# Isotopes of Pennium Lab Name ___________________________ Date _______________ Period ______

```Isotopes of Pennium Lab
Name ___________________________
Date _______________ Period ______
Introduction:
In this investigation, you will determine the relative abundance of the isotopes of pennium and
the masses of each isotope. You will then use this information to determine the atomic mass of
pennium. Recall that the atomic mass of an element is the weighted average of the masses of the
isotopes of the element. The average is based on both the mass and the relative abundance of each
isotope as it occurs in nature.
Pre-Lab Questions
1. What do the 20 pennies in this investigation represent? _______________________________
2. What do the different masses of the pennies represent? ________________________________
3. What information is needed to calculate average atomic mass?
____________________________________________________________________________
Materials
Balance
20 pennies
Procedure
1. Line the 20 pennies up in chronological order.
2. Mass each penny individually. Record its year and mass in the data table.
3. Draw a line(s) through the table indicating where the mass of the penny changed 0.1 g or
greater from the previous penny.
Data Table
Penny
Mass of 20 pennies = ________ g
Year
Mass (g)
1
2
3
4
5
6
7
8
9
10
11
12
13
14
15
16
17
18
19
20
Calculations:
1. Determine the number of isotopes of Pe that are present. _____________________
2. Calculate the percent abundance of each isotope of your sample.
3. Calculate the average atomic mass of each isotope.
4. Using percent abundance and the average atomic mass of each isotope, calculate the atomic
mass of Pe.
Analysis and Conclusions:
1. Was the mass of 20 pennies equal to the mass of 20 times one penny? Explain.
_________________________________________________________________________
_______________________________________________________________________
2. In what year(s) did the mass of Pe change? How could you tell?
_________________________________________________________________________
_________________________________________________________________________
3. How can you explain the fact that there are different “isotopes” of pennium?
_________________________________________________________________________
_________________________________________________________________________
4. Why are the atomic masses for most elements not whole numbers?
_________________________________________________________________________
_________________________________________________________________________
5. How are the three isotopes of hydrogen (hydrogen-1, hydrogen-2, hydrogen-3) alike? How
are they different?
_________________________________________________________________________
_________________________________________________________________________
6. Copper has two isotopes, copper-63 and copper-65. The relative abundance of copper-63 is
69.1% and copper-65, 30.9%. Calculate the average atomic mass of copper.
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