Chem- Module 1 Summary Cards

Chemistry?

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

Macroscopic domain

• Involves objects large enough to be seen and touched.

Solid

• A phase of matter with fixed shape and volume.

Atom

• The smallest particle of an element that can enter into a chemical combination.

Molecule

: A bonded collection of two or more atoms of the same or different elements.

Compound

A pure substance composed of two or more elements that can be broken down chemically.

Element

Back: A pure substance composed of only one type of atom that cannot be broken down chemically.

Front: Physical property

Back: A characteristic of matter not involving a change in chemical composition (e.g., color, boiling point).

Chemical property

Describes how matter changes into different matter (e.g., flammability, acidity).

Physical change

change in the state or properties of matter without altering its chemical composition

Chemical change

: A change that produces a different kind of matter from the original.

Extensive property

A property that depends on the amount of substance present (e.g., mass, volume).

Intensive property

A property that does not depend on the amount of substance (e.g., density, temperature)

Plasma

: A high-temperature, electrically charged state of matter.

Heterogeneous mixture

: A mixture where composition varies from point to point.

Homogeneous mixture (

A mixture with uniform composition throughout.

Pure substance

substance with constant composition; either an element or compound.

Mass

fundamental property indicating the amount of matter in an object.

Matter

Back: Anything that occupies space and has mass.

Volume

The amount of space an object occupies

Density

Mass divided by volume (D = M/V); shows how compact matter is.

Scientific method

A process involving observation, hypothesis, experiment, and theory/law development.

Theory

A well-tested explanation of natural phenomena.

SI units

International system of standard units (e.g., meter, kilogram, second).

Law

A statement summarizing repeated experimental observations.

Kelvin (K)

The SI unit of temperature; 0 K = -273.15 °C.

Celsius

(°emperature scale where water freezes at 0°C and boils at 100°C

Fahrenheit (°F)

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

T°C = (5/9) × (T°F − 32)

Converts Fahrenheit to Celsius

T°F = (9/5 × T°C) + 32

Converts Celsius to Fahrenheit.

T(K) = °C + 273.15

onverts Celsius to Kelvin

T°C = K − 273.15

Converts Kelvin to Celsius.

Cubic centimeter (cm³)

Back: Volume of a cube with 1 cm sides; equals 1 mL.

Front: Liter (L)

Back: A volume unit; 1 L = 1,000 cm³.

Front: Cubic meter (m³)

Back: SI unit of volume.

Front: Milliliter (mL)

Back: Equal to 1/1,000 of a liter or 1 cm³.

Front: Significant figures

Back: All measured digits including the uncertain last digit.

Front: Dimensional analysis

Back: A method for converting between units using conversion factors.

Front: Symbolic domain

Back: Chemical symbols and formulas used to represent substances.