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Chemistry Unit 3: Atoms and Nuclear Chemistry Chapter 3: Pages 74-91* Chapter 21: Pages 649-671* Learning Targets Name ________________________ Block _________ Score: 5 4 3 Learning Target Assessment Test #1 2 1 Test #2 Compare and contrast subatomic particles. Explain and determine the atomic number and atomic mass of elements, and molar mass of compounds. Understand the concept of isotopes and how the mass number and relative atomic mass are calculated. Calculate molar conversion problems. Identify, describe, and write the nuclear equations for alpha, beta, gamma, and neutron decay. Compare fission and fusion reactions and applications of each. Calculate half-life of a radioactive isotope. Please note – Learning Target Assessments (LTAs) cannot be retaken. Test #1 is worth 25 points and Test #2 is worth 15 points. Test #3 will be worth 10 points and with completion of this learning packet the opportunity to replace Test #1 score with the sum of Test #2 and Test #3 is available. You are strongly encouraged to monitor your level of understanding for the learning targets using the table above. *Modern Chemistry – Sarquis.Sarquis; Houghton, Mifflin, Harcourt (2017) Date My homework Date My homework 1 Questions adapted from: Sarquis, M, Sarquis, J.L. (2017). Modern Chemistry Orlando, Florida: Houghton, Mifflin, Harcourt LT 1: I can compare and contrast subatomic particles. **Isotope Lab LEVEL 1 PRACTICE: Questions and Problems 1. What is an atom? What does the term “atom” literally mean? 2. Describe the 2 regions that make up an atom? 3. Subatomic Particle (symbol) Location Size Charge Proton (p+) Electron (e-) Neutron (no) LEVEL 2 PRACTICE: 1. Nuclear forces are said to hold protons and neutrons together. What is it about the composition of the nucleus that requires the concept of nuclear forces? Check for Understanding: 1. What two common types of particles are located in the nucleus of the atom? What are the relative charges of these particles? What are the relative masses of these particles? 2. Where is most of the mass of an atom located and why? 2 LT 2: I can explain and determine the atomic number and atomic mass of elements, and molar mass of compounds. LEVEL 1 PRACTICE: Questions and Problems 1. What is the atomic number? Can it be located on the periodic table, if so where? 2. What is mass number? Can it be located on the periodic table, if so where? 3. Label the components of the following atomic symbols: Ca-40 Calcium – 40 𝟒𝟐 𝐂𝐚 𝟐𝟎 4. The number of protons in one atom of an element determines the atom’s _________________, and the number of electrons determines the ___________________of an element. 5. The atomic number tells you the number of ______________________in one atom of an element. It also tells you the number of ___________________in a neutral atom of that element. 6. In order to calculate the number of neutrons you must subtract the __________________from the ______________________. 7. Give the symbol and number of protons in one atom of: a. Lithium b. Iron c. Oxygen __________ __________ __________ d. Krypton e. Helium __________ __________ 8. Give the symbol and number of protons and electrons in a neutral atom of: Uranium ______ Protons_______ Electrons_______ Boron ______ Protons_______ Electrons_______ 9. Name the element that has the following numbers of subatomic particles: a. 26 electrons, 29 neutrons, 26 protons ________ c. 53 protons, 74 neutrons ________ b. 2 electrons (neutral atom) ________ d. 20 protons _________ e. 15 protons _________ 10. If you know only the following information can you always determine what the element is? If the answer is 'No' explain why not. a. number of protons b. number of electrons in a neutral atom c. number of neutrons d. number of electrons 3 11. What are isotopes? Describe an example. 12. Identify the following pairs of elements as isotopes or different elements. a. Element A has 42 protons and 50 neutrons Element B has 42 protons and 51 neutrons _______________________ b. Element X has 54 protons and a mass number of 124 Element Z has 54 protons and a mass number of 130 ______________________ c. Element C has 38 neutrons and an atomic number of 22 Element D has 38 neutrons and an atomic number of 23 _______________________ 15. Fill in the following missing parts in the charts below: Symbol O-16 F I p+ e- Mass # Atomic # 10 74 69 111 145 50 75 U Symbol no Protons Electrons Mass Number Atomic Number Neutrons 28 42 Cl-36 -87 37 37 14 6 59 65 U- 234 7 9 33 13. Determine the molar mass of the following: KClO4 g/mol Pb(SO4)2 SnI4 g/mol (NH4)3PO4 CBr4 g/mol CO2 H2O g/mol C6H12O6 Ca(NO3)2 g/mol 42 g/mol g/mol g/mol g/mol 14. Describe how molar mass is calculated. 4 LEVEL 2 PRACTICE: 1. Fill in the missing parts to the chart below: (ions=charged atoms) Atomic Symbol Mass Number Protons Number Neutrons Electrons 30 25 21 18 52 Cr 3+ 25 19 133 80 55 54 Br 1- Zinc-65 2. Can two atoms with the same mass number ever be isotopes of each other? Explain. Check for Understanding: 1. Complete the following table. Name Nuclear Symbol Sodium – 23 157N Lithium - _____ Boron - 11 Protons 11 Neutrons Electrons 8 6 5 2. There are three stable isotopes of Argon: Argon-36, Argon-38, and Argon-40. What would the atoms of these isotopes have in common? What would be different about their atoms? 3. Calculate the Molar Mass of each of the following to TWO decimal places. A. CuNO3 ____________________________________ B. Ag2SO4 ____________________________________ C. Ca3(PO3)2 ____________________________________ D. H2O ____________________________________ LT 3: I understand the concept of isotopes and how the mass number and relative atomic mass are calculated. **POGIL – Average Atomic Mass (first 3 questions below taken from: POGIL Activities for High School Chemistry. 2012. The POGIL Project and Flinn Scientific, Inc. LEVEL 1 PRACTICE: Questions and Problems 1. The average atomic mass of nitrogen is 14.0067amu. Predict which isotope listed below is most abundant in nature? a. N-13 b. N-14 c. N-15 2. Explain why a weighted average is used to calculate the average atomic mass of an element. Why is it not sufficient to calculate a simple average of the isotope data? 5 3. A mystery element, called ‘muriacticum’ by its discoverer, exists on Earth as a mixture of two isotopes. The most abundant isotope (75.76%) has a mass of 34.9689amu; the other isotope (24.24%) has a mass of 36.9659 amu. Calculate the average atomic mass and identify the element by its modern name. Example Calculations 4. Calculate the average atomic mass of Carbon. 12 C 13 C 6 Actual Mass 12.000000 amu 98.90% abundant 6 Actual Mass 13.003355 amu 1.10% abundant 5. Determine the average atomic mass of the following: There are 4 isotopes of an unknown element. If out of 100 atoms, 28 have a mass of 171 amu, 45 have a mass of 172 amu, 12 have a mass of 174 amu and 15 have a mass of 178 amu. 6. Determine the percent of each isotope in the following: There are 2 stable isotopes of Warriorium. Warriorium258 and Warriorium-267 have an average atomic mass of 264.275 amu. 7. When a sample of natural copper is vaporized and injected into a mass spectrometer, the results show the sample is 69.09% copper-63 and 30.91% copper-65. Use these data to compute the average mass of natural copper. (The mass values for 63Cu and 65Cu are 62.93 amu and 64.93 amu, respectively.) 6 8. What is the atomic mass of hafnium if, out of every 100 atoms, 25 have a mass of 176 amu, 16 have a mass of 177 amu, 23 have a mass of 178 amu, 31 have a mass of 179 amu, and 5 have a mass of 180 amu? **Hint: Think back to Skittle Lab! 9. What is the atomic mass of lithium if 8.5% of its atoms have a mass of 6.02 amu and 91.5% of its atoms have a mass of 7.02 amu? 10. Three isotopes of argon occur in nature -- calculate the average atomic mass of argon to two decimal places, given the following relative atomic masses and abundances of each of the isotopes: argon-36 (35.97 amu; 0.337%), argon-38 (37.96 amu; 0.063%), and argon-40 (39.96 amu; 99.600%). LEVEL 2 PRACTICE: 1. Three isotopes of silicon occur in nature. 92.23% occur as Silicon-28 (which has an atomic mass of 27.97693 amu); 4.68% occur as silicon-29 (which has and atomic mass of 28.97649 amu); and 3.09% occur as silicon-30 (which has and atomic mass of 29.97377 amu). Calculate the atomic weight of silicon. Check for Understanding: 1. What is the atomic mass of magnesium if 78.99% of its atoms have a mass of 23.98 amu, 11.01% of its atoms have a mass of 24.98 amu, and 10.00% of its atoms have a mass of 25.98 amu? (1 point) 2. What is the atomic mass of hafnium if, our of every 100 atoms, 33 have a mass of 161 amu, 15 have a mass of 163 amu, 15 have a mass of 165 amu, 9 have a mass of 167 amu, and 28 have a mass of 169 amu? (1 point) 3. There are only two isotopes of Antimony: Antimony-121 and Antimony-123. Calculate the percentage of each isotope if the average atomic mass of Antimony is 121.76 amu. 7 LT 4: I can calculate molar conversion problems. LEVEL 1 PRACTICE: Questions and Problems 1. Describe a mole (use, size, etc). -MOLE MAP- Moles and grams 2. 100 g of NaOH = ? moles of NaOH 3. 3.5 moles of CO2 = ? grams of CO2 4. 650 g of H2O = ? grams of H2O Grams to moles = _______________ by molar mass Moles to grams = _______________ by molar mass Moles and molecules 5. 4.25 x 1027 molecules CO = ? moles of CO 6. 1.28 x 108 mol PbBr4 = ? molecules of PbB4 7. 1.2 x 1020 molecules SnO = ? moles SnO Molecules to moles = _____________________ by 6.022 X 1023 Moles to molecules = ____________________ by 6.022 X 1023 Molecules/Formula Units to Atoms 8. 3.0 X 1015 molecules of C6H12O6 = ? atoms of C 8 9. 9.03 X 1024 atoms of Br2 = ? molecules of Br2 10. 2.3 X 1025 formula units of NaCl = ? atoms (total atoms) Atoms to Molecules/Formula Units = _____________________ by subscript of element(s) Molecules/Formula Units to Atoms = _____________________ by subscript of element(s) Mixed Questions 11. Convert the following: 36.03 g C ? atoms C 2.408 X 1024 formula units NaCl ? g NaCl .25 moles H2O ? g H2O 12.67 moles C6H12O6 ? molecules C6H12O6 1000 g Cl2 ? molecules Cl2 3.01 X 1025 atoms of Au ? grams Au 4.2 X 1022 molecules of NO2 ? grams of NO2 9 LEVEL 2 PRACTICE: 1. Juglone, a dye known for centuries, is produced from the husks of black walnuts. It is also a natural herbicide that kills off competitive plants around the black walnut tree but does not affect grass and other noncompetitive plants. The formula for juglone is C10H6O3. (a.) Calculate the molar mass of juglone. (b.) A sample of 1.56 x 10-2 g of pure juglone was extracted from black walnut husks. How many moles of juglone does this sample represent? 2. Calcium carbonate, also called calcite, is the principle mineral found in limestone, marble, chalk, pearls, and the shells of marine animals such as clams. (a) Calculate the molar mass of calcium carbonate. (b) A certain sample of calcium carbonate contains 4.86 moles. What is the mass in grams of this sample? What is the mass of the CO32- ions present? Check for Understanding: 1. What is the mass in grams of 2.52 mol of iron, Fe? 2. How many moles of calcium, Ca, are in 0.565 g of calcium? 3. How many molecules of H2O, water, are in 3.75 mol of water? 4. What is the mass in grams of 5.7 x 1015 atoms of sodium chloride, NaCl? 5. How many atoms of sulfur, S, are in 3.00 g of sulfur? LT 5: I can identify, describe, and write the nuclear equations for alpha, beta, gamma, and neutron decay. LEVEL 1 PRACTICE: Questions and Problems 1. What is a nuclear reaction? What determines the stability of the nuclide? 2. What is the neutron-proton ratio among elements with low atomic numbers? High atomic number? 10 3. What is the difference between ionizing and non-ionizing radiation? 4. Define radioactive decay 5. Compare and contrast the three types of radiation. Type of Radiation Alpha Symbol Change in Mass # Change in Atomic # Charge Decreases by 4 Decreases by 2 2+ Beta No Change Increases by 1 1- Gamma No Change No Change 0 6. Complete the following nuclear decay equations: E. 2386Ra _______ + 42He B. 8737Rb 8738Sr + _______ F. 9943Tc C. 263106Sg 259104 Rf + ________ G. 137N D. 116C H. 10646Pd ______ + 0+1 146C ______ + 0-1 A. ______ + 136C + _______ + ____ 10645Rh 7. Predict the isotopes for the following: A. Th-234 +1 beta particle C. U-238 + 1 alpha particle B. Ba-141 + 1 beta particle D. Cs-136 +1 alpha particle 8. Show the breakdown of the following isotopes being hit by one neutron: A. U-235 to Ba-142 and Kr-92 B. U-235 to Rb-90 and Cs-144 C. U-238 to Xe-142 and Sr-192 9. Write a nuclear equation for the alpha decay of palladium-231. 10. .Write a nuclear equation for the positron decay of nitrogen-13. 11 11. Write a nuclear equation for the beta decay of francium-223. 12. Write a nuclear equation for the alpha decay of gadolinium-150. 13. Uranium-235 decays by the series below. What is the final stable element? 235 U ,,,,,,,,,, __________ 92 Check for Understanding: 1. Show the breakdown of the following radioactive isotope being hit by one neutron. U-238 + Neutron Ba-141 and Kr-90 2. Predict the daughter species when the parent species undergoes alpha decay. Np-238 3. Predict the daughter species when the parent species undergoes beta decay. Th-234 4. Complete the continuing radioactive decay for the following radioactive isotope: Alpha Beta Neutron Gamma 235 92 U _____ _____ _____ _____ LT 6: I can compare fission and fusion reactions and applications of each. LEVEL 1 PRACTICE: Questions and Problems 1.How are nuclear fusion and nuclear fission alike? How are they different? Which is used in nuclear bombs and nuclear reactors? Why? Check for Understanding: 1. Compare and contrast nuclear fission and fusion. Describe an example of each. 12 LT 7: I can calculate half-life of a radioactive isotope. Calculating Half-lives A. Half-life (t1/2) = time required for half of the atoms of a radioactive nuclide to decay. B. Solve half-live problems, first determine the rate constant (k) k = ln(0.5)/half life years C. Use the k value to determine how long it takes for decay to occur t1/2 = ln(time left as decimal)/k Example: The radioactive isotope cobalt-60 has a half-life of 5.27 years. What is the rate constant? K = ln(0.5)/5.27 = -0.132 How long will it take 20% of the cobalt-60 to change to nickel-60? t1/2 = ln(.80)/-0.132 = 1.69 years How long will it take 70% of the cobalt-60 to decay to nickel-60? t1/2 = ln(.30)/-0.132 = 9.12 years LEVEL 1 PRACTICE: Questions and Problems The radioactive isotope carbon-14 has a half-life of 5730 years. 1. What is the rate constant for carbon-14? 2. How long will it take for 10% of the carbon-14 to change to nitrogen-14? 3. How long will it take for 50% of the carbon-14 to change to nitrogen-14? 4. How long will it take for 75% of the carbon-14 to change to nitrogen-14? The radioactive isotope U-238 has a half-life of 4.5 billion years. 5. What is the rate constant for U-238? 6. How long will it take for 20% of the U-238 to change? 7. How long will it take for 65% of the U-238 to change? 8. How long will it take for 90% of the U-238 to change? The radioactive isotope Pu-239 has a half-life of 24,400 years. 9. What is the rate constant for Pu-239? 10. How long will it take for 15% of the Pu-239 to change? 13 11. How long will it take for 60% of the Pu-239 to change? 12. How long will it take for 95% of the Pu-239 to change? Check for Understanding: 1. The radioactive isotope Uranium-238 has a half life of 4,500,000,000 years. A). What is the rate constant for Uranium-238? (1 point) B) How long will it take for 25% of the Uranium-238 to change to Thorium-234? C) How long will it take for 65% of the Uranium-238 to change to Thorium-234? D) How long will it take for 93.75% of the Uranium-238 to change to Thorium-234? Review lab concepts. Reflect: What do I need to work on? What steps will I take to understand and apply the concepts better? CCRS for this Unit: Description Secure (S) Developing (D) Beginning (B) CCRS #1 How well do you productively work towards accomplishing goals? CCRS #2 How well do you collaborate with others? Creates and monitors a personal organization plan that sets and prioritizes goals within a timeframe. Creates a personal organization plan to accomplish a task or meet goals by using available resources and meeting deadlines. Implements teacherdesigned organization plan to accomplish a task or goal. Engages in interdependent work with others to solve problems through communication, questioning, and respectful discussion. Engages in work with others to solve problems while working towards developing habits of questioning and respectful discussion. Participates in independent work and ask questions of others. CCRS #3 How well do you utilize feedback for improvement? CCRS #4 How well do you demonstrate respect? Initiates communication with others to seek and respond to specific information for growth toward a goal. Responds to specific information for growth toward improving skills. Responds to feedback as a part of task completion. Initiates interactions with others using language, body language, listening skills, and actions that contribute to a positive learning community. Understands and acknowledges the impact of using language, body language, listening skills, and actions that contribute to a positive learning community. Recognizes the impact of language, body language, listening skills, and action that contribute to a positive learning community. Score CCRS UNIT REFLECTION: Complete a reflection on your current score recorded for all 4 standards that includes examples of how you have demonstrated or not demonstrated the standard. For all standards record a plan of action (POA) to work towards secure for the standard. **Reflect on the different aspects of class: peer learning activities, class work time, lab time, at home learning, etc… 14