Chemistry Fundamentals, Measurement, Properties, and Atomic Theory

A complete set of vocabulary flashcards derived from the lecture notes, covering physical states, measurement rules, conversion units, classification of matter, properties, mixtures, and basic atomic theory.

Solid (Diffusion Rate & Arrangement)

A state of matter in which particles (atoms, ions, or molecules) are close together, unable to move around freely, and have a slow diffusion rate of $10^{-20}\,m^2/s$.

Liquid (Diffusion Rate)

A state of matter whose particles diffuse at a faster rate than solids, with diffusion rates reaching up to $10^{-10}\,m^2/s$.

Gas (Diffusion Rate)

A state of matter with weak particle interactions that diffuses extremely fast, with diffusion rates reaching $10^3\,m^2/s$.

Covalent Bond

A chemical bond formed by the sharing of available valence electrons between two non-metals, or between a non-metal and a metalloid.

Molecular Decomposition Rule

The principle that the faster a molecule moves, the more it decomposes.

Significant Figures Zero Rules

Zeros to the left and right do not count as significant figures (e.g., $100$ has 1 sig fig; $0.0012$ has 2 sig figs), whereas zeros in the middle do count (e.g., $1.01$ has 3 sig figs).

SI Base Unit for Mass

The fundamental International System base unit used to measure mass, which is the kilogram ($kg$).

SI Base Unit for Temperature

The fundamental International System base unit used to measure temperature, which is Kelvin ($K$).

Accuracy

A measurement concept describing how closely a measured value is to its true value.

Precision

A measurement concept describing how consistent measured results are with one another.

Scientific Notation Rules

A notation system expressed as a value multiplied by $10^x$, where the decimal moves to the right if the exponent $x$ is positive, and to the left if negative (e.g., $3.21 \times 10^7$).

Density

The measure of how much mass is packed in a given space, given by the formula $d = \frac{\text{mass}}{\text{volume}}$ with units of $g/cm^3$ or $kg/m^3$.

Mass

The amount of matter inside an object.

Volume

The amount of space an object takes up.

Angstrom ($\text{\AA}$)

A unit of length defined as $1 \times 10^{-10}\,m$.

Dimensional Analysis

A methodology used in converting between units of measurement by multiplying the original measurement number by conversion ratios and dividing or multiplying to reach the target unit.

Matter

Anything that occupies space, has mass, and is made up of atoms.

Physical Change

A change in size, shape, phase, or state of a substance while its chemical structure stays the same, such as ice cream melting or dry ice disappearing.

Chemical Change

A change at the molecular level resulting in the creation of new molecules, indicated by signs such as color change, odor change, bubble formation, or heat and light release.

Extensive Properties

Properties that depend on sample size and change when the amount of substance changes, such as length, weight, volume, and mass.

Intensive Properties

Properties unique to specific compounds that are not affected by the amount of substance or sample size, such as temperature, density, and boiling point.

Pure Substance

A substance in which all molecules are identical and cannot be physically separated, such as pure elements or pure salt.

Homogeneous Mixture

A mixture where molecules blend in with one another at the atomic level without clustering, remaining translucent or transparent and allowing light to pass through.

Heterogeneous Mixture

A mixture containing non-dissolved clusters of molecules that block light, making the mixture opaque.

Neutron Formation (Atomic Theory)

The phenomenon where protons and electrons fuse under high pressure to make neutrons, which are unstable on their own until binding with a proton to become stable.