Schedule In Class 9/14 Wed Chapter 4 Test Homework (to be completed before coming to the NEXT class period) 9/15 Thurs 9/16 Fri 9/19 Mon 9/20 Tues 9/21 Wed 9/22 Thur % Composition Lab Practical (to be completed on the sheet handed out when you come to lab) ** Bring Head phones: Watch Chapter 5, Video 1: Light and Bohr s Model of the Atom & complete guided notes and learning check problems. Learning check on videos 1 and 2 and discussion video 2 Electron Configuration Problem Practice Orbital Box Diagrams in class notes How to determine the electron configuration of atoms short hand notation in class notes Electron configuration and dots discussion and practice Over weekend: Watch Chapter 5, Video 2: Quantum Mechanical Model and Orbitals & complete guided notes and learning check problems. Watch Chapter 5, video 3 Electron Configuration & complete guided notes and learning check problems. Watch video 4: Electron configuration of ions and electron dot structure & complete guided notes and learning check problems. Prelab for Flame Test Lab 9/23 Fri Flame Test Lab over weekend: Watch Video 5: Special Ionic Nomenclature & complete guided notes and learning check problems. 9/26 Mon Late start More Nomenclature!!! whoop whoop! 9/27 Tues Review for test Study for test 9/28 Wed Chapter 5 Test Prelab for next lab Thur 9/29 Alkaline Earth Metal lab video playlist: https://www.youtube.com/playlist?list=plrokdfxazqngzwd2bzn72tmmhyrirdzfd or linked on my website 1
Video 1. Light and Bohr s Model of the Atom Video: https://youtu.be/9a22fmbmd-u Textbook: Chapter 5 pages 136-148 Guided Notes for Video 1 on Light and Bohr s Model of the Atom Define the three wave properties of light? Wavelength Questions: Frequency Speed How are wavelength, frequency and energy related? How does purple light compare to red light in terms of: Energy Frequency What experiment determined the particle nature of light? and how does it show that light is a particle? What is Quantum Theory? What is a quantum? What is a photon? Describe Bohr s Model of the atom and draw a diagram of his model. (turn the page!!!) 2
What is the ground state of an atom? How does an electron reach an excited state? What happens when an electron falls from an excited state to a lower state? Learning Check (questions and answers will be discussed in class so come prepared): 1. What is the definition of wavelength? a. The number of waves that pass a certain point per second. b. The distance between a peak and a trough of a wave. c. The distance between peaks in a wave. d. The amount of energy a wave carries. 2. How are wavelength related to energy and frequency? a. When wavelength increases frequency and energy decrease. b. When wavelength increases frequency decreases but energy increases. c. When wavelength increases frequency increase and energy decreases. d. When wavelength increases frequency and energy increase. 3. Which statement is true according to the quantum theory of matter. a. matter emits wavelengths of light continuously across the electromagnetic spectrum b. matter and energy can be converted from one into another c. matter can only emit or absorb energy in increments, like stair-steps d. matter does not really exist as an object that has mass, but as a wavelength of light 4. If an electron in the excited state returns to the ground state: a. Energy is absorbed and a photon is given off b. Energy is released and a photon is given off c. It immediately returns to an excited state d. It is destroyed 5. What did the photoelectric effect demonstrate? a. That light is a wave b. That light has high energy c. That all light has energy d. That light has particle properties Discussion Question: Why does Bohr s Model of the atom explain the light emission spectrum of hydrogen? 3
Video 2: The Quantum Mechanical Model of the Atom and Orbitals Video: https://youtu.be/nr2hfzhkj2u Textbook: Chapter 5 pages 148-155 Guided Notes for The Quantum Mechanical Model and Orbitals What is the Quantum Mechanical Model? Questions: What is the Heisenberg Uncertainty Principle? What is an atomic orbital and where is it located? Electron locations are defined by 4 quantum numbers. What is a quantum number? What is the principle quantum number (n) and how does it relate to the energy of an electron? What is the quantum number of the ground state? The second quantum number is the sublevel with in an energy level and it tells the shape of the orbital. There is a limit to how many of each orbital types exist. Below write the shape of the orbital and how many of each orbital exist. Also indicate the direction of increasing energy. orbital Shape # of that orbital in an energy level s p d f (turn the page) 4
How many sublevels can fit into an energy level? Copy the list of the slide that shows what sublevels are in what energy levels: level 1 level 2 level 3 level 4 level 5 What is the Pauli Exclusion Principle? Copy the table from the slide that shows how many electrons can be found in each sublevel. Sublevel # of that type of orbital Maximum number of electrons in sublevel s p d f Learning Check: 1. The principle quantum number of the ground state is: a. 0 b. 1 c. 2 d. It doesn t have a number because it s the lowest energy level. 2. How many orbitals does the d sublevel have? a. 1 b. 3 c. 5 d. 7 3. How many TOTAL orbitals exist in the n = 3 energy level? a. 3 b. 5 c. 9 d. 10 Class discussion questions (be prepared to discuss these in class): 4. Could a 2d orbital exist? Why or why not? 5. Could a 7s orbital exist? Why or why not? 6. What is the difference between a 3p and a 4p orbital? 7. What is the difference between Heisenberg s Uncertainty Principle and the Pauli Exclusion Principle? 5
Video 3: Electron Configuration: Video: https://youtu.be/rbutz0fbkss Textbook: Chapter 5 pages 156-159 Guided Notes for Electron Configuration What is an electron configuration? Questions: What is the Aufbau Principle? Why do s orbitals of the next level fill before d orbitals of the level before? Draw the diagonal diagram below showing the correct filling order of electrons (DO THIS when I do it in the video with you). Write the electron configuration for Beryllium below and label each number and letter used in the configuration. Write the electron configurations for the atoms shown in the video Mg V The periodic table gives clues to electron configuration. What do rows represent? (turn page!!!) 6
What are blocks and how do they help with electron configuration? Write the electron configuration for Germanium. Check your learning Practice: Write electron configurations for the following elements: Na F Ca Answers to above: Na: 1s 2 2s 2 2p 6 3s 1 F: 1s 2 2s 2 2p 5 Ca: 1s 2 2s 2 2p 6 3s 2 3p 6 4s 2 IN CLASS NOTES ON ORBITAL BOX DIAGRAMS and SHORT HAND NOTATION: What is an orbital box diagram? Draw many boxes are each of the orbitals? s p d f How are electrons represented in orbital box diagrams? 7
Define Hund s Rule and how does it relate to box diagrams. Write the electron configuration and orbital box diagram for Oxygen (O) Sodium (Na) What are unpaired electrons and how do you tell how many there are in an electron configuration? What are valence electrons? How are inner electrons (non-valence electrons represented in shorthand?) Show the difference between long hand and short hand for Cl Long hand Short hand: What is the short hand for Germanium? 8
Write the electron configuration shorthand and orbital box diagram for Silver (Ag) Try the short hand for: I Zn Write the electron configuration and orbital box representation for each element. 1. H 2. Cl 3. Fe Write the shorthand configuration and orbital box diagram for: 4. Fe answers to above: 9
Video 4. Electron configuration of ions and electron dot structure Video: https://youtu.be/km0ggpastpw Textbook: Chapter 5 page 161 Guided Notes for Video 4 on electron configuration of ions and dot structure What is an electron dot structure? Questions: Draw the electron dot structure for Na Mg How do you know how many dots to draw? How does the periodic table help you determine this? Draw the electron dot structure for Cs Al Br Write the electron configuration for the following neutral and charged atoms F F -1 O O -2 Check your learning practice: Give the electron configurations and orbital diagrams for the following ion: Sr +2 Write the electron dot structure for xenon: Xe Answers to above: 10
Video 5. Special Ionic Nomenclature Video: https://youtu.be/0aw4jdftr6q Textbook: Chapter 7 pages 218-224 Guided Notes for Video 5 on special ionic nomenclature Where are most of the elements located that are considered special for ionic nomenclature and why are they special? Questions: What does the roman numeral in the number represent? Write the rules for naming binary special ionic nomenclature Practice by naming these: PbCl 4 FeO AgI What are the rules for naming ternary ionic compounds: Practice by naming these: Fe2( SO4)3 Cu(NO3)2 (turn to next page) 11
Write the formulas for the following compounds: Copper (II) Chloride: Lead (II) Sulfate Tin (IV) Sulfite Check your learning Practice: 1. Provide the name for each of the following: a. PbCl 2 b. CuF c. ZnCO 3 2. Provide the formula for each of the following: a. Iron (III) oxide b. lead (IV) bromide c. Copper (I) iodide Answers to above: 1 a. Lead (II) Chloride b. Copper (I) Fluoride c. Zinc (II) Carbonate 2. a. Fe 2O 3 b. PbBr 4 c. CuI 12
Practice problems: Write the electron configuration for each of the following elements. Draw an orbital representation for each element (Use circles and X s or boxes and arrows). 4. Kr 5. As 6. Ne 7. B 8. K Use shorthand notation and draw orbital diagrams for the following large elements: 9a. W 9b. Pb 9c. No 13
Give the electron configurations and orbital diagrams for the following ions: 10. K +1 11. S -2 12. N -3 Which atom is indicated by the following electron configurations? (pay attention because this is not the filling order, hint count electrons) 13. 1s 2 2s 2 2p 4 14. 1s 2 2s 2 2p 6 3s 1 15. 1s 2 2s 2 2p 6 3s 2 3p 6 3d 7 4s 2 16. 1s 2 2s 2 2p 6 3s 2 3p 6 3d 10 4s 2 4p 2 17. 1s 2 2s 2 2p 6 3s 2 3p 4 18. 1s 2 2s 2 2p 6 3s 2 3p 6 3d 10 4s 2 19. 1s 2 2s 2 2p 6 3s 2 3p 6 3d 10 4s 2 4p 6 5s 1 20. 1s 2 2s 2 2p 6 3s 2 3p 6 3d 10 4s 2 4p 6 4d 10 5s 2 5p 1 21. 1s 2 22. 1s 2 2s 2 2p 6 3s 2 3p 6 3d 10 4s 2 4p 6 4d 10 4f 3 5s 2 5p 6 6s 2 14
Write the electron dot structures for the following elements: 23. N 24. Te 25. Rb 26. Sr 24. Provide the name for each of the following: a. HgO d. FeO g. Pb(SO 3) 2 b. AgF e. SnS h. Cr(NO 3) 3 c. Cu(OH) 2 f. Sn 3(PO 4) 2 i. Cu(C 2H 3O 2) 2 25. Provide the formula for each of the following: a. Copper (II) nitride f. chromium (II) chlorate b. Lead (II) sulfate g. zinc chlorite c. mercury (II) nitrate h. tin (II) acetate d. tin (IV) hydroxide i. copper (I) phosphate e. cobalt (II) sulfide 26. Don't forget regular ionic nomenclature (write the name or formula for the following): a. lithium sulfide f. Na 2SO 3 b. calcium phosphate g. Sr(C 2H 3O 2) 2 c. magnesium bromide h. Ba(OH) 2 d. potassium nitride i. Na 2O e. aluminum nitrite j. MgCl 2 15
Answers to practice problems: 9a. W: [Xe] 6s 2 4f 14 5d 4 9b. Pb: [Xe] 6s 2 4f 14 5d 10 6p2 9c. No: [Rn] 7s 2 5f 14 16
24. Provide the name for each of the following: a. HgO Mercury (II) Oxide d. FeO Iron (II) Oxide g. Pb(SO 3) 2 Lead (IV) Sulfite b. AgF Silver Fluoride e. SnS Tin (II) Sulfide h. Cr(NO 3) 3 Chromium (III) Nitrate (note: silvers always +1 so don t have to write the roman numeral) c. Cu(OH) 2 Copper (II) Hydroxide f. Sn 3(PO 4) 2 Tin (II) Phosphate i. Cu(C 2H 3O 2) 2 Cooper (II) Acetate 25. Provide the formula for each of the following: a. Copper (II) nitride Cu 3N 2 f. chromium (II) chlorate Cr(ClO 3) 2 b. Lead (II) sulfate PbSO 4 g. zinc chlorite Zn(ClO 2) 2 (note: zinc always +2 so the roman numeral isn t written) c. mercury (II) nitrate Hg(NO 3) 2 h. tin (II) acetate Sn(C 2H 3O 2) 2 d. tin (IV) hydroxide Sn(OH) 4 i. copper (I) phosphate Cu 3PO 4 e. cobalt (II) sulfide CoS 26. Don't forget regular ionic nomenclature (write the name or formula for the following): a. lithium sulfide Li 2S f. Na 2SO 3 sodium sulfite b. calcium phosphate Ca 3PO 4 g. Sr(C 2H 3O 2) 2 strontium acetate c. magnesium bromide MgBr 2 h. Ba(OH) 2 barium hydroxide d. potassium nitride K 3N i. Na 2O sodium oxide e. aluminum nitrite Al(NO 2) 3 j. MgCl 2 magnesium chloride 17