Transcript History of the Atom - Hazlet Township Public Schools

Electromagnetic Radiation
Gamma
X
ray
ray
Waves
UV Visible Infra
light
red
ROYGBIV
Micro
waves
Radio
TV
Wavelength: lambda (λ)-size of a wave (m, cm)
Frequency: nu (ν) - waves/sec (Hertz or hz)
Speed of light: c; c= wavelength x frequency
c= λ x ν = 3.00 x 10 8 m/s
Duality: light shows wave and particle behavior
Planck equation:
A) E = h x ν
E: energy
ν :frequency
h: Plank’s constant = 6.626 x10-34 Js
B) E= hc / λ
Light Emissions:
Ground State: e- at the lowest energy level
when electrons absorb energy, then go to
higher shells to become an excited atom.
Ground + Energy
Exited atom
absorbed
Excited
Ground + Energy given off
Emitted Energy: specific wave length
Lyman
Balmer
Paschen
UV
Visible
Infra Red
BLS ( Bright Line Spectra):
Each element has an unique BLS (atomic
finger print of an element)
The Bohr Model: only applied to Hydrogen
e- move in shells, add energy, they move to a
higher energy level.
Spectroscopy: an instrument that separates light
into a spectrum which can be examined.
Quantum Model: modern atomic theory which
states electrons carry with a certain energy
(the quantization of e- energy).
L. DeBroglie: electrons might also have waveparticle nature
E. Schrodinger: devised equation that treated emoving around nuclei as laid the foundation of
modern quantum waves theory
W. Heisenberg: “Uncertainty Principle” not possible to measure precisely both velocity
and position of an electron at the same time