1. chemistry
5.3 Introduction

2. Physics and the Quantum Mechanical Model
5.3
Physics and the Quantum Mechanical Model
Neon advertising signs are formed from glass tubes bent in various shapes. An electric current passing through the gas in each glass tube makes the gas glow with its own characteristic color. You will learn why each gas glows with a specific color of light.

3. 5.3
Light
Light
How are the wavelength and frequency of light related?

4. The amplitude of a wave is the wave’s height from zero to the crest.
5.3
Light
The amplitude of a wave is the wave’s height from zero to the crest.
The wavelength, represented by  (the Greek letter lambda), is the distance between the crests.

5. The SI unit of cycles per second is called a hertz (Hz).
5.3
Light
The frequency, represented by  (the Greek letter nu), is the number of wave cycles to pass a given point per unit of time.
The SI unit of cycles per second is called a hertz (Hz).

6. 5.3
Light
The wavelength and frequency of light are inversely proportional to each other.
As wavelength (λ) increases, frequency decreases.
As wavelength (λ) decreases, frequency increases. increases.
The frequency and wavelength of light waves are inversely related. As the wavelength increases, the frequency decreases.

7. 5.3
Light
The product of the frequency and wavelength always equals a constant (c), the speed of light.

8. According to the wave model, light consists of electromagnetic waves.
5.3
Light
According to the wave model, light consists of electromagnetic waves.
Electromagnetic radiation includes radio waves, radar, microwaves, infrared waves, visible light (ROY G BIV), ultraviolet waves, X- rays, and gamma rays. (add sketch slide 10)
All electromagnetic waves travel in a vacuum at a speed of  108 m/s.

9. 5.3
Light
Sunlight consists of light with a continuous range of wavelengths and frequencies.
When sunlight passes through a prism, the different frequencies separate into a spectrum of colors.
In the visible spectrum, red light has the longest wavelength and the lowest frequency.

10. 5.3
Light
The electromagnetic spectrum consists of radiation over a broad band of wavelengths. P 139.
The electromagnetic spectrum consists of radiation over a broad band of wavelengths. The visible light portion is very small. It is in the 10-7m wavelength range and 1015 Hz (s-1) frequency range. Interpreting Diagrams What types of nonvisible radiation have wavelengths close to those of red light? To those of blue light?

11. Explore the properties of electromagnetic radiation.
Light
Simulation 3
Explore the properties of electromagnetic radiation.

12. 5.1
Sodium vapor lamps produce a yellow glow.

13. 5.1

14. 5.1

15. 5.1

16. for Sample Problem 5.1
Problem-Solving 5.15 Solve Problem 15 with the help of an interactive guided tutorial.

17. 5.3
Atomic Spectra
Atomic Spectra
What causes atomic emission spectra?

18. 5.3
Atomic Spectra
When atoms absorb energy, electrons move into higher energy levels. These electrons then lose energy by emitting light when they return to lower energy levels.

19. 5.3
Atomic Spectra
A prism separates light into the colors it contains. When white light passes through a prism, it produces a rainbow of colors.
A prism separates light into the colors it contains. For white light this produces a rainbow of colors.

20. 5.3
Atomic Spectra
When light from a helium lamp passes through a prism, discrete lines are produced.
A prism separates light into the colors it contains. Light from a helium lamp produces discrete lines. Identifying Which color has the highest frequency?

21. 5.3
Atomic Spectra
The frequencies of light emitted by an element separate into discrete lines to give the atomic emission spectrum of the element.
Mercury
Nitrogen
No two elements have the same emission spectrum. a) Mercury vapor lamps produce a blue glow. b) Nitrogen gas gives off a yellowish-orange light.

22. An Explanation of Atomic Spectra
5.3
An Explanation of Atomic Spectra
An Explanation of Atomic Spectra
How are the frequencies of light an atom emits related to changes of electron energies?

23. An Explanation of Atomic Spectra
5.3
An Explanation of Atomic Spectra
In the Bohr model, the lone electron in the hydrogen atom can have only certain specific energies.
When the electron has its lowest possible energy, the atom is in its ground state.
Excitation of the electron by absorbing energy raises the atom from the ground state to an excited state.
A quantum of energy in the form of light is emitted when the electron drops back to a lower energy level. See p. 143, figure 5.14

24. An Explanation of Atomic Spectra
5.3
An Explanation of Atomic Spectra
The light emitted by an electron moving from a higher to a lower energy level has a frequency directly proportional to the energy change of the electron.

25. An Explanation of Atomic Spectra
5.3
An Explanation of Atomic Spectra
The three groups of lines in the hydrogen spectrum correspond to the transition of electrons from higher energy levels to lower energy levels. See p. 143.
The three groups of lines in the hydrogen spectrum correspond to the transition of electrons from higher energy levels to lower energy levels. The Lyman series corresponds to the transition to the n  1 energy level. The Balmer series corresponds to the transition to the n  2 energy level. The Paschen series corresponds to the transition to the n  3 energy level.

26. An Explanation of Atomic Spectra
Animation 6
Learn about atomic emission spectra and how neon lights work.

27. 5.3
Quantum Mechanics
Quantum Mechanics
How does quantum mechanics differ from classical mechanics?

28. The quanta behave as if they were particles.
5.3
Quantum Mechanics
In 1905, Albert Einstein successfully explained experimental data by proposing that light could be described as quanta of energy.
The quanta behave as if they were particles.
Light quanta are called photons.
In 1924, De Broglie developed an equation that predicts that all moving objects have wavelike behavior.

29. Light is a particle - it comes in chunks.
What is light?
Light is a particle - it comes in chunks.
Light is a wave - we can measure its wavelength and it behaves as a wave
If we combine E=mc2 , c=f, E = 1/2 mv2 and E = hf, then we can get:
 = h/mv (from Louis de Broglie)
called de Broglie’s equation
Calculates the wavelength of a particle.

30. Wave-Particle Duality
J.J. Thomson won the Nobel prize for describing the electron as a particle.
His son, George Thomson won the Nobel prize for describing the wave-like nature of the electron.
The electron is a particle!
The electron is an energy wave!

31. Confused? You’ve Got Company!
“No familiar conceptions can be woven around the electron; something unknown is doing we don’t know what.”
Physicist Sir Arthur Eddington
The Nature of the Physical World
1934

32. The physics of the very small
Quantum mechanics explains how very small particles behave
Quantum mechanics is an explanation for subatomic particles and atoms as waves
Classical mechanics describes the motions of bodies much larger than atoms

33. 5.3
Quantum Mechanics
Today, the wavelike properties of beams of electrons are useful in magnifying objects. The electrons in an electron microscope have much smaller wavelengths than visible light. This allows a much clearer enlarged image of a very small object, such as this mite.
An electron microscope can produce sharp images of a very small object, such as this mite, because of the small wavelength of a moving electron compared with that of light.

34. Quantum Mechanics
Simulation 4
Simulate the photoelectric effect. Observe the results as a function of radiation frequency and intensity.

35. 5.3
Quantum Mechanics
Classical mechanics adequately describes the motions of bodies much larger than atoms, while quantum mechanics describes the motions of subatomic particles and atoms as waves.

36. Heisenberg Uncertainty Principle
“One cannot simultaneously determine both the position and momentum of an electron.”
You can find out where the electron is, but not where it is going.
OR…
You can find out where the electron is going, but not where it is!
Werner Heisenberg

37. The Heisenberg Uncertainty Principle
5.3
Quantum Mechanics
The Heisenberg Uncertainty Principle
The Heisenberg uncertainty principle states that it is impossible to know exactly both the velocity and the position of a particle at the same time.

38. 5.3
Quantum Mechanics
The Heisenberg uncertainty principle states that it is impossible to know exactly both the velocity and the position of a particle at the same time.
This limitation is critical in dealing with small particles such as electrons.
This limitation does not matter for ordinary- sized object such as cars or airplanes.

40. It is more obvious with the very small objects
To measure where a electron is, we use light.
But the light energy moves the electron
And hitting the electron changes the frequency of the light.

41. 5.3 Section Quiz.
5.3.

42. 5.3 Section Quiz.
1. Calculate the frequency of a radar wave with a wavelength of 125 mm. Hz Hz Hz Hz

43. 5.3 Section Quiz.
2. The lines in the emission spectrum for an element are caused by
the movement of electrons from lower to higher energy levels.
the movement of electrons from higher to lower energy levels.
the electron configuration in the ground state.
the electron configuration of an atom.

44. 5.3 Section Quiz.
3. Spectral lines in a series become closer together as n increases because the
energy levels have similar values.
energy levels become farther apart.
atom is approaching ground state.
electrons are being emitted at a slower rate.

45. Chem 12 Quantum mechanics: the sequel Overlapping shells slide: slide 9 (this is the 2nd day of the quantum mechanics lesson).

46. Concept Map 5
Concept Map 5 Solve the concept map with the help of an interactive guided tutorial.

47. END OF SHOW