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Lab # 14 TEST REVIEW – ANSWER KEY

Lab # 14 TEST REVIEW – ANSWER KEY. Covering Textbook Sections: 4.3 4.4 4.5. 1. Match the scientist with his achievement. A. Aston C. Moseley E. Thomson B. Chadwick D. Rutherford. _____ i . discovered the atomic nucleus

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Lab # 14 TEST REVIEW – ANSWER KEY

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  1. Lab # 14TEST REVIEW – ANSWER KEY Covering Textbook Sections: 4.3 4.4 4.5

  2. 1. Match the scientist with his achievement.A. Aston C. Moseley E. Thomson B. Chadwick D. Rutherford _____ i. discovered the atomic nucleus _____ ii. first to separate individual isotopes _____ iii. discovered the electron _____ iv. discovered the proton _____ v. discovered the neutron D. A. E. C. B.

  3. 2. 1 amu (atomic mass unit) is approximately equal to ___ grams. 1.66 x 10 – 24 g

  4. 3. All atoms are compared to the isotope carbon-12 in order to express their: • atomic number • mass number • number of electrons • relative atomic mass • number of neutrons

  5. 4. Nitrogen-15 has __ protons and __neutrons. protons = 7 neutrons = 8

  6. 5. What is the atomic number of Pd-103? • 46 • 103 • 57 • 149 • 106.42

  7. 6. What is the mass number of ytterbium-169? • 39 • 130 • 169 • 173.04 • 99

  8. 7. What does the following atomic symbol indicate about this isotope of hydrogen? • It has no protons • It has no neutrons • It has no electrons • It has no mass • It’s atomic number is 2

  9. 8. Write the correct atomic symbol for an isotope of silver with 64 neutrons.

  10. 9. Which of the following atomic symbols correctly represents an isotope of manganese with 31 neutrons? A. B. C. D. E.

  11. 10. Match the words with the correct definition.A. Atomic mass C. Isotope E. nuclide B. Atomic number D. Mass number _____ i. atoms of the same element that have different masses _____ ii. number of p+ in the nucleus _____ iii. one type of isotope or one atom of a specific isotope _____ iv. number of p+ and No in the nucleus _____ v. “weight” of an atom C. B. E. D. A.

  12. 11. How does the mass of an electron compare to that of a proton or neutron? An electron is 1,836timesLESS massive than a proton or neutron

  13. 12. What are the approximate relative atomic masses, in amu, of a proton, an neutron, and an electron? • Proton ≈ 1 amu • Neutron ≈ 1 amu • Electron ≈ 0.00055 amu

  14. 13. Which pair of isotopes contain the same number of neutrons? A. and • and • and • and

  15. 13. Element X has 9 protons, 9 electrons, and 11 neutrons. What is the atomic symbol for element X?

  16. 14. In what way do the following neutral isotopes differ from one another? and They have different numbers of neutrons.

  17. 15. Are the following two nuclides isotopes of the same element? Explain. and NO Each nuclide has a different atomic number…… …..therefore they cannot be isotopes of the same element.

  18. 16. Answer the following questions based on the following atomic symbol. _______ a. What is the atomic number? _______ b. How many neutrons are present? _______ c. What is the mass number? _______ d. How many protons are present? _______ e. What is the identity of this element? 37 31 68 37 Rubidium

  19. 17. After counting and massing 3 types of beans a student made the following data table. Bean 1 Bean 2 Bean 3 TotalCount 22 15 66 103 % abundance total mass of beans(g) 7.558 9.441 6.888 Xaverage mass of bean (g) What is the percent abundance of Bean 3? 66 Bean 3 x 100 = 103 Total Beans 64.08 %

  20. 18. After counting and massing 3 types of beans a student made the following data table. Bean 1 Bean 2 Bean 3 TotalCount 22 15 66 103 % abundance 21.36 14.56 64.08 100.00total mass of beans(g) 7.558 9.441 6.888 Xaverage mass of bean (g) What is the average mass of Bean 1? 7.558 g = 22 beans 0.3435 g/bean

  21. 19. After counting and massing 3 types of beans a student made the following data table. Bean 1 Bean 2 Bean 3 TotalCount 22 15 66 103 % abundance 21.36 14.56 64.08 100.00total mass of beans(g) 7.558 9.441 6.888 Xaverage mass of bean (g) 0.3435 0.6294 0.1044 X What is the weighted average mass of ALL beans? 0.6294 g X 0.1456 % 0.1044 g X 0.6408 % 0.07337 g 0.3435 g X 0.2136 % 0.09164 g 0.06690 g = = + 0.07337 g = 0.09164 g 0.06690 g = 0.2319 g Don’t for get to turn the % into a decimal! Example: 21.36% = 0.2136 decimal

  22. 20. Element X has two isotopes. If 72.0% of the element has an isotopic mass of 84.9 atomic mass units (amu), and 28.0 % of the elements has an isotopic mass of 87.0 atomic mass units, what is the average atomic mass of element X ? • 86.0 amu • 100.0 amu • 171.9 amu • 85.5 amu • 1.719 amu Isotope # 1 Isotope # 2 84.9 amu X 0.720 % 87.0 amu X 0.280 % = = 24.36 amu 61.13 amu 85.5 g 61.13 amu + 24.36 amu =

  23. 21. What is the average atomic mass of element X if a sample is composed of 85% , 12% , and 3.0% ? • 130 amu • 127.0 amu • 127.4 amu • 128.3 amu • 128.8 amu Isotope # 1 Isotope # 2 Isotope # 3 127 amu X 0.85 % 130 amu X 0.12 % 128 amu X 0.030 % = 110 amu = = 16 amu 3.8 amu 130 amu 110 amu 16 amu 3.8 amu + = +

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