Terminology Flashcards
Electronegativity
How much an atom ‘wants’ electrons relative to other atoms
Electron Affinity
The change in energy when one mole of electrons is added to one mole of atoms or ions in the gas phase
Fraunhofer lines
The dark lines in atomic emission spectrums (those light spectrum things)
Threshold frequency (v0)
Minimum energy needed to dislodge an electron as a photoelectron from a material
Work function (φ)
The minimum quantity of energy needed to emit photoelectrons (φ = h*c/ν0)
Rydberg equation
Predicts wavelengths of hydrogen atomic emissions where n is not 2
Heisenberg uncertainty principal
You can’t know where an electron is and its momentum
Node
Spaces between electron shells where there is 0 probability of finding the electron
Pauli exclusion principle
No two electrons in the same atom have the same set of quantum numbers
Effective Nuclear Charge (Zeff)
The magnetic energy exerted on valence electrons by the protons in the nucleus (increases with more protons, decreases with electron shielding)
Aufbau principle
Electrons always go to the lowest energy formation first (unless the species is excited)
Hund’s rule
The lowest energy electron configuration is with the lowest number of unpaired electrons
Ionization energy
the energy it takes to remove one moleof electrons from one mole of gas-phase atoms in their ground state
Isoelectronic
Species that have the same electron configuration
Coulombic attraction
When atoms are held together by electrostatic attraction (such as an anion and a cation being attracted to each other)
