Chemistry: Isotopes Chemistry: Isotopes
In this lab, you will explore isotopes of different elements - pennium, orangeM&Mium, blackM&Mium, and flaskium. By determining the number of isotopes, their masses, and percent abundances, you will calculate the average atomic mass for each element. The process involves measuring masses, analyzing data, and making calculations based on the collected information. Through this experiment, you will gain insight into the concept of isotopes and how they contribute to the overall atomic mass of elements.
Download Presentation
Please find below an Image/Link to download the presentation.
The content on the website is provided AS IS for your information and personal use only. It may not be sold, licensed, or shared on other websites without obtaining consent from the author.If you encounter any issues during the download, it is possible that the publisher has removed the file from their server.
You are allowed to download the files provided on this website for personal or commercial use, subject to the condition that they are used lawfully. All files are the property of their respective owners.
The content on the website is provided AS IS for your information and personal use only. It may not be sold, licensed, or shared on other websites without obtaining consent from the author.
E N D
Presentation Transcript
Document Chemistry: Isotopes Chemistry: Isotopes Average Atomic Mass Lab Average Atomic Mass Lab In this lab, you will investigate isotopes. As you recall, isotopes of an element are atoms that have the same number of protons, but have different numbers of neutrons. You will find the number of isotopes of several elements : pennium, orangeM&Mium, blackM&Mium, and flaskium. You will also find the percent abundance of each of the isotopes. Finally, you will calculate the average atomic mass of the atoms of each type of element. Work steadily. (virtual lab)
Pennium Find one of the containers containing atoms of pennium. Container letter: _________ Using a balance, find the mass of each of the pennies in the container. Record the year and the mass of each penny in the table below. You might not use all of the spaces. Use the data in the table to calculate percent abundance and average atomic mass. Year Mass (g) Year Mass (g) Year Mass (g) 1999 3.21 g 1982 3.19 g 2012 2.51 g 1979 3.21 g 1987 3.20 g 2002 2.50 g 1986 3.20 g 1997 3.19 g 1966 3.21 g 2018 2.49 g 2015 2.48 g 1980 3.20 g 2004 2.50 g 2020 2.50 g 1982 3.19 g 1982 2.51 g 1980 3.22 g 2002 2.50 g 1981 3.21 g 1967 3.19 g 1971 3.24 g 2019 2.51 g 1984 3.23 g 2000 3.22 g 1983 2.47 g 1992 3.19 g 1983 2.50 g 1999 2.49 g 2003 2.52 g 2011 3.21 g Flip a coin 30 x and count how many were heads and how many were tails. Heads = 2.5 g penny; Tails = 3.2 g penny.
Summary of Data Calculate the Average Atomic Mass for Each Isotope of Pennium by adding up all of the masses and dividing by the number of atoms of that isotope (show some work or give a brief explanation) ISOTOPE 1 ISOTOPE 2 Number of Atoms Isotope Description Percent Abundance (show work) 1 Approx. Mass = 2 Approx. Mass = Calculate the Overall Average Atomic Mass of Pennium by using the Average Atomic Mass of each isotope (calculated in the previous step, above) and the % abundance of each isotope (show work).
OrangeM&Mium Find one of the containers filled with atoms of orangeM&Mium. Container letter: __________ Fill in the table below. Isotope Description Number of Atoms 88 37 Percent Abundance (show work) 1 Mass = 3 Summary of Data 2 Mass = 2 Calculation of Average Atomic Mass for OrangeM&Mium (show work) BlackM&Mium Find one of the containers filled with atoms of blackM&Mium. Container letter: __________ Fill in the table below. Isotope Description Number of Atoms 16 45 Percent Abundance (show work) 1 Mass = 2 Summary of Data 2 Mass = 1 Calculation of Average Atomic Mass for BlackM&Mium (show work)
Flaskium Find the setup that has several atoms of flaskium. Fill in the table below Isotope Description Number of Atoms Percent Abundance (show work) 1 Mass = 5 2 Mass = 4 12 3 Mass = 2 Calculation of Average Atomic Mass for Flaskium (show work) 4 7 (Red number is how many of each item you have)
ANALYSIS QUESTIONS ANALYSIS QUESTIONS Refer back to your pennium data and answer the following questions. 1. What do the pennies represent in this investigation? 2. What do the different masses of the pennies represent? 3. What information do you need to calculate the average atomic mass of an element? 4. Was the mass of 20 pennies equal to 20 times the mass of one penny? Explain. 5. In what year did the mass of pennium change? How could you tell? 6. How can you explain that there are different isotopes of pennium?
Refer back to your M&Mium data and answer the following question. 7. Although the percent abundance of large and small atoms of each type of M&Mium were identical, the average atomic mass of orangeM&Mium was different from that of blackM&Mium. Why? Refer back to your flaskium data and answer the following question. 8. Does the formula for finding average atomic mass work equally well for 3 isotopes rather than just 2?
Applications: Answer the following questions. 9. Why are the atomic masses for most elements NOT whole numbers? 10. How are the 3 isotopes of hydrogen (H-1, H-2, and H-3) ALIKE DIFFERENT 11. Copper has 2 isotopes, copper-63 and copper-65. The percent abundance of copper-63 is 69.1% and that of copper-65 is 30.9%. Find the average atomic mass of copper. 12. Lithium has 2 isotopes, Li-6 and Li-7. The percent abundance of Li-6 is 7.42% and that of Li-7 is 92.58%. Find the average atomic mass of Li.
13. Silver has 2 isotopes, Ag-107 and Ag-109. The percent abundance of Ag-107 is 51.35% and that of Ag-109 is 48.65%. Find the average atomic mass of silver. 14. The element Christophersonium (Ch) has three isotopes. Isotope A has a mass of 34.22 amu and a % abundance of 25.1%. Isotope B has a mass of 36.4 amu and a % abundance of 58.6 %. Isotope C has a mass of 37.5 amu and a % abundance of 16.3 %. Find the atomic mass of Ch. 9. 15. The element Normalium (Nm) has an average atomic mass of 85.468 amu. Normalium has two common isotopes, 85Nm and 87Nm. If the mass of 85Nm is 85.00 amu and the abundance is 72.2%, what is the mass of 87Nm?
