Electron Diffraction

Electron diffraction occurs when electrons interact with a regularly spaced structure, such as a crystal, and produce a diffraction pattern.

Diffraction is normally associated with waves. The discovery that electrons can diffract therefore provided powerful experimental evidence that matter has wave-like properties.

This supported Louis de Broglie's proposal that a particle with momentum p has an associated wavelength:

λ = h/p

where:

• λ = de Broglie wavelength
• h = Planck's constant
• p = particle momentum

Electron diffraction became one of the key experimental foundations of quantum mechanics.

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Why Electron Diffraction Was Surprising

In classical physics, electrons were normally regarded as:

particles

They have:

• mass
• electric charge
• momentum
• localized interactions

A classical particle travelling toward a crystal might be expected to scatter from individual atoms.

But experiments showed something remarkable:

electrons can produce diffraction and interference patterns

These are behaviours normally associated with:

waves

This demonstrated that the classical particle model was incomplete.

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de Broglie's Matter-Wave Hypothesis

In 1924, Louis de Broglie proposed that wave behaviour is not limited to light.

If photons can show both wave-like and particle-like behaviour, perhaps particles of matter can do the same.

He proposed:

λ = h/p

For a non-relativistic particle:

p = mv

so:

λ = h/mv

This wavelength is called the:

de Broglie wavelength

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Momentum and Wavelength

The de Broglie equation shows that wavelength is inversely proportional to momentum:

λ ∝ 1/p

Therefore:

greater momentum → shorter wavelength

and:

smaller momentum → longer wavelength

For electrons travelling at suitable speeds, the wavelength can be similar to the spacing between atoms in a crystal.

That makes diffraction observable.

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Worked Example: Electron Wavelength

Suppose an electron travels at:

v = 2.0 × 10⁶ m/s

Electron mass:

m = 9.11 × 10⁻³¹ kg

First calculate momentum:

p = mv

p = (9.11 × 10⁻³¹)(2.0 × 10⁶)

p = 1.82 × 10⁻²⁴ kg·m/s

Now use:

λ = h/p

λ = (6.63 × 10⁻³⁴)/(1.82 × 10⁻²⁴)

λ ≈ 3.64 × 10⁻¹⁰ m

This is approximately:

0.36 nm

This is comparable to atomic spacing in solids.

Therefore, electron diffraction can occur when electrons encounter a crystal.

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Why Crystals Produce Diffraction

A crystal contains atoms arranged in a regular repeating structure.

The distances between planes of atoms are extremely small—typically around the same scale as the wavelength of suitable electrons.

The regularly spaced atomic planes can therefore act somewhat like a:

three-dimensional diffraction grating

Electron waves scattered from different atomic planes can interfere.

Depending on their path difference, they undergo:

• constructive interference
• destructive interference

This produces the observed diffraction pattern.

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Constructive Interference

When scattered electron waves arrive:

in phase

their amplitudes reinforce one another.

This produces:

constructive interference

and a stronger detected electron signal.

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Destructive Interference

When electron waves arrive sufficiently out of phase, they partially or completely cancel.

This produces:

destructive interference

and a weaker detected signal.

Alternating regions of constructive and destructive interference produce the diffraction pattern.

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Bragg's Law

Diffraction from crystal planes can be described using:

nλ = 2d sinθ

where:

• n = diffraction order
• λ = wavelength
• d = spacing between crystal planes
• θ = Bragg angle

This is called:

Bragg's law

It was originally developed to describe X-ray diffraction by crystals.

Remarkably, it can also describe electron diffraction.

That similarity is strong evidence that electrons exhibit wave-like behaviour.

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Understanding Bragg Diffraction

Consider electron waves reflecting or scattering from two neighbouring crystal planes.

The wave reaching the deeper plane travels an extra distance.

For constructive interference, this extra path must equal a whole number of wavelengths:

path difference = nλ

Geometry gives the path difference:

2d sinθ

Therefore:

nλ = 2d sinθ

Only certain angles produce strong constructive interference.

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The Davisson-Germer Experiment

One of the most important demonstrations of electron diffraction was performed by:

Clinton Davisson and Lester Germer

in 1927.

Their experiment provided direct evidence for de Broglie's matter-wave hypothesis.

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Davisson-Germer Apparatus

The experiment used:

• an electron gun
• a heated filament
• an accelerating voltage
• a nickel crystal
• a movable electron detector
• a vacuum chamber

Electrons were accelerated toward the nickel crystal.

The detector measured how many electrons were scattered in different directions.

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Why a Vacuum Was Needed

Electrons can collide with molecules in air.

These unwanted collisions would:

• change electron direction
• change electron energy
• interfere with measurements

Therefore, the experiment was performed in a:

vacuum

This allowed electrons to travel from the electron gun to the crystal with minimal interference from gas molecules.

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Accelerating the Electrons

The electrons were accelerated through a potential difference.

An electron accelerated through voltage V gains kinetic energy:

KE = eV

where:

• e = elementary charge
• V = accelerating voltage

For non-relativistic electrons:

KE = 1/2 mv²

Therefore:

eV = 1/2 mv²

This allows the electron speed and momentum to be calculated.

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Electron Wavelength from Accelerating Voltage

Since:

p = mv

and:

eV = p²/(2m)

we obtain:

p = √(2meV)

Substituting into:

λ = h/p

gives:

λ = h/√(2meV)

This equation is useful for electrons accelerated through a known voltage.

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Effect of Increasing Voltage

From:

λ = h/√(2meV)

we see:

λ ∝ 1/√V

Therefore:

greater accelerating voltage → greater momentum → shorter wavelength

This changes the angles at which diffraction maxima occur.

That prediction can be tested experimentally.

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What Davisson and Germer Observed

If electrons behaved only as classical particles, scientists would expect a relatively smooth distribution of scattered electrons.

Instead, Davisson and Germer observed:

strong peaks at particular scattering angles

These peaks resembled diffraction maxima produced by waves.

The electrons were undergoing:

constructive interference

at particular angles.

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Comparing Prediction and Experiment

The crucial test was whether the wavelength inferred from the diffraction pattern agreed with:

de Broglie's prediction

Using the electron momentum:

λ = h/p

Using the crystal diffraction pattern:

nλ = 2d sinθ

The two methods gave closely matching wavelengths.

This agreement provided strong evidence that:

electrons have wave-like properties

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Why This Was So Important

de Broglie's proposal began as a theoretical hypothesis.

It predicted:

matter should have wavelength

Davisson and Germer provided experimental evidence consistent with that prediction.

This is an excellent example of how science develops:

theory → prediction → experiment → evidence

The experimental evidence supported the emerging theory of:

quantum mechanics

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Electron Diffraction Patterns

Electron diffraction patterns can appear as:

• spots
• rings
• bands

depending on the structure of the material and experimental arrangement.

A single crystal often produces an organized pattern of:

spots

A polycrystalline material containing many differently oriented small crystals often produces:

rings

The pattern contains information about the material's internal structure.

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Interpreting Bright Regions

A bright region or strong detector signal corresponds to:

many electrons arriving at that location

This occurs where the quantum amplitudes combine constructively.

Therefore:

bright region → constructive interference

A weak or dark region corresponds to much lower detection probability.

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What the Pattern Tells Us

The existence of a structured diffraction pattern tells us that the electrons are not behaving like simple classical particles travelling independently along fixed trajectories.

Instead, their behaviour depends on:

• wavelength
• interference
• crystal spacing
• diffraction angle

These are characteristic wave phenomena.

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Electron Diffraction and Probability

It is important not to imagine electrons simply spreading out as tiny pieces of matter.

When an electron is detected, it produces a:

localized detection event

This looks particle-like.

However, when many electrons are detected, their distribution forms a:

diffraction pattern

This is wave-like.

Quantum mechanics describes this using a:

wavefunction

The probability density for detecting the electron is related to:

|ψ|²

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One Electron at a Time

Diffraction and interference do not require many electrons to physically collide with one another.

Experiments can send particles through an apparatus at extremely low rates.

Each electron produces an individual localized detection.

Over time:

individual detections build up into an interference or diffraction pattern

This is one of the most striking examples of quantum behaviour.

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Electron Diffraction and Wave-Particle Duality

Electron diffraction demonstrates:

wave-like behaviour

Electron detection demonstrates:

particle-like behaviour

Therefore electrons exhibit:

wave-particle duality

They cannot be completely described as classical particles or classical waves.

Instead, they require a:

quantum mechanical description

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Comparing Electron and Light Diffraction

Light and electrons can both produce diffraction patterns.

The similarity provides powerful evidence that both radiation and matter have quantum wave properties.

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Light Diffraction

Light passing through a narrow slit spreads and produces a diffraction pattern.

For light:

larger wavelength → greater diffraction

The pattern results from interference between different parts of the wave.

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Electron Diffraction

For electrons, the same basic principle applies.

Electron waves encounter structures whose spacing is comparable to their wavelength.

The waves interfere.

This produces:

diffraction maxima and minima

The major difference is that electron wavelength is determined by:

momentum

through:

λ = h/p

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Light and Electron Similarities

Both light and electrons:

• produce interference
• produce diffraction
• have measurable wavelengths
• can be detected as individual localized events
• require quantum descriptions

This is a major part of:

wave-particle duality

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Light and Electron Differences

Photons and electrons are not identical.

Photon

• zero electric charge
• zero rest mass
• travels at c in vacuum
• electromagnetic quantum

Electron

• charge −e
• has rest mass
• travels below c
• lepton

Yet both can exhibit:

wave-like diffraction

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Diffraction Angle and Wavelength

From Bragg's law:

nλ = 2d sinθ

For fixed:

• n
• d

a larger wavelength requires a larger value of sinθ.

Therefore:

longer wavelength → larger diffraction angle

and:

shorter wavelength → smaller diffraction angle

This allows diffraction patterns to be used to determine wavelength.

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Effect of Electron Speed

For non-relativistic electrons:

λ = h/mv

If electron speed increases:

momentum increases

so:

wavelength decreases

Therefore:

faster electrons → shorter de Broglie wavelength

This changes the diffraction pattern.

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Worked Example: Doubling Momentum

Suppose an electron initially has:

λ = 0.20 nm

Its momentum is doubled.

Since:

λ = h/p

doubling p gives:

λ_new = λ/2

Therefore:

λ_new = 0.10 nm

The electron's matter wavelength is halved.

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Worked Example: Bragg Diffraction

Suppose electrons have wavelength:

λ = 0.10 nm

They diffract from crystal planes separated by:

d = 0.20 nm

For first-order diffraction:

n = 1

Use:

nλ = 2d sinθ

0.10 = 2(0.20)sinθ

0.10 = 0.40 sinθ

sinθ = 0.25

Therefore:

θ ≈ 14.5°

A strong diffraction maximum would occur at the corresponding Bragg angle.

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Worked Example: Finding Wavelength

Suppose first-order diffraction occurs at:

θ = 30°

and the crystal-plane spacing is:

d = 0.20 nm

Use:

nλ = 2d sinθ

λ = 2(0.20)(sin30°)

λ = 0.40 × 0.50

λ = 0.20 nm

The electron wavelength is therefore:

2.0 × 10⁻¹⁰ m

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Worked Example: Finding Momentum

An electron has wavelength:

λ = 2.0 × 10⁻¹⁰ m

Use:

p = h/λ

p = (6.63 × 10⁻³⁴)/(2.0 × 10⁻¹⁰)

p ≈ 3.32 × 10⁻²⁴ kg·m/s

This shows how diffraction measurements can provide information about particle momentum.

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Worked Example: Increasing Accelerating Voltage

Suppose the accelerating voltage increases by a factor of four.

Since:

λ ∝ 1/√V

then:

λ_new = λ_old/√4

λ_new = λ_old/2

Therefore:

quadrupling the accelerating voltage halves the electron wavelength

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Evidence and Scientific Interpretation

Suppose an experiment produces strong electron signals only at particular angles.

A scientist compares those angles with predictions from:

Bragg's law

and calculates a wavelength.

The scientist then independently calculates the electron wavelength using:

λ = h/p

If the two wavelengths agree within experimental uncertainty, this provides evidence supporting:

de Broglie's matter-wave theory

The strength of the evidence comes from agreement between independent theoretical predictions and experimental measurements.

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Why Random Scattering Is Not Enough

Simply observing electrons scatter from a crystal would not by itself prove wave behaviour.

Particles can scatter too.

The crucial evidence is the presence of:

organized diffraction maxima and minima

at angles predicted by wave-interference equations.

Therefore:

structured interference pattern → evidence for wave behaviour

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Diffraction and Crystal Structure

Electron diffraction works in both directions.

If the electron wavelength is known, the diffraction pattern can reveal:

crystal spacing

Using:

d = nλ/(2sinθ)

Scientists can determine distances between atomic planes.

Therefore, electron diffraction is not only evidence for quantum physics—it is also a powerful scientific tool.

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Electron Microscopy

Electron diffraction is closely related to:

electron microscopy

Because electron wavelengths can be much shorter than visible-light wavelengths, electron microscopes can investigate much smaller structures.

Applications include studying:

• crystals
• metals
• semiconductors
• nanoparticles
• biological structures
• defects in materials

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Transmission Electron Microscopy

A transmission electron microscope (TEM) sends high-energy electrons through a very thin sample.

Interactions between the electrons and the material can produce:

• high-resolution images
• diffraction patterns

Scientists can therefore investigate both:

structure and composition

at extremely small scales.

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Selected-Area Electron Diffraction

A technique called:

selected-area electron diffraction (SAED)

allows scientists to collect diffraction information from a small region of a material.

The pattern can reveal:

• crystal orientation
• crystal symmetry
• lattice spacing
• whether the material is crystalline or polycrystalline

This makes electron diffraction valuable in materials science and nanotechnology.

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Diffraction Patterns as Evidence

When interpreting electron diffraction evidence, ask:

Is there a regular pattern?

A regular arrangement of maxima and minima suggests interference.

Do the angles match wave predictions?

Agreement with Bragg's law supports wave behaviour.

Does the calculated wavelength match de Broglie's prediction?

Agreement with:

λ = h/p

supports matter-wave theory.

Does changing momentum change the pattern as predicted?

Increasing momentum should reduce wavelength.

If the diffraction angles change accordingly, this provides additional evidence.

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Classical Particle Prediction

Imagine electrons as tiny classical balls striking atoms in a crystal.

They might:

• bounce
• scatter
• change direction

But this model does not naturally predict the observed systematic:

interference maxima and minima

at particular angles.

Therefore, classical particle mechanics alone cannot adequately explain electron diffraction.

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Quantum Description

Quantum mechanics does not say an electron is simply a tiny classical wave.

Instead, its quantum state is represented by a:

wavefunction

The wavefunction evolves and can interfere.

Detection produces localized events.

Thus:

propagation and interference → wave-like

detection → particle-like

This is a more accurate interpretation of electron diffraction than saying that an electron literally changes from a particle into a classical wave.

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Connection to Atomic Physics

Electron wave behaviour is also important in atoms.

The wave nature of electrons helps explain why only certain quantum states are allowed.

In an early de Broglie interpretation of the Bohr model:

2πr = nλ

Only wavelengths that form appropriate standing-wave conditions around the nucleus are allowed.

Modern quantum mechanics replaces these fixed orbits with:

atomic orbitals

and:

wavefunctions

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Why Macroscopic Objects Do Not Obviously Diffract

The de Broglie equation applies to all matter:

λ = h/p

For a macroscopic object, momentum is enormous compared with that of an electron.

Therefore its wavelength is extraordinarily small.

For example, a 0.10 kg ball travelling at 10 m/s has:

p = mv

p = 1.0 kg·m/s

Therefore:

λ = 6.63 × 10⁻³⁴ / 1.0

λ = 6.63 × 10⁻³⁴ m

No ordinary crystal or slit has spacing small enough to reveal such a wavelength through observable diffraction.

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Why Electron Diffraction Matters

Electron diffraction was important because it demonstrated that:

matter has wave properties

This helped establish the broader concept of:

wave-particle duality

It also supported the emerging framework of:

quantum mechanics

The discovery fundamentally changed how scientists describe matter at microscopic scales.

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From Hypothesis to Application

The progression is remarkable:

de Broglie predicts matter waves

↓

Davisson-Germer observes electron diffraction

↓

quantum mechanics develops

↓

electron diffraction becomes a scientific tool

↓

electron microscopy and materials analysis

A discovery about the fundamental nature of matter became an important practical technology.

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Common Mistakes

Mistake: Saying electrons are only waves.
Electrons display both wave-like and particle-like behaviour and require a quantum description.

Mistake: Saying electrons physically become light waves during diffraction.
Electron matter waves are not electromagnetic waves.

Mistake: Saying electron diffraction proves electrons have no mass.
Electrons have mass; their wavelength is related to their momentum.

Mistake: Saying crystals create electron waves.
The electrons already have quantum wave properties; the crystal allows these properties to produce observable diffraction.

Mistake: Saying any random scattering proves wave behaviour.
The organized maxima and minima characteristic of diffraction provide the important evidence.

Mistake: Saying greater electron momentum produces a longer wavelength.
Correct: λ = h/p, so greater momentum produces a shorter wavelength.

Mistake: Saying higher accelerating voltage increases wavelength.
Higher voltage increases electron momentum and therefore decreases wavelength.

Mistake: Confusing electron diffraction with electron-electron collisions.
Diffraction results from the quantum interaction of electrons with a structured target.

Mistake: Saying Davisson and Germer invented matter-wave theory.
de Broglie proposed matter waves; Davisson and Germer provided important experimental evidence.

Mistake: Saying electron diffraction has no practical applications.
It is widely used in electron microscopy, crystallography, nanotechnology and materials science.

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Key Terms

Electron diffraction — formation of interference patterns when electrons interact with structures whose spacing is comparable to their de Broglie wavelength.

Matter wave — wave-like quantum behaviour associated with matter particles.

de Broglie wavelength — wavelength associated with a particle's momentum, λ = h/p.

Momentum — quantity related to a particle's motion; non-relativistically p = mv.

Davisson-Germer experiment — experiment that demonstrated electron diffraction from a nickel crystal.

Crystal lattice — regular repeating arrangement of particles within a crystalline solid.

Crystal plane — regularly arranged plane of atoms within a crystal.

Constructive interference — combination of wave amplitudes that produces an increased resultant amplitude.

Destructive interference — combination of wave amplitudes that reduces the resultant amplitude.

Bragg's law — diffraction condition nλ = 2d sinθ.

Diffraction maximum — direction in which constructive interference produces a strong detected signal.

Accelerating voltage — potential difference used to increase the kinetic energy of charged particles.

Wavefunction — mathematical description of a quantum state.

Wave-particle duality — principle that quantum objects can display both wave-like and particle-like properties.

Electron microscope — instrument using electron beams to investigate structures much smaller than those easily resolved using visible light.

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Key Takeaways

• Electron diffraction provides direct evidence for the wave-like behaviour of matter.
• de Broglie proposed that particles have wavelength λ = h/p.
• Greater particle momentum produces a shorter de Broglie wavelength.
• Electron wavelengths can be comparable to atomic spacing in crystals.
• Crystals can therefore produce electron diffraction.
• Diffraction results from constructive and destructive interference.
• Bragg's law is nλ = 2d sinθ.
• Davisson and Germer observed electron diffraction from a nickel crystal.
• Their measured wavelength agreed with the wavelength predicted by de Broglie's equation.
• This agreement provided strong experimental evidence for matter waves.
• Electrons are detected as localized particles but collectively produce wave-like diffraction patterns.
• Electron diffraction is therefore an important example of wave-particle duality.
• Electron diffraction and light diffraction both involve interference and wavelength.
• Light wavelength is associated with electromagnetic radiation, while electron wavelength is related to particle momentum.
• An electron accelerated through a potential difference gains kinetic energy KE = eV.
• For non-relativistic electrons, λ = h/√(2meV).
• Increasing accelerating voltage decreases electron wavelength.
• A regular diffraction pattern provides much stronger evidence for wave behaviour than random scattering.
• Diffraction patterns can be used to measure atomic spacing and investigate crystal structure.
• Electron diffraction has important applications in electron microscopy, materials science, nanotechnology and crystallography.
• Electron diffraction helped establish quantum mechanics as the correct framework for describing microscopic matter.

Check Your Understanding

1. What is electron diffraction?
2. Why was the discovery of electron diffraction surprising from a classical perspective?
3. State the de Broglie equation.
4. What happens to de Broglie wavelength when particle momentum increases?
5. Why are crystals suitable for demonstrating electron diffraction?
6. Explain the role of constructive interference in an electron diffraction pattern.
7. Explain the role of destructive interference.
8. State Bragg's law and identify each variable.
9. Describe the main features of the Davisson-Germer experiment.
10. Why was the Davisson-Germer experiment performed in a vacuum?
11. What did Davisson and Germer observe that indicated wave-like behaviour?
12. How did their results support de Broglie's matter-wave hypothesis?
13. An electron has momentum 3.0 × 10⁻²⁴ kg·m/s. Calculate its de Broglie wavelength using h = 6.63 × 10⁻³⁴ J·s.
14. Explain what happens to electron wavelength when accelerating voltage increases.
15. Compare electron diffraction with light diffraction.
16. Why does random scattering alone not provide strong evidence for matter waves?
17. Explain why individual electron detections appear particle-like while the overall diffraction pattern appears wave-like.
18. How can an electron diffraction pattern be used to determine crystal spacing?
19. Give two practical applications of electron diffraction.
20. Explain why electron diffraction was an important development in modern quantum physics.