Emission spectrum of H презентация

Emission spectrum of H
Light Bulb
Hydrogen Lamp
Quantized, not continuous

Emission spectrum of H
We can use the emission spectrum to determine the energy levels for the hydrogen atom.

e- can only have specific (quantized) energy values.
light is emitted as e- moves from one energy level to a lower energy level.
n = principal quantum number (1,2,3,…)
-describe energy level
RH (Rydberg constant) = 2.18 x 10-18J
Bohr’s Model of the Atom (1913)
Z = atomic number (1 for H)

1.Moving from higher to
lower energy levels
emission of energy (e.g.
radiation as light)
2. Moving from lower to
higher energy levels
absorption of
energy (e.g. external
stimulation)
• Energy levels get closer together as n increases
• at n = infinity, E = 0

Bohr’s Model of the Atom (1913)
Electrons cannot have just any amount of energy but can have only certain specified amount; i.e. the energy of an electron is quantized. The specified energy values for an atom are called its energy levels.
As an electron moves instantaneously from one energy level to another, there are no intermediate stages.
Niels Henrik David Bohr was a Danish physicist who made foundational contributions to understanding atomic structure and quantum mechanics, for which he received the Nobel Prize in Physics in 1922.
http://www.youtube.com/watch?v=Ic8OnvRonb0

Ephoton = ΔE = Ef - Ei