hunds rule
within a sublevel, electrons fill orbitals one at a time before pairing
aufbau rule
electrons fill the lowest energy orbitals levels first
bohr model
energy of a photon depends on the difference in energy levels
quantum
the amount of energy needed to move from one energy level to another
are electrons particles or waves
both due to the quantum theory
orbital
defined as a region in space where there is a high probability (90 percent) of finding an electron
n=1
is the closest to the nucleus (low energy)
n=2
is further than n=1 (slightly more energy)
distance in energy levels and N
inversely proportional
as the distance in energy between energy levels..... N increases
decreases
each s orbital holds
2
each p orbital holds
6
each d orbital holds
10
each f orbital holds
14
hunds rule is also called
empty bus seat rule
ions..... electrons to become stable
gain or lose
how do we see light
energy levels come back down and move simultaneously through space
bohr model
he thought the electrons traveled in fixed orbits around the nucleus this isn't actually true
heisnburg/ quantum theory
he said it's impossible to see the velocity and position at the same time
pauli exclusion
no more than two electrons in an atom can copy the same orbitals
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