BC Science 10: Chemical Processes and Reactions

Comprehensive vocabulary flashcard set covering chemical reactions, bonding, conservation of mass, reaction classifications, and energy changes based on BC Science Connections 10.

Chemical reaction

A process in which atoms of one or more substances are rearranged to form one or more different substances.

Physical change

A process describing matter according to characteristics that are observed and measured where no new substance is formed, representing only a change of state or shape.

Chemical change

A process in which one or more new substances are formed with distinct chemical properties, accompanied by clues such as colour change, heat or light release, bubble production, precipitate formation, or difficulty of reversal.

Qualitative property

A characteristic of matter that is observed using the senses, such as state of matter, colour, texture, and malleability.

Quantitative property

A characteristic of matter that is measured numerically, such as conductivity, viscosity, density, length, melting point, and boiling point.

Precipitate

An insoluble solid that forms from a chemical reaction occurring between two liquids or aqueous solutions.

WHMIS

Workplace Hazardous Materials Information System; a Canadian system that uses standardized safety symbols and labels to communicate hazard information for chemicals used in labs and workplaces.

Safety Data Sheet (SDS)

A technical document providing comprehensive information regarding the chemical properties, potential hazards, handling procedures, and first aid treatments for a specific substance.

Pure substance

A form of matter with a uniform and constant chemical composition, classified specifically as either an element or a compound.

Element

A pure substance composed entirely of only one type of atom that cannot be broken down into simpler substances by ordinary chemical processes.

Compound

A pure substance composed of atoms of two or more different elements chemically bonded together in fixed proportions.

Ionic bond

A strong electrostatic attraction that forms between oppositely charged ions following the transfer of valence electrons from a metal atom to a non-metal atom.

Ionic compound

A compound composed of a metal element and a non-metal element bound together through ionic bonds created by oppositely charged ions.

Covalent bond

A strong chemical attraction formed between non-metal atoms when they share valence electrons to achieve stable, full electron shells.

Covalent compound

A chemical compound formed when atoms of two or more non-metal elements bond together by sharing valence electrons.

Molecule

A neutral group of two or more atoms joined together by covalent bonds, representing the smallest fundamental unit of most covalent compounds.

Open system

A reaction system in which both matter and energy can freely enter or leave into the surrounding environment.

Closed system

A reaction system in which energy can enter or leave, but matter is completely sealed and cannot enter or escape.

Law of conservation of mass

The scientific principle stating that in a closed chemical system, mass is neither created nor destroyed; the total mass of the reactants always equals the total mass of the products.

Chemical equation

A symbolic representation of a chemical reaction using chemical formulas and state symbols to denote the identities and proportional quantities of reactants and products.

Reactant

A starting chemical substance that undergoes a chemical change during a chemical reaction, written on the left side of a chemical equation.

Product

A new chemical substance formed as a result of a chemical reaction, written on the right side of a chemical equation.

Coefficient

A whole number placed directly in front of a chemical formula in a balanced equation that multiplies all the atoms in the formula unit or molecule.

Subscript

A small number placed to the lower right of an element symbol in a formula indicating the exact number of atoms of that element present in the particle.

Diatomic element

A non-metal element that naturally exists as paired molecules of two identical atoms joined by a covalent bond, specifically $H_2$, $N_2$, $O_2$, $F_2$, $Cl_2$, $Br_2$, and $I_2$.

Activation energy

The minimum kinetic energy that colliding reactant particles must possess in order to break existing chemical bonds and initiate a chemical reaction.

Exothermic reaction

A chemical reaction characterized by a net release of energy to the surroundings, resulting in a temperature increase in the surrounding environment.

Endothermic reaction

A chemical reaction characterized by a net absorption of energy from the surroundings, resulting in a temperature decrease in the surrounding environment.

Synthesis reaction

A type of chemical reaction where two or more simple reactants combine to produce a single, more complex compound ($A + B \rightarrow AB$), typically releasing energy.

Decomposition reaction

A chemical reaction where a single complex compound absorbs energy and breaks down into two or more elements or simpler compounds ($AB \rightarrow A + B$).

Single replacement reaction

A chemical reaction in which a free element reacts with an aqueous compound, displacing an element within the compound to produce a new element and a new compound.

Double replacement reaction

A chemical reaction in which solutions of two ionic compounds exchange their positive ions to produce two entirely new compounds, commonly resulting in a solid precipitate.

Combustion reaction

A rapid exothermic reaction in which an element or fuel reacts rapidly with oxygen gas ($O_2$) to form an oxide while releasing heat and light.

Hydrocarbon

A chemical compound composed exclusively of bonded carbon and hydrogen atoms, expressed generically by the formula $C_xH_y$.

Incomplete combustion

A combustion reaction that occurs when oxygen is restricted, producing carbon dioxide ($CO_2$), water ($H_2O$), toxic carbon monoxide ($CO$), and solid carbon soot.

Neutralization reaction

A specialized double replacement reaction occurring between an acid and a base that produces neutral liquid water and an aqueous salt.

Acid

A compound that produces hydrogen ions ($H^+$) when dissolved in water, giving the solution a $pH < 7$.

Binary acid

An acid composed of hydrogen bonded to a single non-metal element, named using the prefix 'hydro-' and suffix '-ic acid' (e.g., $HCl(aq)$).

Oxyacid

An acid composed of hydrogen bonded to an oxygen-containing polyatomic ion, such as sulfuric acid ($H_2SO_4(aq)$) or carbonic acid ($H_2CO_3(aq)$).

Base

A compound that releases hydroxide ions ($OH^-$) when dissolved in water, usually containing hydroxide in its formula and yielding a $pH > 7$.

pH scale

A logarithmic scale ranging from $0$ to $14$ that indicates the relative concentration of hydrogen ions in a solution, where each unit step denotes a $10\text{-fold}$ change in acidity.