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Matter
Anything that has mass and occupies space.
Property
Any characteristic that allows us to recognize a particular type of matter and to distinguish it from other types.
Molecules
Two or more atoms that are joined together in specific shapes.
Gas
Has no fixed volume or shape; conforms to the volume and shape of its container.
Liquid
Has a distinct volume independent of its container but has no specific shape. Cannot be compressed.
Solid
Has both a definite shape and a definite volume. Cannot be compressed.
Pure Substance
Matter that has distinct properties and a composition that does not vary from sample to sample.
Ex. Water and Table Salt.
Elements
Substances which cannot be decomposed into simpler substances. On a molecular, each is composed of only one kind of atom.
118 are known.
Compounds
Substances composed of two or more elements; they contain two or more kinds of atoms. Composition is fixed.
Ex. Water (H₂0)
Mixture
Combinations of two or more substances in which each substance retains its chemical identity. Composition can vary.
Physical Properties
Properties that can be observed without changing the identity and composition of the substance.
Ex: color, odor, density, melting point, boiling point, hardness.
Chemical Properties
Properties which describe the way a substance may change, or *react* to form other substances.
Ex: flammability
Intensive Properties
Properties that do not depend on the amount of sample being examined and are particularly useful in chemistry because many intensive properties can be used to *identify* substances.
Extensive Properties
Properties that depend on the amount of sample. They relate to the amount of substance present.
Ex: Mass and Volume.
Physical Change
A change in the physical appearance but not the composition of the substance. It remains the same substance before and after the change.
Ex: The Evaporation of water.
Chemical Change/Chemical Reaction
A change in which a substance is transformed into a chemically different substance.
Ex: when Hydrogen burns in air, it combines with oxygen to form H₂0
SI Prefix: Giga
SI Meaning: 10⁹
SI Prefix: Mega
SI Meaning: 10⁶
SI Prefix: Kilo
SI Meaning: 10³
SI Prefix: Deci
SI Meaning: 10⁻¹
SI Prefix: Centi
SI Meaning: 10⁻²
SI Prefix: Milli
SI Meaning: 10⁻³
SI Prefix: Micro
SI Meaning: 10⁻⁶
SI Prefix: Nano
SI Meaning: 10⁻⁹
Mass
The measure of the amount of material in an object.
Volume x Density
Temperature
A measure of the hotness or coldness of an object. A physical property that determines the direction of heat flow. Heat always flows spontaneously from a substance at a higher temperature to one at a lower temperature.
Kelvin to Celsius
K= °C + 273.15
Fahrenheit to Celsius
°F = 9/5 (°C) + 32
Celsius to Fahrenheit
°C = 5/9 (°F - 32)
Volume
(length)³
Mass/ Density
Speed
m/s
Density
Mass / Volume
Exact Numbers
A quantity that doesn't need measure.
Ex: Number of people in Chemistry class
Inexact Numbers
If the number has been measured.
Ex: Mass of a penny
Precision
A measure of how closely individual measurements agree with one another.
Accuracy
Refers to how closely individual measurements agree with the correct value.
Significant Figures
The numbers of a measurement that are reasonable to report.
All digits of measured quantity, including the uncertain one.
