Data Analysis and Concept Development

Implications and Applications

  1. What did you find out about the number of beans in one relative mass? How do your calculated values compare to your measured values?
  2. How many times larger is the lima bean relative mass than the lentil bean relative mass? How does this relate to the number of beans in the relative mass?
  3. In a very logical statement, explain why there are always the same number of beans in one relative mass. Think very hard about this one.
  4. Compare the volume of relative mass piles. Are they the same? Why or why not?
    1. What is the average mass of the lightest bean?
    2. What is the relative mass of the lightest bean?
  6. Among the elements, hydrogen has the least massive atoms-an atom of hydrogen has an average mass of 1.66 x 10-24 g. This is very small, but remember it is only one atom! What is the relative mass of hydrogen if it is the least massive element?

    Part II

    Examine the beakers of elements and compounds on display. Each beaker contains one mole of a particular substance. Record information on the chart below.

    1. Which substance occupies the largest volume?
    2. Which substance occupies the smallest volume?
    1. One mole of which substance has the largest mass?
    2. Which substance has the most massive individual particles?
    3. Why must the answers to Questions 14a and 14b be the same?

  9. Why do equal amounts (in moles) of different elements and compounds have different masses even though they have the same number of particles?
  10. Why do equal amounts (in moles) of elements or compounds occupy different volumes?
  11. Describe the fastest way to measure one relative mass of beans.
  12. Describe the fastest way to measure out one mole of beans.

    Part III

    Below is a chart reporting the average masses of individual atoms. Calculate the relative mass of each element and record it in the chart. Then look up the molar mass (atomic mass) of each element on a Periodic Table and record it in the table.

    * Although this calculation works with a relative mass of hydrogen of 1.00 as its basis, atomic masses are actually calculated as relative to a particular type of carbon atom viewed as exactly 12.00.

  13. Comment on how the atomic masses found on the Periodic Table compare to the relative masses you calculated.14. What are atomic masses, and how are they determined?
  14. What did you find out about the number of atoms of each element in one relative mass?
  15. Whose name is given to the number of atoms in the relative mass?
  16. One atomic mass unit (u) is the approximate mass of a proton or a neutron. This mass is equal to 1.66 x 10-24 g. How many atomic mass units are in one gram?
  17. If an atom has a mass of 197 u, find the mass (in g) of a mole of these atoms.

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