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ch. 13 chem


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quantum mechanics equations
allows scientists to determine the probability of finding particles in certain places
kernal electrons
innershell electrons and nucleus
valence electrons
outershell electrons involved with bonding
classical mechanics
laws of motion developed by isaac newton that apply to macroscopic world as well as atoms and molecules
hund's rule(stinky bus rule)
before any second electron can be placed in a sub level, all the orbitals of that sub level must contain at least one electron
energy levels
principle 1-7 sub level s,p,d,f
its impossible to know both the speed and location of an electron at the same time
specific orbital - m
aufbau principle
electrons must fill lower energy levels before entering higher level
electron configuration
a representation of the arrangement of electrons in an atom
max number of valence electrons
8- noble gases
de Broglie and Planck
advance the theories of wave mechanics
pauli exclusion principle
electrons occupying the same orbital must have opposite spin
direction of spin - s
Cr, Mo, Ag, Au, Cu, W
exceptions to the aufbau principle
energy sublevel - l
einstein's theory of relativity
shows Newton's equations dont work when objects approach the speed of light
creates the uncertainty principle
lewis dot diagram
orbital notation
another way to represent arrangement in atoms
energy level - n
wave mechanics
developed to help Bohr's theory

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