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Station 1: Parts of an Atom PART I: Model of an Atom Make an atom of Boron-10 by placing the correct number of subatomic particles on the diagram. Use a different color for each subatomic particle. Nucleus Key: = protons = neutrons = electrons PART II: Questions 1. Which particles make up most of the mass of the atom? 2. Most of the volume of the atom is ______ . a. Neutrons b. Protons c. empty space d. electrons 3. Most of the mass of the atom is due to __________. I. Nucleus IV. Electrons II. Protons V. Electron Cloud III. Neutrons a. I, II, and III b. I and V c. I, II, and IV d. IV and V 4. What is the charge of the nucleus? ____________ 5. What is the charge of the electron cloud? __________ 6. How does the mass of an electron compare to the mass of a proton or neutron? 7. Which two particles will always occur in the same numbers in a neutral atom? Station 2: Calculating Protons, Neutrons, and Electrons An atom with a mass of 65 amu and an atomic number Copper-65 of 29 An isotope with 33 protons, 42 neutrons, and 33 Arsenic-75 electrons An atom that contains 64 neutrons and has a mass of Indium-113 113 amu An atom with a nucleus that contains 80 protons and 118 Mercury-198 neutrons An isotope that is made up Antimony-121 of 51 electrons and 51 protons An atom that has 72 Tin-122 neutrons and 50 electrons Lithium-6 Helium-4 Lithium-7 Sodium-23 Station 3: Isotopes 1. Isotopes are atoms of an element with identical chemical properties but with different a. numbers of protons. b. masses. c. numbers of electrons. d. atomic numbers. 2. The reason isotopes have different masses is because they have different numbers of a. protons b. electrons c. neutrons d. energy levels 3. Isotopes of the same element must have the same number of a. protons b. electrons c. neutrons d. energy levels 4. The weighted average of the masses of the stable isotopes of an element as they occur in nature is called the a. atomic number. b. atomic mass. c. atomic weight. d. mass number. 5. The isotope shown above has ____ protons ____ electrons, ____ neutrons, and a mass number of ______. 6. Which of the following are isotopes of each other? (There are 2 pairs of isotopes and one that is not an isotope of any of the others.) I. An atom with 17 protons and 18 neutrons II. An atom with an atomic number of 16 and 18 neutrons III. An atom with 17 protons and 20 neutrons IV. An atom with an atomic number of 16 and an atomic mass of 33 V. An atom with 15 protons and 16 neutrons _____ and _____ are isotopes of each other _____ and _____ are isotopes of each other Station 4: Average Atomic Mass 1. Boron has two naturally occurring isotopes with masses of 10.0129 amu (19.91% abundance) and 11.0093 amu (80.09% abundance). Calculate the average atomic mass of boron. 2. Calculate the average atomic mass of silicon based on the following information: 3. Bromine has two isotopes with the first having a mass of 78.918336 amu (50.69% abundance) and the second isotope having a mass of 80.916289 amu (49.31% abundance). What is the average atomic mass of bromine? 4. The following data was collected for an unknown element. 34.96885 amu and percent abundance of 75.77% 36.96590 amu and percent abundance of 24.23% a. What is the average atomic mass for this element? b. What is the identity of the element? 5. Two isotopes of potassium exist in nature: potassium-39 and potassium-41. Potassium has an atomic mass of 39.0983 amu. Which isotope of potassium is more abundant in nature? Justify your answer. Station 5: Radioactive Particles Alpha Particles Beta Particles 1- charge Electron 2+ charge No charge Helium Nucleus 0.0055 amu Stopped by paper, wood, cloth, etc. Least dangerous to humans Gamma Radiation Electromagnetic Radiation 4 amu 0 amu Stopped by aluminum or other metals Most dangerous to humans Stopped by lead Label each particle that would be stopped by skin, aluminum, and lead. 1. The mass of two protons is approximately equal to the mass of a. an alpha particle b. a positron c. a beta particle d. a neutron 2. Compared to the mass and the penetrating power of an alpha particle, a beta particle has a. less mass and greater penetrating power b. less mass and less penetrating power c. more mass and greater penetrating power d. more mass and less penetrating power 3. Which particle has the least mass? a. alpha particle b. neutron c. beta particle d. proton 4. Which of the following types of radiation is composed of particles with a charge and mass identical to that of an electron? a. a l p h a p a r t i c l e s b. b e t a pa r ti c l es c. g a m m a r a d i a t i o n d. X - r a y s 5. In a. b. c. d. 6. Which of the following statements concerning the penetrating power into matter of various types of radiation is CORRECT? a. Alpha and beta particles penetrate equally. b. Alpha particles penetrate deeper than beta particles. c. Alpha particles and gamma radiation penetrate equally. d. Gamma radiation penetrates deeper than alpha particles. terms of subatomic particles, the composition of an alpha particle is three neutrons and a proton. two neutrons and two protons. one neutron and three protons. one neutron and two protons. Station 6: Balancing Nuclear Equations For each of the statements below write out the decay equation using the cards provided. Remember that the nuclear reactions must be balanced in terms of mass and atomic number. 1) Alpha decay of uranium-233 2) Beta decay of carbon-14 3) Beta decay of nitrogen-16 4) Alpha decay of platinum-192 5) Beta decay of phosphorus-32 6) Alpha decay of radium-226 with gamma emission 229 90 Th 14 6 C 0 1 0 1 32 15 32 16 4 2 He 14 7 N e 192 78 e 0 1 P S 4 2 4 2 Pt 233 92 U 16 8 O 0 0 e 188 76 Os He 226 88 Ra He 222 86 Rn 16 7 N + + + + + + Balancing Nuclear Equations Answer Key 233U229Th 4 He 1) 92 90 2 2) 14C14 N 0e 6 7 1 16 N 0 e16O 3) 7 -1 8 192Pt 4 He188Os 4) 78 2 76 32P 0 e32S 5) 15 - 1 16 226 Ra4 He222Rn 0 6) 88 2 86 0 Station 7: Fusion vs. Fission 1. Given the balanced equation representing a nuclear reaction: 2H 3H4 He1n 1 1 2 0 Which phrase identifies and describes this reaction? a. fission, mass converted to energy b. fission, energy converted to mass c. fusion, mass converted to energy d. fusion, energy converted to mass 2. During a nuclear reaction, mass is converted into a. Charge b. Isomers c. Energy d. Volume 3. Which type of reaction releases the greatest amount of energy per mole of reactant? a. combustion b. nuclear fission c. nuclear fusion d. oxidation-reduction 4. What type of nuclear reaction occurs in the sun? a. nuclear fission b. nuclear fusion 5. What type of nuclear reaction occurs in a nuclear reactor? a. nuclear fission b. nuclear fusion 6. Label the following illustrations as fission or fusion. a. b. Station 8: Half-Life 1. After 4 half-lives have elapsed, the amount of a radioactive sample which has NOT decayed is a. 1/4 the original amount b. 1/8 the original amount c. 1/16 the original amount d. 1/32 the original amount 2. Radioisotopes used in diagnostic medical procedures are usually a. Radionuclides with short half-lives. b. Radionuclides with long half-lives. Explain your answer. 3. Are isotopes with short half-lives or long half-lives more stable? Justify your answer. 4. Use the graph to the below to answer the following questions. a. What is the half-life of for the unknown isotope? b. What mass of the unknown isotope will remain after 300 years? c. How much time would it take for 20 g of the unknown isotope to decay?