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Atomic Number
The number of protons in an atom.
Mass Number
The sum of the protons and neutrons in an atom.
Cation
A positively charged ion formed when an atom loses electrons.
Anion
A negatively charged ion formed when an atom gains electrons.
Isotope
Atoms of the same element with the same atomic number but different mass numbers.
Radio-isotope
An isotope that spontaneously decays to produce smaller nuclei and radiation.
Alpha Particle
A particle identical to a helium atom emitted during radioactive decay.
Beta Particle
Negatively charged particles emitted during radioactive decay, identical to electrons.
Ionizing Radiation
Radiation with enough energy to knock electrons out of atoms, damaging living tissue.
Non-Ionizing Radiation
Radiation that moves atoms in a molecule but does not remove electrons.
Ionic Bond
A bond formed by the complete transfer of electrons from a metal to a non-metal.
Covalent Bond
A bond formed by the sharing of electrons between non-metal atoms.
Molecule
Two or more non-metallic atoms bonded together.
Diatomic Molecules
Molecules consisting of two atoms, such as H2 or O2.
Valence Electrons
Electrons in the outermost shell of an atom.
Lewis Diagram
A representation that shows the valence electrons of an atom.
Octet Rule
The principle that atoms tend to bond in a way that gives them eight valence electrons.
Dipole-Dipole Force
Attractions between polar molecules due to their partial charges.
Hydrogen Bond
A strong dipole-dipole attraction between a hydrogen atom and nitrogen, oxygen, or fluorine.
London Dispersion Forces
Weak forces between non-polar molecules due to momentary dipoles.
High Specific Heat Capacity
The amount of heat energy required to raise the temperature of water, due to hydrogen bonding.
Green Chemistry
The design of chemical products and processes to reduce or eliminate the use and generation of hazardous substances.
