eday Lessons Chemistry Day Two Name: Instructor: School:
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1 Day Two Name: Instructor: School:
2 Topic: Nuclear Academic Learning Targets Compare the potential dangers to society from the release of different types of radiation (alpha, beta, gamma, and positron) including mass, charge, potential to ionize, ability to penetrate and origin. Predict the products of a radioisotope undergoing decay and balance the resulting nuclear equation. Evaluate the advantages and disadvantages of fission and fusion reactions as a source of energy for society. Task Day Two: Radioactive Decay Read the article from INFOhio: you can also refer to pages in Prentice Hall:. Work through worksheet 1: Transmutation Columbus City Schools Page 2 of 5
3 Day 2: Reading Instructions: Read the article from INFOhio at: Day 2: Transmutation Transmutation is the process by which an element, undergoing radioactive decay, transforms from one element into another element. Transmutation is not a chemical change but rather a nuclear change. In a nuclear equation we introduce a few new particles that are not used in a chemical equation. The common particles such as the beta particle: ; the alpha particle: (which is just a helium-4 atom); and the neutron:. There are also less often used particles like the positron: ; the proton: which is a hydrogen-1 nucleus and the gamma ray: which is just energy Nuclear equations are written similar to a chemical equation. For example the nuclear equation for carbon-14 undergoing transmutation into nitrogen-14 would be written like this: In a nuclear equation the sum of atomic mass numbers of the products should equal the sum of atomic mass numbers of the reactants. In looking at the above equation the atomic mass number of carbon (the reactant ) is 14 the atomic mass number for the nitrogen and the is = 14, the same as the carbon. The same is also true for the atomic number. So how do we write a balanced nuclear equation. So let s look at the example of oxygen-19 which undergoes beta decay. First thing we would do is write down the isotope s symbol. Step 1 Now oxygen has eight (8) protons and eleven (11) neutrons. Next thing we do is determine the type of decay. In this case the problem told us that oxygen is undergoing beta decay. Beta decay means that the particle is releasing a beta particle. A beta particle is an electron and is written using the following symbol. Step 2 Remember an electron has very little mass so it is given an atomic mass number of zero (0) and since it has a -1 charge it is given an atomic number of -1. (Continued on the next page) Columbus City Schools Page 3 of 5
4 Now, we need to use the information we have been given to figure out the missing piece the daughter element (the daughter element is the element created by the nuclear decay). Step 3 So, we know that in a nuclear equation the sum of the atomic numbers on the right of the arrow should equal the sum of the atomic numbers on the left of the arrow we determine the missing number. Step 4 Solving for x, we determine that the atomic mass number of the missing element is 19. Now for the atomic number. Since the atomic number has to also be equal on both sides of the equations so therefore: Step 5 Solving for x, we determine that the atomic number is 9. Looking on the periodic table, an atomic number of 9 means that we have fluorine. Putting this information together the nuclear equation for the beta decay of oxygen is: Step 6 Now for some practice. For the following predict the missing piece: Columbus City Schools Page 4 of 5
5 If all went well then you should have gotten,, and. Now you are ready for the real deal. Instructions: Each of the following statements has a missing piece of information. Write the nuclear equation including the missing piece. 1. Aluminum-26 is a long-lived isotope of aluminum (half-life of 7.17x10 5 years) undergoes positron decay. 2. Chlorine-36 undergoes beta-decay. 3. The most common isotope of copper that undergoes radioactive decay is copper-64 which can undergoes beta decay or positron emission. Write both decay equations. 4. Uranium has no stable isotopes but a number of its isotopes have very long half-lives. The most common isotope of uranium is uranium-238 which transmutes to thorium Arsenic-74 decays into selenium-74 Columbus City Schools Page 5 of 5
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