Emission spectrum of H презентация

Содержание

1. Emission spectrum of H
2. Emission spectrum of H Light Bulb Hydrogen Lamp Quantized, not continuous
3. Emission spectrum of H We can use
4. e- can only have specific (quantized) energy
5. 1.Moving from higher to lower energy levels
6. Bohr’s Model of the Atom (1913) Electrons
7. Ephoton = ΔE = Ef - Ei

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

Слайд 1 Emission spectrum of H
“Continuous” spectrum
“Quantized” spectrum
使量子化
Any

ΔE is
possible

Only certain ΔE are
allowed

ΔE

Слайд 2Emission spectrum of H
Light Bulb
Hydrogen Lamp
Quantized, not continuous

Слайд 3Emission spectrum of H
We can use the emission spectrum to determine

the energy levels for the hydrogen atom.

Слайд 4e- 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)

Слайд 51.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

Слайд 6Bohr’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