Quantum Physics is already a very interesting subject, and so even though the presentation has all the required information to get yourself a hold on the subject, I would highly recommend everyone to do some extensive research. Well actually, there is no need for anyone to point out on the research part, you will automatically find yourselves filling the search history with some deep quantum-ish.

2. A General Note
 When you see formulae do not By heart, at least not all of them.
 Eg: Resistance= resistivity *length
 Here, R 𝛼 1
 which means that doubling the Cross-sectional area is like connecting
two identical resistors in parallel, their combined resistance being
“halved”.
 Throughout this lesson we’ll be dealing with terms like “Photons”
including “Protons”, so please don’t mix the words like I did once.
 After each topic we have to do the In-text questions, and so let’s bear
the pain together to achieve our GOAL at the end!
Cross-sectional Area
Cross-sectional Area

3. What are waves?
• They are just a way in which
energy is transferred from one
place to another.
• The characteristic properties of
waves are that they all show
reflection, diffraction and
interference.

4. Light
• Light is a wave, why? – it shows diffraction,reflection
and allthose topicsIGCSE wanted us to learnfor the
exams.
• Butnow whatif I tell you it alsobehaves as a particle?.
• It’s almostas ifI’m saying a smallballthrown at a slit
willdiffractthrough it.

5. How?
• Let’s get real scientific now.
• To see how light multitasks being a wave and a particle,
we need to get our Geiger counters ready.
• The Geiger counter detects ionizing radiation such as
alpha particles, beta particles and gamma rays using
the ionization effect.
• If you place a Geiger counternext to a source of gamma
radiation (electromagnetic), you will hear an irregular series
of clicks whichare indistinguishable from the clicks givenby
alpha & beta particles, whichare of course PARTICLES.

6. Photons
• Light could behave as a stream of
particles.
• These particles are called photons
and we believe that all
electromagnetic radiation consists of
“photons”.
• A photon is a ‘packet of energy’ or a
quantum of electromagnetic energy.

7. According to Albie (Albert
Einstein) who basically stole
some of the idea from Max
Planck (another German
physicist),
the energy E, of a photon in
Joules (of course) is related
to the frequency of the
electromagnetic radiation.

8. Photoelectric Effect
• In the photoelectric effect, light shines on a
metal surface and electrons are released from
it. But why?.
• A simple explanation is that light is a wave
that carries energy and this energy releases
electrons from the metal.
• But, detailed observations showed that there
is a minimum ‘Threshold frequency’ of light
below which no effect is observed.

9. Albie comes up again!
• In 1905, Albert Einstein came up with an
explanation of why weak ultraviolet radiation
could have an immediate effect on the
electrons in the metal, but very bright light
(high intensity) of ‘lower frequency’ had no
effect.

10. The success of Photon model
Observation WAVE model PHOTON model
There is an
instantaneous
electron Emission
Very intense light (high
number of photons)
should be needed
A single photon is
enough to release 1
electron.
Even weak light is
effective
Weak light waves
should not have any
effect
Weak light waves with
the threshold frequency
are effective
Increasing Intensity has
no effect on energies of
released electrons
Greater intensity means
electrons have more
energy
Greater intensity does
not mean more
energetic “photons”, so
electrons cannot have
more energy
A minimum threshold
frequency of light is
needed
Low-frequency light
should work
A photon in a low-
frequency light beam
has energy that is too
small to release an
electron

11. Line Spectra!
• From our previous knowledge of a line
spectra (product of dispersion of light),
we saw a beautiful array of continuous
spectrum of light.
• But now, Quantum mechanics does not
want to be left out, it wants to feel
equally loved and therefore it comes
with a new phenomenon called the
LINE SPECTRA.

12. From this………………

13. To this…………

14. Emission Line Spectra
• Quantum mechanics made the spectrum of light
more interesting with the help of Hot and Cool
gases.
• In Emission Spectra, only hot gases produce such
result.
• If you look at a lamp that contains a gas such as
neon or sodium, you will see that only certain colors
are present.
• Each element has a spectrum with a unique
collection of wavelengths.
• Astronomers use this phenomenon, can you deduce
where?

16. Absorption Line Spectra
• When light is passed through cool
gases……..what happens?
• After the light has passed through a
diffraction grating, the continuous white
light spectrum is found to have black lines
across it,WHAT!, yes.
• Here, certain wavelengths have been
absorbed as the white light passed through
these “Cool gases” – they are indeed cool eh?

21. Photon Energies!!!
• We now know that when an electron changes
its energy from one level 𝐸1 to another 𝐸2, it
either emits or absorbs a single photon.
• Recalling our first equation E = hf, let’s
form another equation.
hf = 𝑬 𝟏- 𝑬 𝟐, which is simply the
change in photon energies between the two
energy levels.

22. • Gas atoms that exert negligible electrical
forces on each other are known as isolated
atoms – they give relatively simple line
spectra.
• Similar spectra can be obtained from some
gemstones and colored gas.
• In a solid or liquid, the atoms are close
together.
• This makes energy level diagrams much more
complicated, with closely packed energy levels.

23.  Here, we can see the conduction and the valence
bands which are just bands of energy levels used
instead of individual energy levels.
 Band gaps which are also called Forbidden gaps are
shown in diagrams to just to tell us that electrons
cannot have energy values between the other 2
bands (i.e) – in between (quantised).

24. Louis de Broglie
• We know that Light has a
dual nature.
• So “Is it possible that
particles such as electrons
also have a dual nature”,
asked Louis de Broglie,
who later created history
with his convincing
results in this particle –
wave disaster.
• De Broglie imagined that
electrons would travel
through space as wave.
Where,
h = Planck constant
= de Broglie wavelength

25. Proof – Electron Diffraction
• In England, George
Thompson fired electrons
into thin sheets of metal
in a vacuum tube.
• This, along with many
other experiments done
by many other scientists
provided evidence that
electrons diffract,
confirming their wave-like
property.
Electron Diffraction tube

26. • The electron diffraction tube
consists of an electron gun
that accelerates electrons
towards a graphite foil.
• Onto this grid, a thin layer of
polycrystalline graphitised
carbon has been deposited by
vaporisation.
• This layer affects the
electrons in the beam much
like a diffraction grating
• The result of this diffraction is
seen in the form of an image
comprising two concentric
rings that become visible on
the fluorescent screen.
Electrons behaving like
particles would not cause a
diffraction picture when
passing a matter like the
graphite foil. Since a
diffraction picture gets
visible, there is diffraction –
electrons behave like waves.