Chem 200 week 1 lecture 2 better

A set of vocabulary flashcards reviewing fundamental concepts, SI units, derived units, and uncertainty principles from Chapter 1 and Chapter 2 of Chem 200.

Physical Properties

Properties of a substance that may depend on its chemical structure and composition, but do not depend on chemical changes (e.g., hardness, density, color).

Chemical Properties

Properties associated with how the molecular structure of a substance actually changes during a chemical process (e.g., combustion, reaction with acids).

Physical Changes

Changes that alter a substance without affecting its underlying molecular structure, such as cutting in half, dissolving, or melting.

Chemical Changes

Processes that alter the molecular properties and structure of a substance, such as combustion or reacting with acids.

Intensive Property

A measured property that does not depend on the amount of material present, such as temperature, density, melting point, or boiling point.

Extensive Property

A measured property that is proportional to the amount of material present, such as volume or mass.

Conservation of Mass

The principle that in any physical or chemical process, total mass is conserved, meaning the initial mass equals the total mass at the end of the process.

Base SI Units

The standard foundational units of the System Internationale, including the kilogram, meter, second, mole, and Kelvin.

Kilogram

The base SI unit for mass, abbreviated as $\text{kg}$.

Meter

The base SI unit for distance, abbreviated as $\text{m}$.

Second

The base SI unit for time, abbreviated as $\text{s}$.

Mole

The base SI unit for the amount of material, defined by Avogadro's number as $6 \times 10^{23}\,\text{per mole}$.

Kelvin

The base SI unit for temperature.

Ampere

The SI unit for electrical current, defined as $1\,\text{coulomb per second}$.

Candela

The SI unit of radiant intensity.

Derived SI Unit

An SI unit formed by combining base SI units through multiplication or division, such as acceleration in $\text{m/s}^2$.

Newton

The derived SI unit for force, equivalent to $\text{kg}\cdot\text{m/s}^2$.

Joule

The derived SI unit for energy, equivalent to force times distance, or $\text{kg}\cdot\text{m}^2/\text{s}^2$.

Liter

A non-SI metric unit of volume equal to $1\,\text{dm}^3$ or $0.1\,\text{m}$ cubed, which is $1000$ times smaller than a cubic meter.

Milliliter

A non-SI metric volume unit equal to $10^{-3}\,\text{liters}$, which is exactly identical to $1\,\text{cm}^3$.

Angstrom

A non-SI unit of distance equal to $10^{-10}\,\text{m}$, convenient for expressing chemical bond lengths.

Degree Celsius

A non-SI unit of temperature defined relative to the freezing point ($0\,^\circ\text{C}$) and boiling point ($100\,^\circ\text{C}$) of water.

Absolute Zero

Represented by $0\,\text{K}$, the theoretical state reached when all possible heat energy has been removed from a substance.

Ideal Gas Law

The relationship $PV = nRT$, in which temperature $T$ must be expressed in Kelvin ($\text{K}$) to yield correct calculations.

Accuracy

The degree to which an experimental measurement or result is close to the correct or true answer.

Precision

The degree to which repeated experimental measurements are reproducible under identical conditions.

Random Errors

Fundamental measurement variations that cannot be eliminated entirely but can be minimized by averaging repeated experiments.

Systematic Error

An experimental error resulting from flaws in the experimental design or setup, causing measurements to consistently deviate in a specific direction.

Significant Digits

A system used to track, communicate, and preserve the level of precision in measured and calculated values.