1. Drill Determine the electron configuration of the following: Determine the electron configuration of the following: H He He

2. Objective SWBAT: SWBAT: Use a flame test in order to determine the identity of the cation in an unknown solution based on its characteristic color in a flame. Use a flame test in order to determine the identity of the cation in an unknown solution based on its characteristic color in a flame.

3. SAT/HSA Enrichment …has a mass that is approximately the same as the mass of … …has a mass that is approximately the same as the mass of … a. a beta article…a proton b. a neutron…a proton c. an alpha particle…an electron d. a positron….an electron e. an electron…a neutron

4. Engagement: Things to think about during today’s activity. Atoms of different elements have distinct properties related to their composition. How do atoms of different elements differ?

5. Physics How do atoms relate?

6. 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. 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.

7. Light The amplitude of a wave is the wave’s height from zero to the crest. 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. The wavelength, represented by (the Greek letter lambda), is the distance between the crests. The frequency, represented by (the Greek letter nu), is the number of wave cycles to pass a given point per unit of time. 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). The SI unit of cycles per second is called a hertz (Hz).

8. Light The wavelength and frequency of light are inversely proportional to each other. The wavelength and frequency of light are inversely proportional to each other.

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

10. Light According to the wave model, light consists of electromagnetic waves. According to the wave model, light consists of electromagnetic waves. Electromagnetic radiation includes radio waves, microwaves, infrared waves, visible light, ultraviolet waves, X-rays, and gamma rays. Electromagnetic radiation includes radio waves, microwaves, infrared waves, visible light, ultraviolet waves, X-rays, and gamma rays. All electromagnetic waves travel in a vacuum at a speed of 2.998  10 8 m/s. All electromagnetic waves travel in a vacuum at a speed of 2.998  10 8 m/s.

11. Light Sunlight consists of light with a continuous range of wavelengths and frequencies. 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. 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. In the visible spectrum, red light has the longest wavelength and the lowest frequency.

12. Light The electromagnetic spectrum consists of radiation over a broad band of wavelengths. The electromagnetic spectrum consists of radiation over a broad band of wavelengths.

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

14. 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. When white light passes through a prism, it produces a rainbow of colors.

15. Atomic Spectra When light from a helium lamp passes through a prism, discrete lines are produced. When light from a helium lamp passes through a prism, discrete lines are produced.

16. Atomic Spectra The frequencies of light emitted by an element separate into discrete lines to give the atomic emission spectrum of the element. The frequencies of light emitted by an element separate into discrete lines to give the atomic emission spectrum of the element. Mercury Nitrogen

17. An Explanation of Atomic Spectra In the Bohr model, the lone electron in the hydrogen atom can have only certain specific energies. 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. 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. 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. A quantum of energy in the form of light is emitted when the electron drops back to a lower energy level.

18. 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. 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.

19. 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. The three groups of lines in the hydrogen spectrum correspond to the transition of electrons from higher energy levels to lower energy levels.

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

21. 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. 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.

22. 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. 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.

23. 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. 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 is critical in dealing with small particles such as electrons. This limitation does not matter for ordinary-sized object such as cars or airplanes. This limitation does not matter for ordinary-sized object such as cars or airplanes.

24. Quantum Mechanics The Heisenberg Uncertainty Principle The Heisenberg Uncertainty Principle

25. Quick Quiz. 1.The lines in the emission spectrum for an element are caused by a. the movement of electrons from lower to higher energy levels. b. the movement of electrons from higher to lower energy levels. c. the electron configuration in the ground state. d. the electron configuration of an atom.

26. Quick Quiz 2.Spectral lines in a series become closer together as n increases because the a. energy levels have similar values. b. energy levels become farther apart. c. atom is approaching ground state. d. electrons are being emitted at a slower rate.

27. Spectrum Park Letter from Mrs. Lattice Letter from Mrs. Lattice Teacher Flame test Demo Teacher Flame test Demo Complete Flame test Lab and Analysis Questions. Complete Flame test Lab and Analysis Questions.

28. Summary Questions Was the objective accomplished? Explain. How do atoms of different elements differ? Identify the main concepts of today’s activity. How does your lab investigation relate to the activity of electrons? Use the following: Ground state – lowest energy level Excited state – higher energy level

29. Homework Letter to Ms. Lattice Letter to Ms. Lattice