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Modern Atomic Theory
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Gravity
Terms in this set (35)
wavelength
distance between two successive peaks in a wave
frequency
the number of wave peaks in a certain time interval
photon
a small packet of light
inverse
the relationship between wavelength and frequency of light
decreases
how energy of a photon changes when wavelength increases
Bohr model
electrons travel around the nucleus in fixed circular orbits
Heisenberg uncertainty principle
it is impossible to know both the momentum and position of an electron simultaneously
orbital
an region of space around an atom where an electron is likely to be found
principal quantum number
quantum number that determines the energy and size of an orbital
36
the maximum number of orbitals allowed in energy level 6
50
the maximum number of electrons allowed in energy level 5
0, 1, 2, 3, ...
allowed values for n
l
determines the shape of an orbital
0, ..., n-1
allowed values for l
s orbital
p orbital
d orbital
contains 3 orbitals
p sublevel
contains 5 orbitals
d sublevel
contains 7 orbitals
f sublevel
2
maximum number of electrons that can occupy an orbital
ground state
lowest energy arrangement of electrons in an atom
-l, ..., 0, ..., +l
allowed values for m
Pauli Exclusion Principle
electrons occupying the same orbital must have opposite spins
violates the Pauli Exclusion Principle
violates Hunds' rule
violates the Aufbau principle
Lewis dot diagram for a noble gas
noble gas notation for an alkali metal
valence electron
outermost electrons occupying s and p sublevels
emission spectrum
electrons transition from higher energy levels to lower energy levels, emitting photons
quantum mechanical model
the behavior of electrons in atoms is based on probability of finding electrons in a certain location
Aufbau filling sequence
2d
an orbital that is not allowed
1s2 2s2 2p5 4s1
an electron configuration for an excited state
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