Mastery Quiz #4: Atomic Structure
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1 Mastery Quiz #4: Atomic Structure Multiple Choice: 1. The literal translation to English of the Greek word atomos (ατομως) is a. Particle b. Indivisible c. Tiny d. Anti æther 2. Which of the following arranges the subatomic particles in order of increasing mass? a. Electron, proton, neutron b. Neutron, proton, electron c. Electron, neutron proton d. None of the above 3. Which of the following is the correct nuclear notation for an isotope with seven protons and eight neutrons? a. b. c. d. 4. Which of the following best captures the chronological order of the development of atomic theory up to the Nuclear Model theory? a. Democritus, Dalton, Thompson, Millikan, Chadwick, Thompson, Rutherford b. Democritus, Dalton, Thompson, Millikan, Chadwick, Rutherford, Thompson c. Democritus, Thompson, Dalton, Millikan, Chadwick, Rutherford, Thompson d. Democritus, Thompson, Dalton, Millikan, Chadwick, Thompson, Rutherford 5. One fluorine isotope has ten neutrons and 9 protons. What is this isotope s mass number? a. 9 b. 10 c. 19 d mass of the electrons 1
2 6. Dalton, among others, had shown that the atom was neutral. The cathode ray tube experiment, however, showed that the atoms were attracted to the positive end of the tube and repelled by the negative end. How did Thompson reconcile these seemingly divergent results? a. Thompson argued that Dalton and others were wrong. Atoms were negatively charged. b. Thompson argued that his own results were wrong and re worked his experiment until he found results that comported with the widely accepted theory. c. Thompson argued that Dalton was wrong about the indivisibility of atoms. Thompson theorized that atoms had to be made up of smaller, charged particles. d. Thompson found a design flaw in the cathode ray tube experiment, thus vindicating Dalton. 7. Which of the following has the most mass? I. Hydrogen 1 II. Proton III. Electron a. I only b. III only c. I and II only d. II and III only 8. Electrons, protons, and neutrons have which of the following charges? a. 1+, 0, 1, respectively b. 1, 0, 1+, respectively c. 1, 1+, 0, respectively d. 1+, 1, 0, respectively 9. What best explained the results of Rutherford s gold foil experiment? a. Electrons were negatively charged particles. b. Atoms were not indivisible and, in fact, were made up of subatomic particles. c. Atoms were neutrally charged. d. Regions of the atoms had to have different charges. 10. Krypton 84 has how many protons, neutrons, and electrons? a. 84, 168, and 84, respectively b. 36, 48, and 36, respectively c. 168, 84, and 84, respectively d. 48, 36, and 36, respectively 2
3 Problems: Show your work for each. You must provide the analysis, solution, and evaluation for each problem in order to earn full credit. The prompt is provided for you. Use sig figs and units! 11. Naturally occurring copper is composed of 69.17% of copper 63, with an atomic mass of u, and 30.83% of copper 65, with an atomic mass of u. What is the average atomic mass of copper? 12. Naturally occurring magnesium is composed 78.99% magnesium 24, which weighs u, 10.00% magnesium 25, which weighs u, and 11.01% magnesiums 26, which weighs u. Calculate the average atomic mass of magnesium. 3
4 13. Rubidium has two naturally occurring isotopes: rubidium 85 at u and rubidium 87 at The former is more abundant than the latter by 44.30%. What is the average atomic mass of rubidium? 14. Naturally occurring bromine is composed of two isotopes: bromine 79, with a mass of u, and bromine 81, with a mass of u. Given that the average atomic mass of bromine is u, determine the relative abundance of each of its naturally occurring isotopes. 4
5 15. A randomly selected sample of 2.00 x 10 2 atoms contains four types of atoms. There are 157 atoms with 14 protons and an atomic mass of u. There are eight atoms with 14 protons and an atomic mass of u. There are five atoms with 14 protons and an atomic mass of u. Finally, there are 30 atoms with 16 protons and an atomic mass u. What is the average atomic mass of the element with more than one isotope in the sample? (Note: round your final answer to the hundredths place.) What is the most likely identity of the element given the calculated atomic mass? 5
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