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Transcript
Development of Quantum Mechanics
Bohr’s Contribution
AP Chemistry
by
Diane Paskowski
Questions to Consider
 Why do the different chemicals give us different
colors?
 Why do we get colors at all?
7.1
Atomic Spectrum of Hydrogen
 Continuous spectrum – contains all the
wavelengths of visible light
 Line spectrum – each line corresponds to a discrete
wavelength:
 Hydrogen emission spectrum
7.3
Significance?
 Only certain energies are allowed for the
electron in the hydrogen atom.
 Energy of the electron in the hydrogen atom
is quantized.
7.3
Bohr Model
 Electron in a hydrogen atom moves around the nucleus only in
certain allowed circular orbits.
ΔE = -2.178×10-18J[(1/nfinal2)-(1/ninitial2)]
Where n is the energy level
(principal quantum number)
7.4
Electronic Transitions in the Bohr Model for the
Hydrogen Atom
7.4
Figure 7.7 A Change Between Two Discrete
Energy Levels Emits a Photon of Light
Line Spectrum Of Hydrogen
 http://www.mhhe.com/physsci/chemistry/essentialchemis
try/flash/linesp16.swf
Bohr Model
 Bohr’s model is
fundamentally incorrect. This
model only works for
hydrogen.
 Electrons do not move around
the nucleus in circular orbits.
7.4