ChemLab #14 - Diameter of a Zinc Atom Lab Group #
Zinc Data:

Density = 7.14 g/cm3

Atomic radius = 1.53 Å
(1 angstrom = 1 X 10 −8 cm)

Atomic volume = 9.2 cm3/mole

The Lab Problem: Using data from your mole lab (ChemLab #13), calculate the diameter of a zinc atom.

Hypothesis:

Your hypothesis should be the theoretical value for the diameter of a zinc atom from research.

The diameter of a zinc atom is ___________________ centimeters.

Research References: Given:
  • Mass of zinc (from ChemLab #13) =
     
  • Moles of zinc (from ChemLab #13) =
You may make the following assumptions for this lab:
  • All zinc atoms are the same size.
  • A zinc atom completely fills a cubic space.
  • There is no unoccupied space between zinc atoms.
  • The length of one edge of a cube is the cube root of the volume.
  • The number of atoms along one edge of a cube is the cube root of the total number of atoms in the cube.
  • The diameter of a zinc atom will be the length of one edge of the cube divided by the number of atoms along that edge.
Lab Calculations: (This is where your grade is made. MAKE CALCULATIONS NEAT AND CLEAR!)
 
Show all calculations on the back of this lab report.

 
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What is the most likely source of error?