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Science
Observation of the physical world.
Scientific Law
Generalization created from a large amount of related observations.
Hypothesis
Explanation of observations.
Scientific Theory
Explains underlying reasons for observations and laws.
Experiments
Controlled procedures designed to produce new observations.
Law of Conservation of Mass
Matter is neither created nor destroyed in a chemical reaction.
Law of Definite Proportions
All samples of a compound have the same proportions of constituent elements.
Law of Multiple Proportions
Masses of element B that combine with 1 g of element A can be expressed as a ratio of small whole numbers.
Dalton’s Atomic Theory
Elements are composed of indestructible particles called atoms.
Thomson’s Plum-Pudding Model
Electrons are small particles held within a positively charged sphere.
Rutherford’s Nuclear Model
Most of the atom's mass and positive charge are in the nucleus.
Chadwick
Discovered neutrons in the nucleus.
Protons
Positively charged particles in the nucleus.
Neutrons
Neutral particles in the nucleus.
Electrons
Negatively charged particles outside the nucleus.
Atomic Mass
Average mass of an element's isotopes.
Intensive Properties
Properties used to identify substances based on type (e.g., density).
Extensive Properties
Properties that depend on the amount of substance (e.g., mass).
Physical Properties
Properties displayed without changing composition (e.g., color, melting point).
Chemical Properties
Properties displayed by changing composition via a chemical change (e.g., flammability).
Law of Conservation of Energy
Energy is neither created nor destroyed.
Metric System
Standard system of measurement using SI units.
Prefix Multiplier
A factor used to convert between different units (e.g., Giga, Mega).
Significant Figures
Digits that carry meaning contributing to a number's precision.
Density
Mass per unit volume of a substance.
Mole Concept
1 mol = 6.022 × 10²³ particles.
Ionic Bonds
Form between metals and nonmetals, involving the transfer of electrons.
Covalent Bonds
Form between nonmetals, involving the sharing of electrons.
Empirical Formula
Shows the relative number of atoms of each element in a compound.
Molecular Formula
Shows the actual number of atoms of each element in a molecule.
Structural Formula
Represents covalent bonds and how atoms bond in a molecule.
Octet Rule
Atoms tend to bond in a way that gives them eight valence electrons.
Ball-and-Stick Model
A model representing molecular compounds and their structure.
Lattice Structure
Regular 3-D array formed by ionic compounds.
Formula Mass
The sum of the atomic masses of all atoms in a compound.
Composition of Compounds
The relative amounts of each element in a compound.
Determining Chemical Formula
Process of finding a chemical formula from experimental data.
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