13. Liquids, Solids & Intermolecular Forces
Body Centered Cubic Unit Cell
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Practice this topic
- Multiple Choice
Tungsten possesses a body-centered cubic structure. If its density is 19.28 g/cm3, what is its radius in pm?
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Vanadium has a body-centered cubic structure. If the atomic radius of vanadium is 134 pm, calculate the density of solid vanadium.
1802views3rank - Multiple Choice
The edge of a body-centered cubic unit cell of an element Z was found to be 2.88 x 10-8 cm. The density of the element is 7.2 g/cm3. What is the approximate molar mass of Z?
1391views4rank - Textbook Question
Identify each of the following kinds of packing: (d)
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Determine the number of atoms per unit cell for each metal.
(b) Tungsten
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Sodium metal (atomic weight 22.99 g/mol) adopts a body-centered cubic structure with a density of 0.97 g/cm3. (a) Use this information and Avogadro’s number (NA = 6.022 × 1023/mol) to estimate the atomic radius of sodium. (b) If sodium didn't react so vigorously, it could float on water. Use the answer from part (a) to estimate the density of Na if its structure were that of a cubic close-packed metal. Would it still float on water?
1700views1comments - Textbook Question
Molybdenum crystallizes with the body-centered unit cell. The radius of a molybdenum atom is 136 pm. Calculate the edge length of the unit cell and the density of molybdenum
2036views1comments - Multiple ChoiceA metal crystallizes in a body-centered cubic structure with a unit cell edge length of 4.31 Å. What is the radius of the atoms in Å?424views