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Unit 2: the Atom Day Page # Description IC/HW Due ? Date: Done? Webquest: Atomic Theories and 0 X IC/HW Models Name: ______________________________ Period:_______________ Unit 2: The Atom Day Page # Description IC/HW Due ? Date: Done? WebQuest: Atomic Theories and 0 X IC/HW Models 1 3 Atomic Models Summary Table IC The Atom and Average Atomic 1 4-6 IC Mass Notes 2-A: Atomic Structure and 1 9-10 HW Day 2 Average Atomic Mass Worksheet 2-V1: The Atom and Average 1 VISION HW Atomic Mass HW Radioactive Decay and Half-life 2 6-8 IC Notes 2-B: Radioactive Decay and Half 2 11-12 HW Day 3 Life Worksheet 2 13-16 Unit 2 Review HW 4 Unit 2 Quiz Unit 2 1 Atomic Models Summary Table Name Characteristics Picture Dalton Electrons: (marble model) Protons: Neutrons: Other: Thomson Electrons: (plum pudding model) Protons: Neutrons: Other: Rutherford Electrons: (planetary model) Protons: Neutrons: Other: Bohr Electrons: (quantum model) Protons: Neutrons: Other: Important Scientists in the Atomic Theories and Models -atomos, initial idea of atom – Democritus - first atomic theory of matter, solid sphere model – John Dalton - discovery of the electron using the cathode ray tube experiment, plum pudding model – J. J. Thomson - discovery of the nucleus using the gold foil experiment, nuclear model – Ernest Rutherford - discovery of charge of electron using the oil drop experiment – Robert Millikan - energy levels, planetary model – Niels Bohr - periodic table arranged by atomic mass – Dmitri Mendeleev - periodic table arranged by atomic number – Henry Moseley - quantum nature of energy – Max Planck - uncertainty principle, quantum mechanical model – Werner Heisenberg - wave theory, quantum mechanical model – Louis de Broglie. Unit 2 2 The Atom- Notes - Atoms are the basic unit of ______________ and is made up of ______________________ particles Atomic Subatomic Proton Neutron Electron Particles Where is it? Mass Charge Influence (What happens if you change it?) Atomic Number – the number of _______________ in an element Mass Number – the number of ______________ and ____________ in an element Isotope – Atoms of an element with different number of __________________ , giving it a different _________________ but the same ___________________. AMU - ____________ ______________ ___________; used to describe the mass of subatomic particles Standard nuclear notation is used to represent each isotope in existence. 퐴 푍푋 Write the symbol for the atom that has an atomic number of 9 and a mass number of 19. How many protons, neutrons and electrons does this atom have? Unit 2 3 How many protons, neutrons and electrons does this atom have? Isotope Protons Neutrons Electrons Oxygen-16 Hydrogen-2 Carbon-13 Nitrogen-15 Average Atomic Mass- Notes The mass of each element is a ___________________________________ of the isotopes in the element. Example 1: Silicon has three stable isotopes. The following information is available for the three isotopes: Fractional Relative Relative Mass Isotope Mass (amu) Abundance (%) Abundance (amu) Silicon-28 27.977 92.21 Silicon-29 28.976 4.70 Silicon-30 29.974 3.09 Example 2: Element J has four stable isotopes. The following information is available for the four isotopes. Determine the average atomic mass and identity of element J. Isotope Mass (amu) Fractional Abundance (%) J-54 53.9396127 5.845 J-56 55.9349393 91.754 J-57 56.9353958 2.119 J-58 57.9332773 0.282 Unit 2 4 Example 3: The two naturally occurring isotopes of chlorine are 35Cl with a mass of 34.9689 amu and 37Cl with a mass of 36.9659 amu. The atomic mass of elemental chlorine on earth is found to be 35.46 amu. Calculate the percent abundance of each of the two chlorine isotopes. Average Atomic Mass Practice: 1. Find the average atomic mass for Li if 7.50 % of Li atoms are 6-Li with a mass of 6.01512 amu and 92.5% are 7-Li with a mass of 7.0160 amu 2. Find the average atomic mass for element M if 19.9% of M atoms have a mass of 10.0129 amu and 80.1% are 11.0093 amu. Determine the identity of element M. 3. Europium has two stable isotopes: 151Eu with a mass of 150.9196 amu and153Eu with a mass of 152.9209. If elemental Europium is found to have a mass of 151.96 amu on earth, calculate the percent of each of the two isotopes. Unit 2 5 Radioactive Decay Notes The stability of a nucleus is dependent on the ratio of neutrons to protons (N:Z). For light nuclei (atomic number of 20 and less), the N:Z ratio should be 1:1. For heavy nuclei (above 20), the N:Z ratio should be 1.5:1. Band of Stability Atoms that lie either above or below the band of stability will undergo nuclear decay to achieve stability. Atoms that lie ABOVE the band of stability have ________ ______________________________________________. Atoms that lie BELOW the band of stability have _______ ______________________________________________. Beta Decay: Atoms that lie above the band of stability will undergo beta decay. The source of the beta particle is a neutron. Beta decay will increase the number of protons. Beta Decay of Carbon-14: Alpha Decay: Atoms with more than 83 protons will decay automatically. The number of neutrons and protons need to be reduced. An alpha particle is the same as the nucleus of a helium atom. Alpha Decay of Polonium-210: Unit 2 6 Positron Emission: Isotopes that lie below the band of stability will undergo positron emission. The source of a positron is a proton. The number of protons will decrease. Positron Emission of Carbon-11: Electron Capture: Isotopes that lie below the band of stability can undergo electron capture. A proton incorporates an inner shell electron and forms a neutron. This will decrease the number of protons. Electron Capture of Aluminum-26: Gamma Radiation: A release of energy, no change in mass occurs. There is no charge. Gamma rays are assumed to be released in all forms of decay. Radiation Change in Change in Particle Mass Charge Type Mass # Atomic # Decrease Decreases Alpha Decay by 4 by 2 No Increases Beta Decay Change by 1 Positron No Decreases Emission Change by 1 Electron No Decreases Capture Change by 1 Gamma No N/C Radiation Change Unit 2 7 Half-life Notes - Every radioisotope has a characteristic rate of decay - Half-life is the time required for one half of a radioisotope’s nuclei to decay After each half life of a radioisisotope, half of the original radioactive atoms have decayed into atoms of a different isotope (or atom) Formula for calculating half-lives: mf: mo: t: t1/2: n: Example 1: Fluorine-21 has a half-life of 5.0 seconds. If you start with 25 g of fluorine-21, how many grams would remain after 60.0 s? Unit 2 8 2-A: Atomic Structure Worksheet Complete the table and then answer the questions below: Element Symbol Protons neutrons electrons Atomic # Mass # Hydrogen 1 1 H-2 Helium 2 4 Mg-24 Carbon 6 6 H-3 Oxygen 8 8 Cl-36 Neon 10 10 20 Aluminum 13 27 O-18 238 U92 Mg2+ 24 Cl- 35 Zinc 30 30 65 Rb+1 85 P-3 31 1. What is the mass number of carbon? 2. What is the atomic number of oxygen? 3. How many electrons does an atom of aluminum contain? 4. An atom of which element contains two neutrons? 5. Which element has mass number of 16? Unit 2 9 2-A: Average Atomic Mass Worksheet: 6. There are 2 isotopes of copper that occur naturally; 63Cu and 65Cu. The63Cu atoms have a mass of 62.929601 amu and the 65Cu atoms have a mass of 64.927794 amu. What is the percent natural abundance for each isotope? 7. There are 2 isotopes of gallium that occur naturally; 69Ga and 71Ga. The 69Ga atoms have a mass of 68.925581 amu and the 71Ga atoms have a mass of 70.924707 amu. What is the percent natural abundance for each isotope? 8. Iridium is composed essentially of two isotopes: 191Ir and 193Ir. The average mass of an iridium atom is 192.217 amu. Determine the natural abundance of each of these isotopes in a naturally occurring sample. (The mass of an 191Ir atom is 190.961 amu, and the mass of an193Ir atom is 192.963 amu.) Unit 2 10 2-B: Radioactive Decay and Half Life Worksheet Write the reaction that represents the following: 1. Alpha decay of Polonium – 218. 2. Electron capture of Promethium – 142. 3. Beta decay of Potassium – 43. 4. Alpha decay of Uranium – 233 5. Beta decay of Nitrogen – 13. 6. Positron emission of Carbon – 14. 7. Alpha decay of astatine – 196. 8. Electron capture of mercury – 201. 9. Alpha decay of Radon – 226. 10. Beta decay of Iodine – 136. Unit 2 11 2-B: Complete the following half-life problems. Show ALL work. 11. The half-life of plutonium – 239 is 24,100 years Of an original mass of 100. g, how much remains after 96,440 years? 12. Exactly 1/16 of a given amount of protactinium-234 remains after 26.76 hours. What is the half life of protactinium – 234? 13. How many milligrams remain of a 15.0 mg sample of radium – 226 after 6396 years? The half-life of radium – 226 is 1599 years. 14. Technetium – 99 has been used as a radiographic agent in bone scans. If 99Tc has a half-life of 6.0 hours, what fraction of the administered 100.0 g dose will remain after 2.0 days? Unit 2 12 Unit 2 Review: Matching: Match the person in column B to the experiment, discovery or model in column A.
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