Many metals pack in cubic unit cells. The density of a metal and length of the u
ID: 809592 • Letter: M
Question
Many metals pack in cubic unit cells. The density of a metal and length of the unit cell can be used to determine the type for packing.
(a) How many platinum atoms are in exactly 1 cm3?
_________atoms
(b) How many unit cells are in exactly 1 cm3?
________ unit cells
(c) How many platinum atoms are there per unit cell?
__________atom(s)
(d) The atoms/unit cell suggests that platinum packs as a (---Select--- simple, body-centered, or face-centered) unit cell.
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Knowledge of the type of packing and side length a of the unit cell will allow calculation of the atomic radius, using one of the equations below. You may need to draw the unit cell to determine which formula to use to calculate the atomic radius.
(e) What is the atomic radius of platinum?
___________? (angstroms)
Explanation / Answer
a) Relative Atomic Mass(RAM) of platinum= 195
195g= 1 mole of platinum
21.45g= 21.45/195
= 0.11 moles of platinum
1 mole of platinum= 6.02x10^23 atoms
0.11 moles of platinum= 0.11x6.02x10^23
= 6.62x10^22 atoms(no of platinum atoms in 1cm^3)
b) Are the side lengths 3.93
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