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Station 1: Isotopes All atoms of the same element have the same number of protons, but the number of neutrons may vary. Isotopes are atoms of the same element, which have different numbers of neutrons. Complete the following table for the 3 commonly occurring isotopes of oxygen. Isotope Nuclear Symbol Number of Protons Number of Electrons Number of Neutrons Mass Number Mass (amu) Oxygen – 16 15.99415 Oxygen – 17 16.999131 Oxygen - 18 17.999160 What structural characteristics do all oxygen atoms have in common? What differences exist between the isotopes of oxygen? The isotopes of an element do not differ significantly in their chemical behavior. Why do you think this is so? Station 2: Atomic Mass and Percent Abundance The average atomic mass for an element is given on the periodic table, but how was it determined? In order to calculate the average atomic mass for an element, you must know the percent abundance and atomic mass for each of the isotopes of that element. Example Problem Isotope Atomic Mass Percent Abundance Oxygen – 16 15.99415 amu 99.762% Oxygen – 17 16.999131 amu 0.038% Oxygen – 18 17.999160 amu 0.200% The average atomic mass of oxygen is given as 15.999 amu on the periodic table. Let’s see how that was calculated 15.99415 amu x (99.762 / 100) = 15.95608 amu 16.99415 amu x (0.038 / 100) = 0.0064597 amu 17.99160 amu x (0.200 /100) = 0.03598 amu 15.95608 amu + 0.0064597 amu + 0.03598 amu = 15.999 amu A certain element exists as three natural isotopes as shown in the table below. Isotope Mass (amu) Percent Abundance Mass Number 1 19.99244 90.51 20 2 20.99395 0.27 21 3 21.99138 9.22 22 Calculate the average atomic mass of this element to the nearest thousandth. Identify the Element. Station 3: Isotopes and Abundance Carbon has three naturally occurring isotopes: Carbon-12 (12.000 amu), Carbon-13 (13.003 amu), and Carbon-14 (14.003 amu). Based upon the average atomic mass of carbon (12.011 amu), which isotope of carbon do you think is the most abundant in nature? Explain your answer. An element has two naturally occurring isotopes. The mass of the first isotope is 64.9278 amu and the mass of the second isotope is 62.9296 amu. The average atomic mass of the element is 63.546 amu. Calculate the percent abundance of each isotope to two decimal places. Let x = the percent as a decimal of the first isotope. 1-x = the percent as a decimal of the second isotope Station 4: Beanium Review Period 1 and 4: Take time now to make sure your data table is complete for your Beanium activity we completed on Friday. If you did not get mass make sure to get that information from a classmate now. Check your calculations. Based on the lab activity answer the following question: How did the Beanium lab represent different isotopes of an atom? How were the isotopes used to calculate the average atomic mass written on the periodic table? Using the average atomic mass you calculated create a periodic table symbol of Beanium – abbreviation Bu (include atomic number, symbol, and average atomic mass) Indicate which elements it would be near on the periodic table if added. Period 3: the data is being provided to you now. Complete the calculations for the Beanium activity using the instructions provided. Based on the lab activity answer the following question: How did the Beanium lab represent different isotopes of an atom? How were the isotopes used to calculate the average atomic mass written on the periodic table? Using the average atomic mass you calculated create a periodic table symbol of Beanium – abbreviation Bu (include atomic number, symbol, and average atomic mass) Indicate which elements it would be near on the periodic table if added. Station 5: Cl-Ev-R summary of Beanium Use the following format to create a lab summary report based on your Beanium Lab : How do the different beanium isotopes represent an isotope in real life ? Start your Claim based on what you know about Isotopes. This Report is due on Friday September 13, 2013. Each Table should translate into a paragraph. It must be TYPED, Times New Roman, 12 font, Double spaced. Remember your title requirement in your syllabus. Station 6: Ions Ions are formed when an atom gains or loses electrons. • anion – negatively charged ion formed when an atom gains electrons • cation – positively charged ion formed when an atom loses electrons Atomic Number • determined by the number of protons in the nucleus • found on the periodic table Determine the atomic number for each of the following elements. Li 3 N 7 Mg 12 Mass Number • equal to the sum of the neutrons and protons in the nucleus of an atom • not given on the periodic table Ways to indicate mass number: Hyphen notation Chlorine - 35 Nuclear Symbol 1. Write the hyphen notation and nuclear symbol for the element containing 4 protons and 5 neutrons. 2. Determine the number of neutrons in Argon-4 Complete the following table: Element (hyphen notation) Nuclear Symbol Number Number Number Atomic Mass of of of Number Number Protons Neutrons Electrons 22 Sodium -22 9 19 9 80 40 45 20 0