Atomic Electron Shells and Energy Levels
Electron promoted
from heat energy
from the Bunsen
burner
Energy given out as
light as the electron
falls back to its
original position
We think of an atom like
this. Having electron
shells at equal distances
apart
If it was like this then
surely the lines in the
spectra would be equally
spread out.
The red is of lower energy
so would represent the
electron shell nearest the
nucleus
Rotate the spectra
The line emission spectra
tells us something different.
Each new line represents a
new electron shell. As you
move away from the
nucleus they get closer
together.
So the electron
shells must look
more like this
We can change the
diagram to make it
easier to see what is
going on in the atom
We only need to look at
one section of the atom:
We only need to look at
one section of the atom:
We can change the
diagram to make it
easier to see what is
going on in the atom
From here, we extend
the curves into straight
lines. This gives us a
chart called an energy
level diagram:
1
st
electron shell
2
nd
electron shell
3
rd
electron shell
4
th
electron shell
5
th
electron shell
Energy
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Energy
At GCSE you only filled the first 2
electron shells: 2.8. But if you
keep filling they can hold more
electrons (because they are
bigger). We will look at this in
more detail later.
2e
32e
18e
8e
To work out the number of electrons = 2n
2
Exploring how electrons move between energy levels in atoms, providing insights into electron shells and emission spectra. The progression from heat energy to light emission is visualized, shedding light on the arrangement of electron shells and the concept of energy level diagrams.
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Presentation Transcript
E E E E E E P s N s E E E E E
Electron promoted from heat energy from the Bunsen burner
Energy given out as light as the electron falls back to its original position
We think of an atom like this. Having electron shells at equal distances apart If it was like this then surely the lines in the spectra would be equally spread out.
The line emission spectra tells us something different. The red is of lower energy so would represent the electron shell nearest the nucleus Rotate the spectra Each new line represents a new electron shell. As you move away from the nucleus they get closer together.
So the electron shells must look more like this
We can change the diagram to make it easier to see what is going on in the atom We only need to look at one section of the atom:
We can change the diagram to make it easier to see what is going on in the atom We only need to look at one section of the atom: From here, we extend the curves into straight lines. This gives us a chart called an energy level diagram:
5th electron shell 4th electron shell 3rd electron shell 2nd electron shell 1st electron shell
5th electron shell 4th electron shell 3rd electron shell 2nd electron shell 1st electron shell
Energy 5th electron shell etc 4th electron shell n=4 n=3 3rd electron shell We call these diagrams energy level diagrams and each electron shell is now called The Principle Quantum Number, n 2nd electron shell n=2 1st electron shell n=1
Energy 5th electron shell 4th electron shell 32e 18e 3rd electron shell At GCSE you only filled the first 2 electron shells: 2.8. But if you keep filling they can hold more electrons (because they are bigger). We will look at this in more detail later. 2nd electron shell 8e 1st electron shell 2e To work out the number of electrons = 2n2
