Atomic Structure Flashcards
Refers to inability to know the momentum and position of a single electron simultaneously
Heisenberg Uncertainty Principle
An early attempt to describe the behavior of the single electron in a hydrogen atom
Bohr model
Describes a dense, positively charged nucleus
Rutherford model
Explains electrons fill empty orbitals before doubling up in the same orbital
Hund’s Rule
Explains no two electrons in an atom can possess the same four quantum numbers
Pauli Exclusion Principle
Explains electrons fill from lower to higher energy subshells
Aufbau Principle
Equal to number of protons found in an atom of an element
Atomic number (Z)
Sum of protons and neutrons, synonymous with atomic mass
Mass number (A)
Species of atom with differing number of neutrons
Isotopes
Weighted average of different naturally occurring isotopes
Atomic weight
Relation between energy, Planck’s constant, the speed of light, and wavelength
E = hc / λ
region of space around nucleus where electrons are localized and move rapidly
orbitals
Energy difference between energy levels, described by Planck
Quantum
Material consisting of atoms with unpaired electrons
Paramagnetic
Material consisting of atoms with all paired electrons
Diamagnetic
