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### Course: Physics library > Unit 17

Lesson 2: Atoms and electrons- De Broglie wavelength
- Quantum Wavefunction
- Atomic Energy Levels
- Bohr model radii (derivation using physics)
- Bohr model radii
- Bohr model energy levels (derivation using physics)
- Bohr model energy levels
- Absorption and emission
- Emission spectrum of hydrogen
- Bohr's model of hydrogen

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# Quantum Wavefunction

In this video David gives an introductory explanation of what the quantum wavefunction is, how to use it, and where it comes from.

## Want to join the conversation?

- Why is there an imaginary unit in Schrodinger's equation? What does that mean?(32 votes)
- nice question.

As I see it, physically, it means that the wave function has no 'real' meaning until it is squared and then we get a real, physical quantity that can be measured.(58 votes)

- does this wave function also applies to photon?(13 votes)
- Nice question.

I am not a quantum expert but, as far as I know, ANY quantum system will have a wave function associated with it. Including photons, electrons, etc and, from what I understand, we are also part of a wave function when we are observing quantum phenomena. ie when we make an observation, the wave function collapses because we have (by observing it) made certain, something that was probabilistic.

So, until you observe the photon, it is defined by a wave function and its probabilty density is proportional to the square of the amplitude. When you have observed it , the wave function collapses.

mmm... hope that makes sense...(28 votes)

- This is bothering me.

What about the electrons through the double slit experiment? The scientists did observe a wave like pattern, no? How can the wave function then be considered as a probability function? Because if it were a probability function then we would have only observed it at specific places not like a wave, right?

Thanks very much!(15 votes)- What actually happens when we perform the double slit experiment and record its outcome on a screen, is that we are making a
*measurement*.

When an electron is observed it's**wave function collapses except at that point**, thus the electron exists only at said point and the observation is made. Before the measurement, the electron exists at*multiple places at the same time*(given by Schrodinger's eq.)

[refer Quantum superposition] {also refer Schrodinger's cat}

Each electron contributes to only one observation. However in the double slit experiment, we send a stream of electrons. In principle,**more electrons end up where the probability is higher**simply because the electrons are likely to end up there,and few electrons end up where the probability is less.

Hence, to put it simply, the wave pattern is formed due to individual electrons measured at different places , based on their actual numbers, which in-turn depend on the wave function.(19 votes)

- How did Schrödinger come up with this equation?

On coming up with it...how did he know that it was indeed consistent with laws of Thermodynamics?(9 votes)- The Shrodinger Equation stems from the Hamiltonian, or the total energy equation, E = KE + PE and the equation for Psi = cos(kx-wt)+isin(kx-wt) = e^[i(kx-wt)] ─ doing a bit of multivariable calculus (since psi depends on both x and t) and some algebraic manipulation you'll find that everything begins to fit together, but there are a few other identities that you need to know; ie, k=2pi/wavelength and wavelength = h/p (as seen in the previous video) and that w = E/hbar where hbar=h/2pi.

Start with E = KE + PE = 1/2mv^2 + U (where U is the general potential energy) and rewrite the KE term as p*^2 / 2m , (p being momentum, since mv*mv*1/2*1/m =1/2mv^2.

Do the necessary partial derivatives on Psi (as seen in the Shrod. eq) and start substituting things around.

Mess around with that a bit and let me know if you get stuck, I'll be happy to go into further detail if you'd like, but this should give you a headstart :)(22 votes)

- Why not square the equation to begin with? Is there a use for it in it's 'unsquared'/normal state?(8 votes)
- I believe its because you must first solve the second order differential equation provided in the video to obtain the actual wave function.(7 votes)

- Schrodinger equation tells us what; the wave function of a single electron or of a system of an electron?(3 votes)
- This equation gives perfect results (in line with experimental data) when describing a single-electron system such as hydrogen or cations having only one electrons (for example He+)....(4 votes)

- At1:20, what is X exactly?(6 votes)
- X denotes the position of a quantum particle in space. The wavefunction is a function of position (and time too, in Schrodinger's time dependent equation).(1 vote)

- Why do we need to square the wave function when we already made it into absolute value already there?

|psi|(4 votes)- the wave function is not wholly real. (it has an imaginary part to it)

So we can not measure it.

It only makes physical sense if it is squared.(4 votes)

- Consider a wave (Disturbance) in water.

As the wave propagates, the water molecules though stationary along the direction of propagation of wave move up and down.

So how does an electron behave like a wave? Does it have something like a water molecule moving up and down? I am unable to comprehend it.(4 votes)- *
**If you think you understand quantum mechanics, you don't understand quantum mechanics*** - RPF

On a serious note, the waves in both the situations are actually physicaly different, only the mathematical formulation is the same. In QM, the waves are probabilistic amplitudes, while the water waves are simple transverse/longitudinal periodic oscillations of the constituent particles. Probability waves simply mean they talk about the probability of finding the electron at a particular place. Why is it a wave like formulation, why is it so weird? Nobody knows. :)(3 votes)

- Is this electron wave is produced by electron? when the electrons produce this matter waves? Is there any connection with scattering of light?

Sorry for grammar mistakes. Please help me with this..(2 votes)- Electrons are excitations in the electron field. Photons are excitations in the electromagnetic field. Neither the electron or electromagnetic fields are the same as the quantum wave function.(4 votes)

## Video transcript

- [Instructor] So when people first showed that matter particles like electrons can have wavelengths and
when DeBroglie showed that the wavelength is Planck's constant over the momentum, people were like cool, it's pretty sweet. But you know someone
was like wait a minute, if this particle has wavelike properties and it has a wavelength, what exactly is waving? What is this wave we're
even talking about? Conceptually it's a little strange. I mean a water wave, we know what that is. It's a bunch of water that's
oscillating up and down. A wave on a string, we know what that is. This string itself is moving up and down and it extends through space. But it's hard to imagine, how is this electron having a wavelength and what is the actual wave itself? So physicists were
grappling with this issue, trying to conceptually understand how to describe the wave of the electron. They wanted to do two things. They wanted a mathematical description for the shape of that wave, and that's called the wave function. So this wave function gives
you a mathematical description for what the shape of the wave is. So different electron
systems are gonna have different wave functions, and this is psi, it's the symbol for the wave function. So this is psi, the psi symbol. It's a function of x. So at different points in x, it may have a large value,
it may have a small value. This function would give
you the mathematical shape of this wave. So that was one of the things
they were trying to determine. But they also wanted to interpret it. Like what does this
wave function even mean? So we've got two problems. We want a mathematical
description of the wave and we wanna interpret what
does this wave even mean. Now the person that gave us
the mathematical description of this wave function
was Erwin Schrodinger. So Schrodinger is this guy right here. Schrodinger's right here. He wrote down Schrodinger's Equation, and his name now is basically synonymous with quantum mechanics
because this is arguably the most important equation
in all of quantum mechanics. There's a bunch of partial
derivatives in here and Planck's constants, but the important thing is that it's got the wave function in here. Now if you've never
seen partial derivatives or calculus, it's okay. All you need to know for our
purposes today in this video is that this equation
is a way to crank out the mathematical wave function. What is this function that
gives us the shape of the wave as a function of x? And you could imagine
plotting this on some graph. So once you solve for this
psi as a function of x, you could plot what this looks like. Maybe it looks something like this, and who knows, it could
do all kinds of stuff. Maybe it looks like that. But Schrodinger's Equation is the way you can get this wave function. So Schrodinger gave us a way to get the mathematical wave function, but we also wanted to interpret it. What does this even mean? To say that this wave function
represents the electrons is still strange. What does that mean? Schrodinger tried to
interpret it this way. He said, okay maybe this electron
really is like smudged out in space and its charge
is kinda distributed in different places. Schrodinger wanted to
interpret this wave function as charge density, and I mean it's kind of
a reasonable thing to do. The way you get a water
wave is by having water spread out through space. So maybe the way you get an electron wave is to have the charge of the electron spread out through space. But this description didn't work so well, which is kinda strange. Schrodinger invented this equation. He came up with this equation, but he couldn't even interpret what he was describing correctly. It took someone else. It took a guy named Max Born to give us the interpretation we go with
now for this wave function. Max Born said no, don't interpret
it as the charge density. What you should do is interpret this psi is giving you a way to get the probability of finding the electron
at a given point in space. So Max Born said this, if you find your psi,
like he said go ahead and use Schrodinger's
equation, use it, get psi. Once you have psi, what you do
is you square this function. So take the absolute value, square it, and what that's gonna give
you is the probability of finding the electron at a given point. Now technically it's
the probability density, but for our purposes, you can pretty much just think about this as the probability of finding the electron at a given point. So if this was our wave
function in other words, Max Born would tell us that
points where it's zero, these points right here
where the value is zero, there is a zero percent
chance you're gonna find the electron there. Points where there's a large value of psi, be it positive or negative, there's gonna be a large probability of finding the electron at that point. And we could say the odds
of finding the electron at a given point here are gonna be largest for this value of x right here because that's the point
for which the wave function has the greatest magnitude. But you won't necessarily
find the electron there. If you repeat this
experiment over and over, you may find the electron here once, you may find it over here, you
may find it there next time. You have to keep taking measurements, and if you keep taking measurements, you'll get this
distribution where you find a lot of 'em here, a lot of 'em there, a lot of 'em here, and a lot of 'em here, always where there's these
peaks you get more of them than you would have at other points where the values are smaller. You build up a distribution
that's represented by this wave function. So the wave function does not tell you where the electron's gonna be. It just gives you the probability, and technically the square of it gives you the probability of
finding the electron somewhere. So even at points down here
where the wave function has a negative value, I mean you can't have
a negative probability. You square that value. That gives you the probability
of finding the electron in that region. So in other words, let's get rid of all this. Let's say we solved some
Schrodinger equation or we were just handed a wave function and we were told it looks
like this and we were asked, where are you most likely
to find the electron? Well the value of the
wave function is greatest at this point here, so you'd be most likely
to find the electron in this region right here. You'd have no shot of
finding it right there. You'd have pretty good odds
of finding it right here or right here, but you'd have the greatest
chance of finding it in this region right here. So you'd have to repeat
this measurement many times. In quantum mechanics, one measurement doesn't
verify that you've got the right wave function. Because if I do one experiment and measure one electron, boop I might find the
electron right there. That doesn't really tell me anything. I have to repeat this
over and over to make sure the relative frequency of
where I'm finding electrons matches the wave function
I'm using to model that electron system. So that's what the wave function is. That's what it can do for you, although if I were you, I'd still be unsatisfied. I'd be like, wait a minute,
okay, that's fine and good. Wave function can give us the probability or the probability density
of finding the electron in a given region, but we haven't answered the question, what is waving here and what exactly is this wave function? Is this a physical object
sort of like a water wave or even an electromagnetic wave? Or is this just some mathematical trickery that we're using that has
no physical interpretation other than giving us
information about where the electron's gonna be? And I've got good news and bad news. The bad news is that
people still don't agree on how to interpret this wave function. Yes they know that the
square of it gives you the probability of finding
the electron in some region, but people differ on how
they're supposed to interpret it past that point. For instance, is this wave function the wave function of a single electron or is this wave function
really the wave function of a system, an ensemble of electrons, all similarly prepared
that you're gonna do the experiment on? In other words, does it
describe one electron or only describe a system of electrons? Does it not describe the electron at all but only our measurement of the electron? And what happens to this wave function when you actually measure the electron? When you measure the electron
you find it somewhere, and at that moment there's no chance of finding it over here at all. So does the act of measuring the electron cause some catastrophic
collapse in this wave function that's not described by
Schrodinger's Equation? These and many more
questions are still debated and not completely understood. That's the bad news. The good news is that we don't really need to understand that to make progress. Everyone knows how to
use the wave function to get the probabilities of measurements. You can have your favorite interpretation, but luckily pretty much
regardless of how you interpret this wave function, as long as you're using it correctly to get the probabilities of measurements, you can continue making progress, testing different models, and correlating data to the measurements that people make in the lab. Now I'm not saying that interpretations of this wave function are not important. People have tried cracking
this nut for over 100 years, and it's resisted. Maybe that's because it's a waste of time or maybe it's because the
difficulty of figuring this out is so great that whoever
does it will go down in history as one of the
great physicists of all time. It's hard to tell right now, but what's undebatable is
for about 100 years now, we've been able to make
progress with quantum mechanics even though we differ on
how exactly to interpret what this wave function really represents. So recapping the wave function gives you the probability of finding a particle in that region of space, specifically the square
of the wave function gives you the probability density of finding a particle
at that point in space. This almost everyone has agreed upon. Whether the wave function
has deeper implications besides this, people differ, but that hasn't yet
stopped us from applying quantum mechanics correctly in a variety of different scenarios.