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Transcript
NAME________________________________________________ PERIOD_______________ DATE__________________________ Isotopes and Radioactive Decay CHAPTER 4 NOTES: ISOTOPES ISOTOPES: Atoms that contain the same number of ______________ but a different number of ______________. Isotopes containing more neutrons have a _____________________________ mass. Despite the difference in mass, isotopes of an atom will have the ____________ chemical ____________. Generally in nature most elements are found as ______________________ of ______________________. An example of this can be found with the Potassium (K) in a banana. 93.26% of the potassium __________ have 20 _________________, 6.73% of the potassium atoms have ________ neutrons, and 0.01% of the potassium atoms have 21 ______________________. ATOMIC MASS: The weighted _________________ mass of the _________________ of a certain _____________. Atomic mass is expressed in units of ________________________________________, which is defined as the one-twelfth the mass of a _____________________________ atom. 1 amu is nearly equal to the mass of a single _____________________ or a single _________________________. ISOTOPE/NUCLEAR NOTATION: ISOTOPE/NUCLEAR NOTATION FOR THE 3 ISOTOPES OF HYDROGEN: Given the data in the table, calculate the atomic mass of unknown Element X: ISOTOPE ABUNDANCE FOR ELEMENT X Isotope Mass (amu) Percent abundance 6X 6.015 7.59% 7X 7.016 92.41% Ex #1): Write nuclear symbols for 3 isotopes of carbon (atomic number = 6) in which there are 6, 7, and 8 neutrons respectively. Ex #2): A radioactive isotope that is used for radiation treatment of cancer is the Cobalt – 60 atom. How many protons are there? How many neutrons are there? RADIOACTIVE DECAY NUCLEAR REACTION: Reaction that can change an _______________________into a new ___________________. It requires a change in an atom’s _______________________________. Radiation is the ____________________ and ______________________ emitted by radioactive materials. Radioactive ______________ emit radiation because their _______________ are ___________________. Radioactive decay is a ____________________________ process in which unstable nuclei _____________ energy by emitting ___________________________. Radioactive decay will continue to occur until a stable _________________ has formed, which is often a different _____________________ altogether. The most important factor in determining an atom’s stability is its _________________ of _____________ to _____________________. Nuclei are unstable when there are either too many or too few of protons or neutrons. Types of Radiation: o ALPHA RADIATION: Radiation that is made up of ____________________________ particles. An ______________________ particle contains _____________ protons and ____________ neutrons and has a ______________ charge. An alpha ________________ is equivalent to a ____________ nucleus. Alpha particles are represented by _____________________ or ___________________. o Example of alpha radiation (the following equation is an example of a nuclear equation): BETA RADIATION: Radiation that is made up of _______________________ particles. A _____________ particle contains an ___________________ with a ___________ charge. Beta particles are _____________________________________. Beta particles are represented by the symbols ________________________ or __________________________. o Example of beta radiation (the following equation is an example of a nuclear equation): GAMMA RADIATION: Radiation that is made up of ________________________ rays. A gamma ray is high-energy and contains no _____________ and is represented by the symbol __________. Gamma rays usually accompany ___________________ and ___________________ radiation. Gamma rays also account for ______________ of the __________________ lost during _________________________ decays. Since gamma radiation is massless the ________________ of gamma rays cannot end in the ____________________ of a new _______________. Example of gamma radiation (the following equation is an example of a nuclear equation): Characteristics of Radiation: Alpha Beta Gamma Symbol Mass (amu) Charge HOMEWORK PRACTICE PROBLEMS: 1. Which subatomic particle identifies an atom as that of a particular element? 2. An element contains 66 electrons. Which element is it? 3. An element contains 14 protons. Which element is it? 4. Boron (B) has two naturally occurring isotopes: boron-10 (abundance = 19.8%; mass = 10.013 amu) and boron-11 (abundance = 80.2%; mass = 11.009 amu). Calculate the atomic mass of boron. 5. Copper has two isotopes: Cu-63 (abundance = 69.2%; mass = 62.930 amu) and Cu-65 (abundance = 30.8%; mass = 64.928 amu). Calculate the atomic mass of copper. 6. Three magnesium isotopes have atomic masses and relative abundances of 23.985 amu (78.99%), 24.986 amu (10.00%), and 25.982 amu (11.01%). Calculate the atomic mass of magnesium. 7. Nitrogen has two naturally occurring isotopes, N-14 and N-15. Nitrogen’s atomic mass is 14.007. Which isotope is more abundant and WHY? 8. Boron-10 emits alpha particles. Write a balanced nuclear reaction for this radioactive decay. 9. Cesium-137 emits beta particles. Write a balanced nuclear reaction for this radioactive decay. 10. Iodine-121 emits alpha particles. Write a balanced nuclear reaction for this radioactive decay.