Electrons and Quantum Mechanics - Oakland Schools

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Demonstration 7: Flame Tests Absorption and emission spectra are used to identify any elements. When elements are heated to high temperatures they may be placed in an excited state; in this excited state valence electrons move to higher energy levels. When the electrons return to their ground state, they may emit visible light of characteristic colors that can be used to identify the element. In this demonstration, students will identify the colors of the emission spectra of some metallic ions, using a burner and wood splints. Place the substance in the hottest part of the flame Substance to be tested Wood splint a a a a Materials Burner Wood splints Copper(II) nitrate, Cu(NO 3 ) 2 , solid crystals Barium nitrate Ba(NO 3 ) 2 , solid crystals Sodium nitrate, NaNO 3 , solid crystals Strontium nitrate, Sr(NO 3 ) 2 , solid crystals Procedure Place a small amount of one of the solid ionic compounds (about the size of a rice grain) on the tip of a wooden splint. Place the splint at the edge of the hottest part of the flame (top of inner blue cone) and observe the color. (Some students, particularly some males, may be color blind. Consider allowing students to compare their observations in small groups, alerting them to the possibility of color blindness.) (Note: Good results have been obtained with concentrated syrups of the nitrate salts.) Results Key Questions 1. What are the principal parts of an atom? 2. What forces hold atoms together? [] 3. How are electron orbitals different from orbits? 4. What is an energy level diagram? 5. How are electron energies related to orbitals? 6. How do cations form? 60
7. What determines the ionization energy of an element? 8. What determines the commonly formed cation of an atom? 9. What is the process of electron excitation? 10. Why do atoms emit light when excited? 11. How do the physical sizes of atoms and nuclei compare? 12. What are the three dimensional shapes of s and p orbitals? 13. What is meant by wave-particle duality? 14. What information is provided by quantum numbers? 15. How do quantized and continuous processes differ? 16. What is the electron configuration of (specify an element)? 61
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Oakland Schools Chemistry Resource
Page 3 and 4:
Nature of electrons Instructional B
Page 5 and 6:
Emission and Absorption Spectra htt
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Summary • An electron absorbs hea
Page 9 and 10: State the Aufbau principle. Referen
Page 11 and 12: Here is a copy of the periodic char
Page 13 and 14: Shapes of orbitals The shape of the
Page 15 and 16: “Und” is the undiscovered inert
Page 17 and 18: The octet rule as seen on the perio
Page 19 and 20: 10. The sum of the oxidation number
Page 21 and 22: Terms and Concepts Absorbance spect
Page 23 and 24: Materials (For 24 students working
Page 25 and 26: Assessment Ideas 1. Why don’t all
Page 27 and 28: 4. Return the front target, carbon
Page 32 and 33: Electrons & Quantum Mechanics Activ
Page 34 and 35: Name:______________________________
Page 36 and 37: Tips • Clorox 2 is a commercial p
Page 40 and 41: One of the odd things that we somet
Page 42 and 43: Name ___________________ Date _____
Page 44 and 45: Flame tests observations table Ion
Page 46 and 47: Going further Paper logs soaked in
Page 48 and 49: Name___________________________ Dat
Page 50 and 51: Questions and observations Examine
Page 52 and 53: Procedure 1. Into the first large t
Page 54 and 55: Analysis and Conclusions 1. Record
Page 58 and 59: Demonstraion 4: Modeling Orbitals.
Page 62 and 63: Answers to Key Questions 1. The nuc
Page 64 and 65: Counterintuitive Examples 1. Adjust
Page 66 and 67: Equipment pH paper small test tubes
Page 68 and 69: Name ______________________________
Page 70 and 71: Disposal Discussion Solutions may b
Page 72 and 73: References Beren and Brady, Laborat
Page 74 and 75: Utilizing the table below of known
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Electrons and Quantum Mechanics - Oakland Schools

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