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Chemistry Unit 3: Atoms and Nuclear Chemistry Name ______Chapter 3: Pages 74-91* Block ______Chapter 21: Pages 649-671* 100% Complete Yes No Chemistry Unit 3: Atoms and Nuclear Chemistry Name _______________________________________ Chapter 3: Pages 74-91* Block _________ Chapter 21: Pages 649-671* 100% Complete Yes No Learning Targets Learning Test #1 Test #2 Target Assessment I can compare and contrast subatomic particles. I can explain and determine the atomic number and atomic mass of elements, and molar mass of compounds. I can understand the concept of isotopes and how the mass number and relative atomic mass are calculated. I can calculate molar conversion problems. I can identify, describe and write the nuclear equations for alpha, beta, gamma and neutron decay; I can compare fission and fusion reactions and applications of each. Please note – Learning Target Checks (LTCs) cannot be retaken. Test #1 is worth 25 points and Test #2 is worth 15 points. Test #3 (taken on the day of the term test) 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) 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. Practice Problems: 1. What is an atom? What does the term “atom” literally mean? (Look up if not sure) 2. Describe the 2 regions that make up an atom. 3. Subatomic Particle Location Size Charge (symbol) Proton (p+) Electron (e-) Neutron (no) 1 4. Draw and label the parts of an atom. 5. Where is most of the mass of an atom located and why? Where is most of the volume of an atom? 6. Write whether the following characteristics pertain to protons (P), neutrons (N) or electrons (E). You may use more than one letter on each line! a) ________Determines an element’s identity. b) ________Has a mass of 1 AMU c) ________An atom’s average atomic mass includes this type of subatomic particle. d) ________Is found in the nucleus of an atom e) ________Has a positive charge f) ________Has a neutral charge g) ________These subatomic particles can vary and ions form when they are gained/lost h) ________Is found outside the nucleus of an atom i) ________Has a negative charge j) ________Has a mass of that is estimated to be 0 AMU k) ________Subatomic particle used to determine the atomic number. l) ________Makes up most of the mass of an atom m) ________Are the smallest of all 3 subatomic particles n) ________These subatomic particles can vary and form different isotopes. o) ________These subatomic particles are found in orbitals/energy levels. p) ________Subatomic particle used to determine an element’s chemical properties. q) ________The number of these subatomic particles present determines the charge. LT 2: I can explain and determine the atomic number and atomic mass of elements, and molar mass of compounds. Practice Problems: 1. What is the atomic number? Identify, if possible, in the image to the right. 2. What is mass number? Identify, if possible, in the image to the right. 3. What is the relative atomic mass? Identify, if possible, in the image to the right. 2 4. Answer the following questions about different formats for writing elements: Ca-40 Element __________________ Atomic # ________What does the 40 represent? __________________ Carbon – 14 Atomic # __________ What does the 14 represent? ____________________ ퟑퟔ 퐂퐥 Element __________________ Atomic # ________What does the 36 represent? __________________ ퟏퟕ 5. In a neutral atom, the atomic number tells you the number of _________________________ and __________________________ in one atom of an element. 6. In order to calculate the number of neutrons you must subtract the ______________________________from the ______________________. 7. Give the symbol and number of protons and electrons in a neutral atom of: Uranium ______ Protons_______ Electrons_______ Boron ______ Protons_______ Electrons_______ 8. 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 _________ 9. 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 10. What are isotopes? Describe an example. 11. 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 _______________________ 12. 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 13. Can two atoms with the same mass number ever be isotopes of each other? Explain. 14. Fill in the following missing parts in the charts below: Symbol Protons Electrons Mass Number Atomic Number Neutrons 28 42 Cl-36 -87 37 37 14 6 59 65 U- 234 7 9 33 42 15. Fill in the following missing parts in the charts below (note: charges are included this time!) Symbol Atomic Number Mass Number Protons Neutrons Electrons 52 Cr 3+ 25 30 25 19 21 18 133 55 54 80 Br 1- 16. What is molar mass? 17. Describe how molar mass is calculated. 4 18. Determine the molar mass of the following: KClO4 g/mol Pb(SO4)2 g/mol SnI4 g/mol (NH4)3PO4 g/mol Ca(NO3)2 g/mol C6H12O6 g/mol 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. Example Calculations: Practice 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. 4. Calculate the average atomic mass of carbon: ퟏퟐ ퟏퟑ 퐂 퐂 ퟔ ퟔ Actual Mass Actual Mass Average Atomic Mass = _____________ 12.000000 amu 13.003355 amu 98.90% abundant 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. 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.) 7. 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? 8. 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%). 9. 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? 6 10. 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. 11. CHALLENGE: 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. LT 4: I can calculate molar conversion problems. Practice Problems: 1. Describe a mole (use, size, etc). 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 = ? moles of H2O Grams to moles = _______________ by molar mass Moles to grams = _______________ by molar mass 7 Moles and molecules 5. 4.25 x 1027 molecules CO = ? moles of CO 6.
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