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Bohr

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Quantum Mechanics. Through the Looking Glass. This is how the model of the atom ... c = where c =2.99 x 108 m/s. Sample Problem: The yellow light given off by a ... – PowerPoint PPT presentation

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Title: Bohr


1
Quantum Mechanics
Through the Looking Glass
2
This is how the model of the atom has developed
so far
3
Understanding Radiant Energy
c ?? where c 2.99 x 108 m/s
4
Sample Problem The yellow light given off by a
sodium lamp has a wavelength of 589 nm. What is
the frequency of this radiation?
c ??, where c 2.99 x 108 m/s
x ?
2.99 x 108 m/s 589 nm x
? 5.08 x 1014 s 1-
5
Plancks Theory Energy is released
incrementally as as individual packets of energy
called quanta where the change in energy of a
system is ?E h?, 2h?,n h? and h (planks
constant) 6.63 x 10-34 J-s
Sample Problem Calculate the smallest increment
of energy that an object can absorb from yellow
light whose wavelength is 589 nm
we know from the previous problem c ??, that ?
5.08 x 1014 s 1-
since ?E h? and h (planks constant) 6.63 x
10-34 J-s
?E (6.63 x 10-34 J-s )(5.08 x 1014 s 1- )
?E 3.37 x 1019 J
6
A Continuous Spectrum
7
Light is a form of ...
Electromagnetic Radiation
8
An Emission Spectrum...
is produced when a gas is placed under reduced
pressure...
...and a high voltage is applied
9
Balmers Description of the Emission Spectrum of
Hydrogen
-
where n 3, 4, 5, 6 and C 3.29 x 1015 s-1
? C
10
Bohrs Model of the Atom (1914)
Limited the path of electrons to circular orbits
with discrete energy (quantum energy levels)
Explained the emission spectrum of hydrogen
11
Radii and Energies of the Three Lowest Energy
orbits in the Bohr Model
0

En -RH
n 3
-0.242 x 10 -18 J
n 2
-0.545 x 10 -18 J
where RH 2.18 x 1018J
En -RH
n 1
-2.18 x 10 -18 J
o
0 A
o
o
0.53 A
2.12 A
4.77 A
radius n2 (5.3 x 10-11m)
12
Hydrogens Spectrum is Produced When
Electrons appear in excited state
electrons transfer from an excited state
Electrons are excited from their ground state
Electrons return to their ground state
13
Pashen Series
  • Infrared

Balmer Series
  • Visible and Ultraviolet

Lyman Series
  • Ultraviolet

14
Explaining the Emission Spectrum of Hydrogen
since ?E E f - E i
-
then ?E
-RH
-

15
Sample Problem Calculate the wavelength of
light that corresponds to the transition of the
electron from the n 4 to the n2 state of the
hydrogen atom.
-
2.18 x 10-18J
?E
-4.09 x 10-19 J
?E
-4.09 x 10-19 J
? ?E

h
6.63 x 10-34 J-s
? 6.17 x 1014 s -1
? c
3.00 x 108 m/s
4.86 x 10-7 m 486 nm (green)
?
6.17 x 1014 s -1
16
ON TO PARTICLE WAVES
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