Problem: The diameter of a rubidium atom is 4.95 Å. We will consider two different ways of placing the atoms on a surface. In arrangement (a), all the atoms are lined up with one another. Arrangement (b) is called a close-packed  arrangement because the atoms sit in the "depressions" formed by the previous row of atoms: If extended to three dimensions, which arrangement would lead to a greater density for Rb metal?

FREE Expert Solution

The ratio of atoms in arrangement B to arrangement A is:

  • Atom A: 4.713 x 1014 atoms
  • Atom B: 4.081 x 1014 atoms
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Problem Details

The diameter of a rubidium atom is 4.95 Å. We will consider two different ways of placing the atoms on a surface. In arrangement (a), all the atoms are lined up with one another. Arrangement (b) is called a close-packed  arrangement because the atoms sit in the "depressions" formed by the previous row of atoms: (A) 16 atoms are arranged in a square grid of four rows of four atoms. (B) 16 atoms are arranged in four rows of four, but each row is offset so that the atoms below fit “between” the atoms above rather than directly below them.

If extended to three dimensions, which arrangement would lead to a greater density for Rb metal?

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