) The nucleus of an atom, when compared to the entire atom, is (Circle two).

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1 Unit 3: The Atom Review Packet Directions: Answer the following questions WITHOUT using your notes first. This will be a great way to study for your test. Then, get out your notes and go back and fill in the answers you didn t already know. This is the material that you should study harder for your test! 1) Match each scientist below with their main contribution to the Atomic Model. You may use some scientists more than once, and some scientists may not be used at all. 1. discovered e- 2. discovered mass of e- 3. gold foil experiment 4. first theory of atoms 5. first MODERN atomic theory 6. discovered nucleus 7. plum pudding atomic model Democritus Crookes John Dalton Lavoisier J.J. Thomson Millikan Rutherford ) In Rutherford s gold foil experiment, most of the alpha particles passed through the foil. Why?? (Circle TWO answers). The atom is mostly empty space. The atom has no empty space. The atom has a negative nucleus. The atom has a positive nucleus. 3) The nucleus of an atom, when compared to the entire atom, is (Circle two). Large Contains most of the atom s mass Small Contains little of the atom s mass

2 4) Dalton s atomic theory states that atoms cannot be divided into smaller parts. What is wrong with this statement? He also states that all atoms of the same element are identical (same size, mass, chemical properties). What is wrong with that statement? 5) Cathode rays are attracted to a positive plate in the cathode ray tube. Therefore, cathode rays are composed of. (Circle your answer below) Uncharged particles Positive particles Negative particles No particles 6) In the space below, create a timeline that shows the development of the Atomic Model throughout history! You should include the name of each scientist we have discussed AND what their main contribution to the Atomic Model was. You DO NOT need to include dates, but your order should be correct. 7) What does the atomic number of an atom tell us? 8) What does the mass number of an atom tell us? 9) How can you determine the number of neutrons in an atom if you know the atomic number and mass number? Write a mathematical equation.

3 10) Complete the table below using your periodic table. Element Name Atomic Number Number of Protons Number of Neutrons Name: Mass Number Cobalt Potassium Iodine Lead Sodium ) How many electrons are in Argon-40? Protons? Neutrons? 12) How many electrons are in Xenon-130? Protons? Neutrons? 13) How many electrons are in Oxygen-18? Protons? Neutrons? Isotope Symbol 1 1H 32 16S U 19 9F Es

4 14) What is the mass number of an atom with 40 protons, 40 neutrons, and 38 electrons? 15) Which atom has a nucleus that contains 5 protons and 6 neutrons? (Circle one) Be Na C B 16) An atom s nuclear charge refers to the number of protons in the NUCLEUS ONLY!! So which of the following nuclides has the greatest nuclear charge? (Circle one) Nitrogen-14 Carbon-12 Hydrogen-1 Helium-4 17) Compared to an atom of nitrogen-15, an atom of oxygen-16 contains (Circle one). One less neutron One less proton One more neutron One more proton 18) Atoms of oxygen-16, oxygen-17 and oxygen-18 have the same number of but a different number of. 19) What particles make up the mass (protons and/or neutrons) of the following elements? Hydrogen-1: Hydrogen-2: Hydrogen-3: 20) What is the total number of electrons in a neutral atom of phosphorus? Sulfur? 21) Base your answers to this question on the diagrams below. What is this atom s atomic number? What is this atom s mass number? What is this atom s atomic number? What is this atom s mass number? 22) A sample of element X contains 95% X-75 atoms, 3.0% X-77 atoms and 2.0% X-78 atoms. The average isotopic mass is closest to. (Circle one)

5 23) Uranium has 3 major isotopes: Uranium-238 (99.28% natural abundance), Uranium-235 (0.71% natural abundance), and Uranium-234 (0.0054% natural abundance). What is the average atomic mass of Uranium? 24) Neon is used in lighted signs (mostly Open signs) and has 3 isotopes: Neon-20 (98.48% abundant), Neon-21 (0.27% abundant), and Neon-22 (9.25% abundant). What is its average atomic mass? 25) Tungsten has 5 stable isotopes: W-180 (0.135%), W-182 (26.41%), W-183 (14.4%), W-184 (30.64%), and W-186 (28.41%). Calculate the average mass of Tungsten. 26) Complete the following nuclear equation: Th 88Ra _ Is this an alpha particle, beta particle, gamma ray, or neutron? 27) Complete each nuclear reaction by filling in the blank space Po Ra Np Pb 4 2He 1 0 e He U Pa Th Np 1 0 e 28) The half-life of a radioactive substance is 20 minutes. What fraction of this substance will remain after 80 minutes? (Circle one) 1/2 1/4 1/8 1/16

6 29) Manganese-56 is a beta emitter with a half-life of 2.6 hours. What is the mass of manganese-56 in a 1.0 mg sample of the isotope at the end of 10.4 hours? 30) A mg sample of hydrogen-3 was collected. After years, mg of the sample remains. What is the half-life of hydrogen-3? 31) Iodine-131 is a major contributor to the birth defects found from Chernobyl. If 100 g were formed from nuclear fallout from the reactor, how much will be around after 32 days if its half-life is 8 days? 32) A radioactive isotope that has a half-life of 5 years is used to irradiate (sanitize with radiation) space steaks. If the steaks are safe for consumption after 15 years, what is the fraction of the radioisotope that is safe to consume? 33) Chemical reactions release energy but fission reaction (splitting the atom like in the A-bomb) releases a greater amount of energy because of E = mc 2. What is happening? (Circle one) Energy is converted into mass 34) Draw fission (heavier isotope to lighter isotope). Mass is converted into energy 35) Draw fusion (lighter isotopes to heavier isotopes).

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