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AP chem chapter 7

Hund's rule Every orbital in a subshell is occupied with only one electron before the electrons can be paired.
Aufbau Principle electrons fill lower levels before filling the higher levels. ex: 1s before 2s
Heisenberg uncertainty principle the more precisely one property is measured, the less precisely the other can be controlled, determined, or known.
Pauli exclusion principle an orbital can only hold up to two electrons. the two electrons must have opposite spins. Therefore, no two electrons in the same atom can have the same 4 Quantom numbers.
Absorption and emmision spectra the colors for each element. The lines that are left when the electron falls.
Quantized Energy can be gained or lost only in integer mulitples of hv.
photoelectric effect electrons are emitted from the surface of a metal when light strikes it.
line spectrum Hydrogen only, only certain energies are allowed for the electron in the hydrogen atom.
Quantum model the electron in a hydrogen atom, moves around the nucleus only in certain allowed circular orbits.
polyelectronic atoms atoms with more than one electron
core electrons inner electrons
Metals *shiny *ductile *good conductors of heat/energy
nonmetals *brittle *aborbs heat *dull
___has more protons than ____ and a greater inward pull... 1st explanation
___ has more energy levels than ___ and it's outer electrons are farter from the inward pull of the nucleus... 2nd explanation
Exception 1: S electrons sheild the P electrons from the inward pull
exception 2: paired up electrons have extra repulsion.
IE dips in what groups? 3 and 6
EA dips in what groups? 2 and 5
Created by: darci_k2013