Beanium_Lab

Beanium Isotope Dr.Mazzur 10/6/11-10/10/1 I. INTRODUCTION: 1) Purpose: In this lab I carried out experiments and performed the necessary calculations to determine the atomic mass of the fictitious element Beanium. These experiments and calculations are equivalent to the way scientists actually determine the atomic mass of elements. The six different isotopes of Beanium are black eyed, black, kernels, white, brown, and spotted brown. As in real elements, the mixture of isotopes are collections of atoms of the element each having different masses because they have different numbers of neutron. My job was to obtain a sample of Beanium with all six of its representative isotopes, and determine the relative abundance of each isotope. From this data I had to calculate the average mass of each isotope and the weighted average atomic mass of the element Beanium. Unlike real isotopes, the individual isotopic particles of Beanium differ slightly in mass, so I had to determine the average mass of each type of isotopic particle. Then calculate the "weighted average atomic mass" of Beanium. 2) Lab Report: I had to complete the lab and begin to write my own lab report in class – one per student – NO GROUPS! My s lab report will have, labeled with roman numerals: I Introduction Section, II procedure Section, III Data Table/ Calculations Section, and V a conclusion section. 3) What is an isotope: form of element with same atomic number: each of two or more forms of a chemical element with the same atomic number but different numbers of neutrons. II. PROCEDURE: 1) Obtain a sample of the Beanium “atoms” in a cup from the bag 2) Separate your beans by color. 3) Count the number of each color of bean. Record on data table. 4) Weigh all the black beans. Record mass on data table. Do the same with all 5) Mass the total in each group 6) Place all the beans back in the container at the front of the room. III. DATA TABLE: 1) Table 1:Mass of Sample: measure mass minus mass of tray ( 2.47) TYPE | NUMBER OF BEANS | MASS OF SAMPLE | Black eyed | 52 | 14.42-2.47= 11.95g | Black | 36 | 8.42-2.47=5.97g | Kernels | 21 | 5.82-2.47=2.81g | White | 46 | 18.31-2.47=15.89g | Brown | 16 | 10.15-2.47=7.68g | Spotted brown | 17 | 9.04-2.47=6.57g | SKETCH OF BEANS Total beans in the can = 188 Total Mass of beans in can = 50.77g 2) Table 2: Average Mass of one bean: Divide the total mass of the black beans by the total number of black beans. Record under “average mass” in data table. Do the same for the brown and white beans. Include calculations in the calculations section. Write results in data table. Type | Average Mass (+ calculations) | Black eyed | 50.77/11.95= 4.2485 g/cm3 | Black | 50.77/5.97= 8.5041 g/cm3 | kernels | 50.77/2.87=17.6898 g/cm3 | White | 50.77/15.89=2.6876 g/cm3 | Brown | 50.77/7.68=6.6106 g/cm3 | Spotted brown | 50.77/6.57=7.7275 g/cm3 | 3) Table 3: Percent Abundance: Divide the number of each isotope (color bean) by the total number of particles (beans). Multiply this by 100 to get percent. Results in the data table under percent abundance. Type | Percent abundance (+ calculations) | Black eyed | 52/188 x 100=27.65% | Black | 36/188x100=19.14% | kernels | 21/188x100=11.17% | White | 46/188x100=24.46% | Brown | 16/188x100=8.51% | Spotted brown | 17/188x100=9.04% | 4) Table 4: Average Atomic Mass: Use the percent abundances and the average masses in the atomic mass equation. Atomic mass = % of isotope #1 x (mass isotope #1) + % of isotope #2 x (mass Isotope #2) + % of isotope #3 x (mass Isotope #3) = Type | Average Atomic Mass (+ calculations) | Black eyed | .2765x11.95= 3.30 + | Black | .1914x5.97=1.14 + | kernels | .1117x2.81=0.31 + | White | .2446x15.89=3.88 + | Brown | .851x7.68=6.53 + | Spotted brown | .904x6.57=5.93 + | AVERAGE ATOMIC MASS = | 21.09 | IV. CONCLUSION: What is an isotope' It’s a form of element with same atomic number: each of two or more forms of a chemical element with the same atomic number but different numbers of neutrons. The purpose of this lab was to determine the experimental atomic mass of the element beanimium using the relative abundance and relative masses of the randomly selected isotopes of the element. In the lab the colored beans represented the different kinds of isotope in an element. But the importance of those beans (isotopes) is that they help keep that element stable, also they have a role in calculating the atomic the number of protons plus neutron. For example just by using the isotope of beanium you can calculate that it has an atomic weight of 21.09. But just by changing the number of isotopes in the element you change it mass and neutron but not it protons. . As in real elements, the mixture of isotopes are collections of atoms of the element each having different masses because they have different numbers of neutrons. These experiments and calculations are equivalent to the way scientists actually determine the atomic mass of elements.