Heisenberg uncertainty principle
The Heisenberg uncertainty principle states that there is a limit to how precisely certain pairs of physical properties of a particle can be known simultaneously. Explore the Heisenberg uncertainty principle by calculating uncertainty in position given the uncertainty in momentum for Bohr model of hydrogen. Created by Jay.
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- Does light have mas? Doesn't the dibroglie equation show that it does?(23 votes)
- No, the De Broglie equation shows that matter can behave like a wave. Light has no rest mass, but it does have momentum and energy. Using Einstein's full equation, E² = p²c² + m²c⁴, with a m (rest mass) = 0, we see that for light, E = pc. So, with momentum, De Broglie's equation still applies to light without the need for mass. λ = ɦ/p(83 votes)
- at0:29jay said if we know the position of particle in space we cant find out momentum of that particle my question is why we cant find out the momentum of that particle if we know the position?(11 votes)
- That's not exactly right. Every matter in the universe act as waves and particles, matter has a dual nature wave-particle. However, the smaller the mass, the most significant is wave behavior. I, as a person, have a wave behavior, BUT you cannot see it as my rest mass is big enough to make my wave behavior insignificant to your eyes, and a planet has even more rest mass and it's even more difficult to detect it's wave behavior. So when the mass of a particle is higher, it's more uncertain to predict it's wave aspects (wavelenght, amplitude, frequency), than it's to predict it's particle aspects (position, velocity, momentum). When the rest mass is lower, tending to zero, it's easier to predict wave it's wave behavior than it's to predict it's particle behavior. That's why we have a uncertainty principle regarding MOMENTUM and POSITION when talking about ATOMIC PARTICLES.(33 votes)
- How can one cite a Khan video such as this? Is it academically advisable to do so?
I am doing a biographical report on Heisenberg; I wish to cite this as background information in the report, and to quote directly.(11 votes)
- You should always cite your sources when you quote directly.
Here's one possible format:
Author name. Video name. Publisher name. Year of publication. Media source. Date of access.
Khan Academy. "Heisenberg Uncertainty Principle". N.p., 2016. Web. 24 Jan. 2016.
"N.p." means "No publisher".
Follow the punctuation exactly. Just change the 24 Jan. 2016 to the date you accessed the site.(26 votes)
- How do we know the uncertainty in the velocity of the particle??(18 votes)
- The 10% uncertainty was just made up to illustrate a calculation.
The point is this: The Bohr model assumes that the radius and velocity of the electron can theoretically be known with no uncertainty (like in classical physics). Later, it was found that there is a fundamental limit to precision in quantum mechanics, so Bohr's model can't be the whole picture.(6 votes)
- At8:13Jay says that the Bohr model is incorrect. Is this because the Uncertainty Principle showed that the position of the electron would be at a distance greater than 2 times the radius. Whereas the Bohr model had the position of the electron at r1?(4 votes)
- The Bohr model could not be correct because it only worked for H and even for H it did not properly explain all the observations about the emission spectrum of H. That's why physicists continued to search for a better model, and through the work of DeBroglie, Schrodinger, Heisenberg, Born and others, the modern model was developed.(6 votes)
- Is the mass of an electron moving in an orbit constant or not?? if yes, then why didn't heisenberg use velocity instead of momentum??(8 votes)
- As far as I understand, the formula is valid for any particle, not just electron. If we used velocity instead of momentum, we would have to exclude particles that have no mass, like photon.(1 vote)
- Okay now , a node is a region where one cannot find an electron . Assuming it is a p orbital , we can find a node at the center . So does that mean that an electron cannot pass through there ; ie ,does this mean to tell us that one can find one specific electron all the time in one specific "compartment" of the px, py or pz orbital?(5 votes)
- No, it just means that there is zero probability that you will ever locate the electron at that spot.
Electrons in an atom can go from one place to another without passing through the place in between.
That's why we think of them as probability clouds rather than little balls. Quantum objects just don't behave like the objects you are used to.(6 votes)
- At5:06, why do we multiply the equation by .1 when there is a 10% uncertainty? Don't quite see the reasoning or the logic behind doing this.(5 votes)
- Previously, he converted the 10% uncertainty into a decimal (.1), which is more suitable for the equation and easier to use on a calculator.(3 votes)
- Why did we take the 10% and not 45% for example or 90%.?(4 votes)
- Here, Jay assumed the uncertainty to be 10%. It can be anything.(5 votes)
- why exactly is it that there is no way of measuring both velocity and position of electron. cant we find some better method of measurement or instrument or something?(1 vote)
- It isn't so much that we cannot measure both momentum (and it is momentum, not velocity) and position of an electron at the same time, but rather there is a limit placed by nature on how precisely we may simultaneously measure both.
Any mechanism by which we might measure the electron's momentum will affect the position, making the position less certain. Likewise, any mechanism by which we might measure the electron's position will affect its momentum, making the momentum less certain. This is known as the observer effect.
Thus, while we can refine instruments to some extent, it is utterly impossible to construct any instrument that would overcome this problem. This is a limit imposed by nature and it can never be overcome as far as we know with current understanding of nature.
However, it goes deeper than that. Completely apart from any measurement anyone might make, the more set the momentum becomes the less the particle even HAS a set location. Likewise, the more set the position becomes the less set the momentum of the particle actually is. So, it is not MERELY a matter of our not being able to measure with arbitrary precision, but that the particle itself does not HAVE an exact momentum nor an exact location within very specific rules. The rule is that the product of the uncertainties of the position and momentum cannot be less than h/(4π) = 5.27286×10⁻³⁵ J∙s (h is the Planck constant).(7 votes)
- Heisenberg uncertainty principle is a principle of quantum mechanics. And so if we take a particle, let's say we have a particle here of Mass M, moving with Velocity V, the momentum of that particle, the linear momentum is equal to the Mass times the Velocity. And according to the uncertainty principle, you can't know the position and momentum of that particle accurately, at the same time. So if you know the position, if you know where that particle is in space really well, you don't know the momentum, or you don't know the velocity of that particle, and vice versa. If you know the momentum really well, you don't know the position. So let's look at a mathematical description of the uncertainty principle. So the uncertainty in the position, so Delta X is the uncertainty in the position, times the uncertainty in the momentum, so Delta P is uncertainty in momentum, the product of these two must be greater than or equal to some constant. And that constant is Planck's Constant: h divided by four pi. So we have a constant divided by another constant. So this just gives us a number on the right side, and you might see something a little bit different in another textbook. It doesn't really matter that much, it just depends on how you define things. So the point is, the product of the two uncertainties must be greater than or equal to some number. So the uncertainties are inversely proportional to each other: if you increase one, you decrease the other. Let's go ahead and use some really simple numbers here, just so you can understand that point. So let's say, and this is just extremely simplified, so let's just see if we can understand that idea of inversely proportional. So if you have an uncertainty of two for the position, and let's say you had an uncertainty of two for the momentum. Alright, so two times two is equal to four, so I won't even worry about greater than, I'll just put equal to here. So if two times two is equal to four. If I decrease the uncertainty of the position, so I decrease it to one, so the uncertainty in the momentum must increase to four, because one times four is equal to four. If I decrease the uncertainty in the position even more, so if I lower that to point five, I increase the uncertainty in the momentum, that must go up to eight. So point five times eight gives us four. And so, what I'm trying to show you here, is as you decrease the uncertainty in the position, you increase the uncertainty in the momentum. So another way of saying that is, the more accurately you know the position of a particle, the less accurately you know the momentum of that particle. And that's the idea of the uncertainty principle. And so let's apply this uncertainty principle to the Bohr model of the hydrogen atom. So let's look at a picture of the Bohr model of the hydrogen atom. Alright, we know our negatively charged electron orbits the nucleus, like a planet around the sun. And, let's say the electron is going this direction, so there is a velocity associated with that electron, so there is velocity going in that direction. Alright, the reason why the Bohr model is useful, is because it allows us to understand things like quantized energy levels. And we talked about the radius for the electron, so if there's a circle here, there's a radius for an electron in the ground state, this would be the radius of the first energy level, is equal to 5.3 times 10 to the negative 11 meters. So if we wanted to know the diameter of that circle, we could just multiply the radius by two. So two times that number would be equal to 1.06 times 10 to the negative 10 meters. And this is just a rough estimate of the size of the hydrogen atom using the Bohr model, with an electron in the ground state. Alright, we also did some calculations to figure out the velocity. So the velocity of an electron in the ground state of a hydrogen atom using the Bohr model, we calculated that to be 2.2 times 10 to the six meters per second. And since we know the mass of an electron, we can actually calculate the linear momentum. So the linear momentum P is equal to the mass times the velocity. Let's say we knew the velocity with a 10% uncertainty associated with that number. So a 10% uncertainty. If we convert that to a decimal, we just divide 10 by 100, so we get 10% is equal to point one. So we have point one here. If I want to know the uncertainty of the momentum of that electron, so the uncertainty in the momentum of that particle, momentum is equal to mass times velocity. If there's a 10% uncertainty associated with the velocity, we need to multiply this by point one. So let's go ahead and do that. So we would have the mass of the electron is 9.11 times 10 to the negative 31st. The velocity of the electron is 2.2 times 10 to the sixth, and we know that with 10% uncertainty, so we need to multiply all of that by point one. So let's go ahead and do that. We're gonna multiply all those things together. So we take the mass of an electron, 9.11 times 10 to the negative 31st and we multiply that by the velocity, 2.2 times 10 to the sixth, and we know there's a 10% uncertainty associated with the velocity, so we get an uncertainty in the momentum 2.0 times 10 to the negative 25. So the uncertainty in the momentum is 2.0 times 10 to the negative 25. And the units would be, this is the mass in kilograms, and the velocity was in meters over seconds, so kilograms times meters per second. Alright, so this is the uncertainty associated with the momentum of our electrons. Let's plug it in to our uncertainty principle here: we had the uncertainty in the position of the electron, times the uncertainty in the momentum of the electron must be greater than or equal to Planck's Constant divided by four pi. So we can take that uncertainty in the momentum and we can plug it in here. So now we have the uncertainty in the position of the electron in the ground state of the hydrogen atom times 2.0 times 10 to the negative 25. This product must be greater than or equal to, Planck's Constant is 6.626 times 10 to the negative 34. Alright, divide that by four pi. So we could solve for the uncertainty in the position. So, Delta X must be greater than or equal to, let's go ahead and do that math. So we have Planck's Constant, 6.626 times 10 to the negative 34, we divide that by 4, we need to divide that also by pi, and then we need to divide by the uncertainty in the momentum. So we also need to divide by the uncertainty in momentum, that's 2.0 times 10 to the negative 25, and that gives us 2.6 times 10 to the negative 10. So the uncertainty in the position must be greater than or equal to 2.6 times 10 to the negative 10 and if you worked our your units, you would get meters for this. So the uncertainty in the position must be greater than or equal to 2.6 times 10 to the negative 10 meters. Let's go back up here to the picture of the hydrogen atom. 2.6 times 10 to the negative 10 meters, that's greater than the diameter of our hydrogen atom, so the uncertainty would be greater than this diameter. So the uncertainty in the position would be greater than the diameter of the hydrogen atom, using the Bohr model. So the Bohr model is wrong. It's telling us we know the electron is orbiting the nucleus at a certain radius, and it's moving at a certain velocity. The uncertainty principle says this isn't true. If we know the velocity fairly accurately, we don't know the position of the electron, the position of the electron is greater than the diameter, according to the Bohr model. So this just one reason why the Bohr model is wrong. But again, we keep the Bohr model around because it is useful as a simple model when you're just starting to get into chemistry. But this concept of the uncertainty principle goes against our natural intuitions. So our every day life doesn't really give us any experience with the uncertainty principle. For example, if we had a particle, let's make it a much bigger particle here, so a much bigger particle than an electron, so something that we can actually see in our real life, and so this has a much bigger mass, and moving with some velocity, logic tells us we can figure out pretty accurately where the position of that object is, and we can probably, pretty accurately, figure out the velocity, and so we know the momentum. And, that's true. We do know these things fairly accurately. But if you did a calculation using the uncertainty principle, so if you plugged in some different numbers, like if you increased the mass, so instead of 9.11 times 10 to the negative 31st, let's say you're using nine kilograms, and you plugged in some velocity here, and you solved for the uncertainty in the position, you're gonna get an uncertainty in the position that's extremely small. So you don't really notice those things on a macroscopic scale. You only notice them when you think about the atomic scale. And so that's why this isn't really an intuitive concept. Same idea with quantum mechanics: quantum mechanics is something that makes absolutely no sense when you first encounter it. You have no experience with quantum mechanics in your daily life, it just doesn't make any sense. You don't see these sorts of things. So this is just showing you an application at an atomic scale. Again, this is the uncertainty principle. We'll get more into quantum mechanics, and how quantum mechanics affects electrons and atoms in the next few videos.