may produce a precipitate.

Precipitation reaction

A reaction in which a solid precipitate forms from two solutions.

Oxidation

Process where a substance gains oxygen (and often loses electrons).

Reduction

Process where a substance loses oxygen (and often gains electrons).

Redox reaction

A reaction involving simultaneous oxidation and reduction.

Corrosion

Deterioration of metals due to reactions with moisture or other substances.

Rusting

Corrosion of iron forming iron oxide.

Rancidity

Oxidation of fats/oils causing bad smell/taste; prevention includes antioxidants, airtight containers, and nitrogen.