Introductory Chemistry Lecture Notes Review

Vocabulary practice flashcards covering introductory chemistry concepts, including states of matter, atomic theory, physical and chemical properties/changes, subatomic particles, isotopes, ions, and chemical compounds.

Matter

Anything that has mass, occupies discrete space, and is affected by gravity.

Energy

Anything that is not matter, has no mass, and is not affected by gravity.

State of Matter

A general set of temporary behaviors of a substance that depends on relative temperature but not on the identity of the substance.

Gas State Density

A state of matter where particles are far apart and moving fast, resulting in a density that is approximately $1000$ times less dense than as a liquid or solid.

Sublimation

The state change in which a solid transforms directly into a gas, skipping the middle liquid state (e.g., dry ice / solid carbon dioxide, menthol cough drop).

Deposition

The state change in which a gas transforms directly into a solid, skipping the middle liquid state.

Physical Properties

General characteristics of a substance observed or measured by itself that are independent of the amount of matter present (e.g., color, texture, odor, taste, melting point, boiling point, density, intersolubility, conductivity, specific heat, molar mass).

Chemical Properties

A general description of how a substance does or does not react with other common substances such as $\text{O}_2$, $\text{H}_2\text{O}$, acids, or bases.

Pure Substance

Matter with constant composition and constant properties, where every particle is the same (e.g., water).

Mixture

Matter made from two or more pure substances mixed together, possessing variable composition and properties (e.g., salt water).

Atomic Number ($Z$)

The number of protons ($p^+$) in the nucleus of an atom.

Mass Number ($A$)

The total number of protons ($p^+$) and neutrons ($n^0$) in an atom's nucleus.

Isotopes

Atoms of the same element that have the same number of protons but different masses due to having different numbers of neutrons (e.g., Carbon-12, Carbon-13, Carbon-14).

Ion

A charged atom created by altering its number of electrons ($e^-$).

Cation

A positively charged ion created by removing electrons ($e^-$).

Anion

A negatively charged ion created by adding electrons ($e^-$).

Physical Change

Any change to matter that does not alter its chemical composition, meaning the underlying substance stays the same (e.g., state change, shape change, mixture).

Chemical Change

Any change to matter that alters its chemical composition to form a new substance, indicated by changes in color/odor/properties, state changes without temperature changes, or measured heat energy changes.

John Dalton's Atomic Theory

Theory stating that elements consist of tiny neutral particles called atoms, which are indivisible, indestructible, identical within an element, distinct between elements, bond in fixed ratios to form compounds, and rearrange during chemical reactions.

Electrostatic Forces

Forces of attraction between oppositely charged particles and forces of repulsion between particles carrying the same charge.

Electron ($e^-$)

A subatomic particle that orbits the nucleus, carries a $-1$ charge, and has a mass of $0.00065\,\text{amu}$.

Proton ($p^+$)

A subatomic particle located inside the nucleus that carries a $+1$ charge and a mass of $1\,\text{amu}$.

Neutron ($n^0$)

A subatomic particle located inside the nucleus that carries a charge of $0$ and a mass of $1\,\text{amu}$.

Compound

Matter in which each particle is made from atoms of two or more elements bonded together in a fixed ratio, possessing properties completely different from its constituent elements and capable of being broken down.

Atomic Mass Unit (amu)

The standard unit of mass for subatomic particles, where protons and neutrons each equal $1\,\text{amu}$ and electrons equal $0.00065\,\text{amu}$.