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# Heisenberg Uncertainty Principle

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Let's say you have a professional camera, and you want to take pictures of a tennis ball moving. If you began by taking pictures of the ball with a fast shutter speed, you could capture the ball without blur, allowing you to see its position. However, you would be unable to determine the ball's velocity. Conversely, if you try to capture the ball's velocity instead of its position, your photos will appear blurry, and you won't be able to tell the ball's position.

This is a simple analogy to Heisenberg's uncertainty principle, which states that we cannot know an object's position and velocity at the same time!

• First, we will look at an overview of some important concepts for understanding the Heisenberg uncertainty principle.
• Then, we will look at the definition of the Heisenberg uncertainty principle, and its formula.
• After, we will briefly look at the derivation of the Heisenberg uncertainty principle formula.
• Lastly, we will discuss its importance and solve a simple problem.

## Heisenberg Uncertainty Principle Overview

Before diving into the Heisenberg uncertainty principle, we need to review what energy levels are. We know that the structure of an atom consists of neutrons and protons in the atom's nucleus, and electrons "orbiting" the nucleus. These electron orbits are called energy levels, and the electrons in the outermost level are known as valence electrons.

An electron's possible location around a nucleus can be determined by its energy level.

For example, the Bohr model of the element calcium (Ca) shows 20 electrons arranged in four energy levels.

In the process of moving from a higher to a lower energy level (closer to the nucleus), an electron releases energy, emitting a photon.

But, how exactly does an electron behave? Does it behave like a wave or like quantum particles of energy? Well, it depends on which scientist you ask!

According to Louis de Broglie, matter possesses both particle and wave properties. de Broglie suggested that objects (such as electrons) can behave as though it moves in a wave. Louis de Broglie came up with the de Broglie wavelength formula to calculate the wavelength of matter. This formula relates the wavelength of a moving particle like an electron to its mass and velocity.

$$\lambda = \frac{h}{m\times v}$$

Where:

• $$\lambda$$ is equal to wavelength (in meters).
• $$h$$ is equal to planck's constant $$6.626\times 10^{-34}\text{ J}\cdot \text{s}$$.
• $$m$$ is equal to the mass of object (in kg).
• $$v$$ is equal to the velocity of the object (in m/s).

## Heisenberg Uncertainty Principle Definition

Later, in 1927, a German physicist called Werner Heisenberg proposed that it is not possible to know where exactly an electron is located when it behaves like a wave and what its velocity is simultaneously because by trying to take any measurements, we would be disturbing it in some way. So, he developed the Heisenberg uncertainty principle.

Let's look at the definition of the Heisenberg uncertainty principle.

The Heisenberg uncertainty principle states that it is impossible to know the momentum $$(mv)$$ and position ($$\text{x})$$ of an object (for example, an electron) simultaneously and with precision.

• The object's velocity is related to its wave nature, whereas the position of the object is related to its particle nature.

In simpler terms, Heisenberg suggested that objects (from electrons to a tennis balls) can be seen as particles or waves, but not both simultaneously!

## Heisenberg Uncertainty Principle Formula

The Heisenberg uncertainty principle formula is as follows:

$$\Delta\text{x}\cdot \Delta\text{p}\geqslant \frac{h}{4\pi}$$

Where,

• $$\Delta\text{x}$$ = uncertainty in the particle's position (in m).
• $$\Delta\text{p}$$ = uncertainty in momentum (in $$kg\cdot \frac{m}{s}$$).
• $$h$$ = Planck's constant $$(6.626\times 10^{-34}\text{ J}\cdot \text{s})$$

The equation to calculate the uncertainty in momentum, $$\Delta {\text {p}}$$ is: $$\Delta\text{p = }m\text{ }\times \text{ }\Delta v$$. Here, $$m$$ is the mass in kg and $$\Delta v$$ is the uncertainty in velocity (in m/s).

According to the Heisenberg uncertainty formula, the uncertainty in position times the uncertainty in momentum is greater than/equal to Planck's constant $$(h)$$ divided by four $$\pi$$.

According to this formula, the more accurately we know an object's position, the less accurately we can know its momentum (and vice versa). When talking about electrons, the uncertainty principle says that we cannot know the exact motion of an electron as it moves around the nucleus.

## Heisenberg Uncertainty Principle Derivation

Now that we know that the Heisenberg uncertainty principle is, let's look at how it was derived. The best way to explain Heisenberg uncertainty principle is by looking at a single slit diffraction experiment using an electron beam. In this experiment, electrons are allowed to pass through a slit, and because of the wave nature of these electrons, they spread out and create a diffraction pattern on a projected screen.

However, we can't know for sure where an electron will hit or land after it passed through the slit, only that will you be somewhere within the slit. This is where uncertainty in position $$(\Delta\text{x})$$ comes in. In this case, the uncertainty in position $$(\Delta\text{x})$$ = width of the slit, $$a$$.

Similarly, for the electron waves to spread out and produce a single slit diffraction pattern, electrons must have a horizontal velocity ($$v$$), and this velocity differs for each electron. Now, if we try to focus on finding the electron's exact position, then we create an uncertainty in their velocity ($$\Delta v$$).

In short, when the slit gets narrower, the uncertainty in position, $$\Delta\text{x}$$, of the electron is decreased, and the spot being projected on the screen starts to spread out. By decreasing $$\Delta\text{x}$$, we are increasing the uncertainty in momentum ($$\Delta\text{p}$$).

The simple derivation of the Heisenberg uncertainty principle is shown below. Here, scientists started with the equation for kinetic energy, where $$m$$ is the mass and $$v$$ is the velocity, and then by using dimensional analysis, they found out that energy (E) multiplied by time (t) is equal to momentum (p) times position (x).

Then, they noticed that $$\text{E }\times \text{t} = ℏ$$ (Planck's constant), and since kinetic energy (E) has a 1/2 factor, scientists divided  by 2, arriving to the uncertainty principle for momentum (p) and position (x):

$$\Delta\text{p }\Delta \text{x }\geqslant \frac{ ℏ}{2}$$.

$$\frac{ ℏ}{2}$$ is the same as $$\frac{h}{4 \pi}$$, making the heinsenberg uncertainty principle formula

$$\Delta\text{x}\cdot \Delta\text{p}\geqslant \frac{h}{4\pi}$$.

Fig. 3: Requested the same image.

There is another formula for Heisenberg uncertainty principle for simultaneous measurements of energy and time. In this formula, $$\Delta\text{E}\cdot \Delta\text{t}\geqslant \frac{h}{4\pi}$$, where, ΔE is the uncertainty in energy, and Δt is the uncertainty in time.

## Heisenberg Uncertainty Principle Importance

The importance of the Heisenberg uncertainty principle lies in that, together with the wave/particle duality, it helps indicate how different objects behave at microscopic levels.

Let's finish off by looking at an example of a problem involving Heisenberg uncertainty principle.

Suppose that you measured an electron's position to an accuracy of $$1.5\times 10^{-11}$$ meters. Calculate the electron's uncertainty in velocity ($$\Delta v$$).

This question gives us uncertainty in position ($$\Delta \text{x}$$), which is $$1.5\times 10^{-11}$$ meters, and asks us to find ($$\Delta v$$). Now, to find uncertainty in velocity, we first need to solve for uncertainty in momentum ($$\Delta \text{p}$$) and then use the formula to calculate $$\Delta v$$.

Step 1 - Solve for uncertainty in momentum ($$\Delta \text{p}$$).

$$\Delta\text{p}= \frac{h}{4\pi \cdot \Delta\text{x} }$$

$$\Delta\text{p}= \frac{6.626\times 10^{-34} \text{J}\cdot \text{s}}{4\pi (1.5\times 10^{-11}\text{ m)} }$$

$$\Delta\text{p}= 3.52\times 10^{-24}\text{ kg}\cdot\frac{\text{m}}{\text{s}}$$

Step 2- Solve for uncertainty in velocity ($$\Delta v$$) using $$\Delta \text{p}$$.

Remember that, the mass of an electron is $$9.11\times 10^{-31} \text{ kg}$$

$$\Delta\text{p}= m\times \Delta v$$

$$\Delta v =\frac{ \Delta\text{p}}{m}$$

$$\Delta v=\frac{3.52\times 10^{-24} \text{ kg}\cdot \text{m/s}}{9.11\times 10^{-31} \text{ kg}} = 3.86\times 10^{6}\text{ m/s}$$

Now, I hope that you were able to understand Heisenberg uncertainty principle a bit better!

## Heisenberg Uncertainty Principle - Key takeaways

• The Heisenberg uncertainty principle states that it is impossible to know the momentum $$(mv)$$ and position ($$\text{x})$$ of an object (for example, an electron) simultaneously and with precision.
• According to the Heisenberg uncertainty principle, the more accurately we know an object's position, the less accurately we can know its momentum (and vice versa).
• According to the Heisenberg uncertainty formula, the uncertainty in position times the uncertainty in momentum is greater than/equal to Planck's constant divided by four $$\pi$$.
• The general formula for the Heisenberg uncertainty principle is: $$\Delta\text{x}\cdot \Delta\text{p}\geqslant \frac{h}{4\pi}$$.

## References

1. Jackson, G. (2016, June 23). GM Jackson Physics and Mathematics: A Simple Way to Derive the Heisenberg Uncertainty Principle. GM Jackson Physics and Mathematics. http://gmjacksonphysics.blogspot.com/2016/06/here-is-simple-way-to-derive-heisenberg.html
2. Openstax. (2012b). College Physics. Openstax College.
3. Randall Dewey Knight, Jones, B., & Field, S. (2019). College physics : a strategic approach. Pearson.
4. Swanson, J. (2021). Everything you need to ace chemistry in one big fat notebook. Workman.

Heisenberg's uncertainty principle was derived from the relationship between the wave and particle nature of objects.

Heisenberg's uncertainty principle states that the more accurately we know an object's position, the less accurately we can know its position (and vice versa).

An example of the Heisenberg uncertainty principle can be seen in a single slit diffraction experiment using electron beams.

Heisenberg's uncertainty principle implies that particles/objects have no definite pathway or location.

According to Heisenberg uncertainty principle, we cannot know the exact motion of an electron as it moves around the nucleus.

## Heisenberg Uncertainty Principle Quiz - Teste dein Wissen

Question

An electron's possible location around a nucleus can be determined by its  ______

energy level

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Question

Electrons in the outermost level are known as _______.

valence electrons

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Question

In the process of moving from a higher to a lower energy level (closer to the nucleus), an electron _____ energy, emitting a photon.

releases

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Question

True or false: according to Louis de Broglie, matter possesses both particle and wave properties.

True

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Question

The ______  states that it is impossible to know the momentum and position of an object at the same time.

Heisenberg uncertainty principle

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Question

In Heisenberg's uncertainty principle, The object's velocity is related to its ____ nature.

wave

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Question

In Heisenberg's uncertainty principle, the position of the object is related to its ____ nature.

particle

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Question

The Heisenberg uncertainty principle tells us that the more accurately we know an object's position, the  _____ accurately we can know its momentum (and vice versa).

less

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Question

According to the ______, the uncertainty in position times the uncertainty in momentum is greater than/equal to Planck's constant divided by four π.

Heisenberg uncertainty formula

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Question

What are the steps to find an electron's uncertainty in velocity, given the electron's uncertainty in position.

1. Solve for uncertainty in momentum using Heisenberg's uncertainty formula

2. Solve for uncertainty in velocity using the general formula relating uncertainty in momentum, mass and velocity.

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Question

Who proposed Heisenberg's uncertainty principle?

Werner Heinsenberg

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