1.05 The dual nature of the electron

Loading...

En provenance du cours de University of Kentucky

Chemistry

560 notes

University of Kentucky

Chemistry

560 notes

This course is designed to cover subjects in advanced high school chemistry courses, correlating to the standard topics as established by the American Chemical Society. This course is a precursor to the Advanced Chemistry Coursera course. Areas that are covered include atomic structure, periodic trends, compounds, reactions and stoichiometry, bonding, and thermochemistry.

À partir de la leçon

Week 1

We will learn about the components inside the atom and look especially at the electrons. The electron structure determines the properties of the elements. So, by the end of this series of lessons, you will know for each elements where the electrons are located in the atom.

1.01 Subatomic Particles: Protons, Neutrons, Electrons and the Nucleus 21:51

1.02 Understanding Light 19:02

1.03 Quantum Theory, Energy and frequency and the photoelectric effect17:29

1.03a Energy of Photon 4:24

1.03b Watts to Photons 7:02

1.04 Bohr's model of the hydrogen atom 6:42

1.05 The dual nature of the electron 8:01

1.06 The Heisenberg Uncertainty principle 6:40

1.07 Quantum Numbers 25:33

1.07a Quantum Numbers 3:29

1.08 Explaining Atomic Theory 16:20

1.08a Balmer Series 5:38

1.09 Atomic Orbitals 15:45

1.10 Orbital Diagrams 6:21

1.10a QN and Orbital Diagram 1:54

1.11 Electron Configuration 33:33

1.11a Electron Configuration 12:06

Rencontrer les enseignants

Dr. Allison Soult
Lecturer
Chemistry
Dr. Kim Woodrum
Sr. Lecturer
Chemistry

The previous learning objective, we talked about how electromagnetic radiation, or

light, can behave as a wave but also as a particle, it has a dual nature.

In this learning objective,

we're also going to see dual nature that is applying to electrons.

We're going to see why this is a,

it was proposed as an explanation for electronic structure.

We are going to see the evidence that supports the fact that

electrons have this dual nature, and we're going to

learn how to do calculations of wavelengths of these particles.

Now we know that the electrons, according to Bohr's model,

could only occupy certain fixed locations around the nucleus.

The question was why?

Why can an electron be traveling in a region where the n equals 1, and in

a region where n equals 2, but it cannot travel anywhere in between those two?

Well de Broglie was the one who provided a solution, by proposing this dual nature.

By proposing that electrons not only have the particle nature, they have mass,

we know they are particles, but also behave as waves.

Now these two diagrams show an allowed state for the electron and

a non-allowed state for the electron, when you're thinking about them as a wave.

If the red represents the distance from the nucleus that the electron can

exist at, so that's an n equals 1 or a n equals 2 or a n equals 3 region.

The electron will have a wavelength such that it is an integral number of

wavelengths around that area.

So that when the electron travels as a wave,

the wave will line up on itself, and it can exist there.

But if you moved a little bit different distance away, and

you were traveling at that same wavelength, then at this distance,

the down and the up trough, or the down trough and

the up peak of the wave would make it so that the wave could not exist there.

So this is why de Broglie proposed that electrons have this wave nature that,

that would help explain why an electron can be here, but it cannot be here.

So proposing that it has a dual nature is one thing.

Seeing evidence that they have this wave nature is something else.

Now if an electron were a particle, and you were to pass the particles through

the slits, what you would see is those particles would travel straight from

the slit and strike the surface of this plate that is detecting electrons.

And it would travel, and it would do straight to this slit through there, and

you would see it lighting up only in two spots that correspond to the slits.

But this is not what happens.

If you were to pass these electrons through those slits instead you

would see a defraction pattern much like light does.

When light travels through the slits you have a,

an alternating bright and dark patches on the photo-electric paper.

Well, these are detecting electrons instead of just two beams.

What we see is a sequence of dark and light and dark and light.

What that means is those electrons have a wave nature and

those waves are being bent by the slits.

And as they interact, and they have a peak and a peak, you'll see a bright spot and

a trough and a peak.

You'll see a dark spot.

And we see this very definite diffraction pattern occurring of constructive and

deconstructive interference of those waves.

Now, if it behaves as a wave, it would have a wave length.

And they were actually able to, with this equation,

get a relationship between the wavelength of the particle and the mass and

the velocity of the particle as it travels.

So that of course is wavelength.

This is mass.

And the mass is going to need to be put in, in kilograms.

This is velocity.

And velocity was in meters per second.

And we've seen Planck's constant before, okay?

That's Planck's constant.

And Planck's constant, you will be provided with that when you work problems,

but it's 6.626 times 10 to the minus 34.

And it's joules times seconds.

But, you need to watch your units when you work this.

Now I've given what they need to be in, but why do they need to be in this?

It is because of what a joule is.

A joule if you break it down into its base units,

is a kilogram, meter squared per second squared.

And then that would be time second.

So this would be the units of Plank's constant.

If this is in kilograms, it's going to be canceling with this kilograms nicely.

And if these are meters per second,

they're going to cancel with the meters per second.

So we're going to be left with one of these meters left over, and

that'll give off our wavelength out, in meters.

So let's work a problem.

Now this one is a silly problem, dealing with a ping-pong ball.

But any particle can have this wave nature.

We just don't really observe that wave nature with something as large as a tin,

a ping-pong ball.

And let's see why that is.

Wavelength would be equal to Planck's constant, 6.626 times 10 to the minus 34.

Joules times second and joule is a kilogram,

meters squared, per second squared and then times seconds.

That's the Planck's Constant units.

Divided by mass, now it's a 2.5 gram ping-pong ball, so 2.5 grams.

We don't want it in grams because of this kilogram here.

So we'll convert it to kilograms, a kilogram is 1,000 grams, so

that'll give me my mass in kilograms, and velocity.

It's 15.6 meters per second.

So now let's have our units cancelling here, the grams are certainly canceling.

The kilograms are cancelling.

One of these seconds is cancelling one of these seconds, and

this second is cancelling this one.

And this meter is cancelling with one of those, so we're left with meters.

Now it's asking for it in nanometers, we'll worry about that later.

And when we divide all of these values out we get 1.7 times 10 to the negative 37.

Sorry, times 10 to the negative 32 meters.

1.7 times 10 to the negative 32 meters.

This is tiny, tiny, tiny,

too tiny to even observe kind of wavelength.

Let's go ahead and

convert it to nanometers cause that is what wavelength is usually reported at,

especially when we're dealing with electromagnetic radiation.

So a nanometer is 10 to the minus 9 meters and

that's going to give me 1.7 times 10 to the minus 23 nanometers.

So any particle, if you know its mass and

its speed, can have a calculated wavelength.

But it's only really the wavelength of the very,

very tiny, tiny particles that give you if you have a mass of very,

very small, very small mass.

Then you're going to have a wavelength that is actually measurable and

observable.

So this is the end of learning objective five.

We see that electrons not only have the particle nature that we would expect.

But also have a wave nature, and you can calculate the wavelength

of any particle if you know the mass and the velocity.

Explorer notre catalogue

Rejoignez-nous gratuitement et obtenez des recommendations, des mises à jour et des offres personnalisées.

Coursera propose un accès universel à la meilleure formation au monde, en partenariat avec des universités et des organisations du plus haut niveau, pour proposer des cours en ligne.

© 2019 Coursera Inc. Tous droits réservés.

Télécharger dans l'App Store

Disponible sur Google Play