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4-3 Another Look at the Atom
Line Spectra
 A spectrum
that contains only certain colors, or
wavelengths, is called a line spectra.
 All elements emit light when vaporized, or
electricity passed through.
 Atoms absorb energy, then give it off in the form
of light.
 Each
element has a unique line spectra.
 Also referred to as emission spectra
Sample Emissions
The Bohr Model of Hydrogen Atom
 Why
do elements emit different wavelengths of
 Bohr
realized that the wavelengths had to do with
quantized energy proposed by Planck.
 Electrons in the atom are quantized
 Each orbital has different energies.
 When energy is absorbed electrons jump up in energy
levels, when released energy is given off as light
 Each
energy level was labeled by the quantum
number , n
n =1 was the lowest energy state
n= 2 a more excited state…..and so on.
 Using
Planck’s equation E = hv
 Calculated
 Matched for Hydrogen only
Bohr’s Model
His model was only able
to accurately predict for
Hydrogen with one
Matter Waves
 Planck
and Einstein described light as consisting of
photons – or quanta of energy.
 Light
travels as a wave
 Light interacts with matter as a particle
 Does
matter have a duel nature as well?
 De
Broglie referred to this as matter waves
Later scientists noticed
patterns in electrons that
had been reflected from
metals after being
Heisenberg Uncertainty Principle
 The
position and momentum of a moving object
can not simultaneously be measured and known
 Due
to the duel nature of matter and energy
 Only important with small scale objects
 For
example, This means that we cannot know for
sure where an electron is at any given time within
an atom.
We can only know the probability of finding an electron,
not its exact location.
 Orbital – a 3-dimensional region around the nucleus
that indicates the probable location of an electron.