Chapter 1 Notes - Chemistry Foundations

Vocabulary flashcards covering key concepts from the lecture notes.

Chemistry

The study of the composition, properties, and interactions of matter.

Central science

Chemistry’s role as a bridge connecting many STEM disciplines and natural phenomena.

Macroscopic domain

The domain of chemistry involving ordinary objects large enough to be seen or touched.

Microscopic domain

The domain of chemistry at the molecular/atomic level, often imagined rather than directly observed.

Symbolic domain

The domain that uses chemical symbols and formulas to represent matter.

Matter

Anything that occupies space and has mass.

Phases of matter

The common states: solid, liquid, gas; plus plasma as a fourth state.

Solid

A state of matter with a definite shape and volume.

Liquid

A state of matter that flows and takes the shape of its container, with a definite volume.

Gas

A state of matter that expands to fill both the shape and volume of its container.

Plasma

A high-energy, ionized gas containing charged particles; found in stars and lightning.

H2O

Chemical formula for water; exists in gaseous, liquid, and solid phases.

Mass

A measure of the amount of matter in an object; independent of location.

Weight

The force of gravity acting on an object; varies with gravitational field.

Law of conservation of matter

Total mass remains constant during physical or chemical changes.

Element

A pure substance that cannot be broken down into simpler substances by chemical changes; listed on the periodic table.

Atom

The smallest unit of an element that retains its properties.

Molecule

Two or more atoms bonded together.

Compound

A pure substance that can be broken down into simpler substances; composed of two or more elements bonded.

Mixture

A combination of two or more types of matter that can be separated by physical changes.

Homogeneous mixture

A mixture with uniform composition throughout; also called a solution.

Heterogeneous mixture

A mixture with nonuniform composition that varies by region.

Physical property

A property observed without changing the substance’s chemical identity (e.g., density, color, melting point).

Chemical property

A property describing how a substance changes its composition (e.g., flammability, reactivity).

Intensive property

Property that does not depend on the amount of material (e.g., density, temperature, boiling point).

Extensive property

Property that depends on the amount of material (e.g., mass, volume).

Physical change

A change in state or properties without changing chemical composition (e.g., melting, boiling).

Chemical change

A change that alters chemical composition; new substances form (e.g., rusting, combustion).

NFPA hazard diamond

A standard hazard symbol that summarizes the hazards of a chemical substance.

Periodic Table

Organization of elements by groups and periods; color codes indicate metal/metalloid/nonmetal and state of matter.

SI base units

The seven base units of the International System: meter, kilogram, second, kelvin, ampere, mole, candela.

Meter (m)

SI base unit of length.

Kilogram (kg)

SI base unit of mass.

Second (s)

SI base unit of time.

Kelvin (K)

SI base unit of temperature; absolute scale with zero at absolute zero.

Ampere (A)

SI base unit of electric current.

Mole (mol)

SI base unit of amount of substance.

Candela (cd)

SI base unit of luminous intensity.

SI prefixes

Prefixes (e.g., kilo, centi, milli) that indicate multiples or submultiples of base units.

Volume

Amount of space occupied; derived from length; base unit is m3; common units are L and mL.

Liter (L) and milliliter (mL)

Common volume units; 1 dm3 = 1 L; 1 cm3 = 1 mL.

Density

Mass per unit volume; common units are kg/m3, g/cm3, and g/L.

Dimensional analysis

Unit conversion method using conversion factors to cancel units.

Conversion factor

A ratio of two equivalent quantities expressed in different units.

Significant figures

Digits that carry measurement precision; rules govern how to report measurements.

Exact numbers

Numbers with unlimited significant figures (e.g., counting numbers, defined quantities).

Accuracy

Closeness of a measurement to the true value.

Precision

Reproducibility or repeatability of measurements.

Measurement uncertainty

Uncertainty in a measurement expressed as the estimate of the last significant digit.

Fahrenheit

Temperature scale; water freezes at 32°F and boils at 212°F.

Celsius

Temperature scale; water freezes at 0°C and boils at 100°C.

Kelvin temperature conversion

TK = TC + 273.15; Kelvin is the absolute temperature scale.