Introduction to Chemistry and Properties of Matter

A complete set of vocabulary flashcards covering introductory chemistry concepts, including the scientific method, physical and chemical properties, energy, kinetic molecular theory, classification of matter, elements and compounds, and separation methods.

Hypothesis

An unproven prediction explaining how nature will behave.

Theory

A tested, refined, and expanded explanation of how nature works.

Law

A summary statement (e.g., a mathematical formula) that predicts cause and effect.

Matter

Anything that has volume and mass.

Extensive Properties

Properties that depend on how much matter you have, such as mass in grams, volume in liters, or electrical resistance.

Intensive Properties

Properties that do not depend on how much matter you have, such as melting point, boiling point, and density.

Physical Properties

Properties that describe physical changes (state or form) and characteristics, such as temperature, density, and opacity.

Chemical Properties

Properties that describe chemical changes where new substances are formed, such as reactivity, flammability, and toxicity.

Qualitative Properties

Properties that describe matter in ways without numbers, such as colour, state, and malleability.

Quantitative Properties

Properties that describe matter using numbers, such as melting point, density, and concentration.

Melting Point

The temperature at which a solid changes to a liquid, and vice-versa.

Boiling Point

The highest temperature at which a liquid can remain a liquid, or the lowest temperature a gas can remain a gas.

Heat of Fusion ($H_f$)

The amount of heat required to melt a substance at its melting point.

Heat of Vaporization ($H_v$)

The amount of heat required to evaporate a substance at its boiling point.

Physical Change

Anything done that affects a substance without changing its chemical identity (e.g., cutting, crumpling, mixing, or changes of state).

Reactivity

A chemical property describing if a substance reacts and its reaction rate, influenced by temperature, concentration, surface area, and catalysts.

Heat of Formation

The heat released when a substance is formed, such as water from hydrogen and oxygen ($2259\,J/g$).

Heat of Combustion

The heat released when a substance is combusted, such as methane reacting with oxygen ($54000\,J/g$).

Chemical Change

Anything that fundamentally changes the molecular structure or bonding within a molecule, indicated by formation of new materials, temperature changes, or colour changes.

Kinetic Energy

The energy of movement, measured in Joules ($J$).

Thermal Energy

An extensive property representing the total kinetic energy of a substance's particles.

Temperature

An intensive property representing the average kinetic energy of a substance's particles.

Heat

An amount of energy transferred between substances.

Pure Substance

A material with atoms that are chemically combined in a fixed ratio and only exhibits one set of properties.

Mixture

A material consisting of more than one pure substance that can be separated by physical means (e.g., filtering or distillation).

Element

A pure substance that cannot be decomposed, containing only one type of atom.

Compound

A pure substance of more than one type of atom that can be decomposed into elements.

Homogeneous Mixture

A mixture with small particles that appears to be the same throughout (e.g., orange juice).

Heterogeneous Mixture

A mixture with large particles that is easily differentiated (e.g., a bowl of cereal).

Solvent

The major component of a solution (e.g., water).

Solute

The minor component of a solution that has been dissolved into the solvent.

Aqueous Solution

A solution in which water is the solvent.

Metals

Elements found on the left side of the periodic table (~$80\%$ of elements) that are good conductors of heat and electricity, malleable, ductile, lustrous, and react with water to form bases.

Non-metals

Elements found on the right side of the periodic table that are poor conductors of heat and electricity and react with water to form acids.

Metalloids

Elements found along the 'staircase' in the periodic table (except aluminium) that exhibit properties of both metals and nonmetals.

Organic Compounds

Compounds containing carbon and hydrogen, along with other elements (often oxygen).

Inorganic Compounds

Compounds that do not contain carbon and hydrogen together (everything other than organic compounds).

Binary Compounds

Compounds containing only 2 different elements.

Non-binary Compounds

Compounds containing 3 or more different elements.

Ionic Compounds

Compounds containing positive and negative ions held together in large crystal lattices by attracting charges called ionic bonds.

Cations

Positive ions.

Anions

Negative ions.

Molecular Compounds

Nonmetals held together by sharing electrons called covalent bonds.

Acids

Ionic compounds containing $H^+$ ions.

Bases

Ionic compounds containing $OH^-$ ions.

Salts

All ionic compounds other than acids and bases.

Mechanical Separation

A separation technique based on size where large pieces are present and can be picked through using hands, sieves, or magnets.

Filtration

A separation technique based on size where solid pieces present in a liquid are pulled through a filter.

Gravity Separation

A separation technique based on density where solid pieces present in liquid float or sink apart via gravity using a density column or centrifuges.

Solvent Extraction

A separation technique based on dissolving where mixed solids and/or liquids are selectively dissolved into a solvent by washing it.

Chromatography

A separation technique based on dissolving where solids are dissolved and pulled through something 'sticky', separating based on speed.

Evaporation (Separation)

A separation technique based on energy where liquids evaporate away while solids remain.

Distillation

A separation technique based on energy where liquids with different boiling points are heated and evaporate in order.