1. Define the following terms: face-centered cubic unit cell, percent-occupied volume, and coordination number 2. If...

1. Define the following terms: face-centered cubic unit cell, percent-occupied volume, and coordination number

2. If the side length, , of a unit cell that crystallizes in a face-centered cubic unit cell is 4.57 Å, what is the radius of an atom

? 3. If an element crystallizes in a body-centered cubic unit cell, write the formula for the volume of the unit cell in terms of the side length,  and write the formula for the volume of the atom in terms of the radius of the atom, r?

4. Which one of the three types of cubic unit cells has the most occupied volume?

Expert Solution

queen_honey_blossom answered 2 years ago

Face Centered Cubic unit cell problem

An element has a face centered cubic unit cell with a length of 352.4 pm along an edge.The density of the element is 8.9 gcm-3.How many atoms are present in 100g of an element?

To calculate the number of atoms in a face centered cubic cell?

The element lead (Pb) crystallizes with a Face Centered Cubic unit cell. The density of lead...

The element lead (Pb) crystallizes with a Face Centered Cubic unit cell. The density of lead is 11.3 g/cm3. Use this information to calculate the theoretical metallic radius of a lead atom in picometers. 1 pm = 1×10−12 meters [Note: The theoretical value for the metallic radius may be different from the experimentally determined value. Simply Googling the value of atomic radius may not yield the correct result]

Gold has a face-centered cubic arrangement with a unit cell edge length of 4.08 Å ....

Gold has a face-centered cubic arrangement with a unit cell edge length of 4.08 Å . How many moles of gold fit in a gold nanoparticle sheet with a length of 57.3 nm , a width of 20.1 nm , and a thickness of 10.2 nm ?

Iridium crystallizes in a face-centered cubic unit cell that has an edge length of 3.811 Å....

Iridium crystallizes in a face-centered cubic unit cell that has an edge length of 3.811 Å. (a) Calculate the atomic radius of an iridium atom. (b) Calculate the density of iridium metal.

Palladium crystallizes in a face-centered cubic unit cell. Its density is 12.02 g/cm^3 .Calculate the atomic...

Palladium crystallizes in a face-centered cubic unit cell. Its density is 12.02 g/cm^3 .Calculate the atomic radius of Pd. A) calculate the average mass of 1pd atom B) calculate the number of pd atoms in FCC C) use the density to calculate the volume D) Determine the edge lenth using volume E) determine the atomic radius using the pythagorean theorem .

An element crystallizes in a body-centered cubic lattice. The edge of the unit cell is 3.28...

An element crystallizes in a body-centered cubic lattice. The edge of the unit cell is 3.28 Å in length, and the density of the crystal is 6.50 g/cm3 . a.) Calculate the atomic weight of the element.

(a) Generally, you have four types of unit cell arrangements like 1. Simple cubic 2. Face...

(a) Generally, you have four types of unit cell arrangements like 1. Simple cubic 2. Face centered 3. Body-centered 4. Base centered. Can you calculate the number of atoms in each cubic cell? For example, a simple cubic has 1 atom, base-centered has 2 atoms, body-centered has 2 atoms and face-centered has 4 atoms. Explain how these cubic units 1 – 4 have a specified number of atoms. (b) You have two types of glass solids, both have a cooling...

A) A metal (FW 295.6 g/mol) crystallizes into a body-centered cubic unit cell and has a...

A) A metal (FW 295.6 g/mol) crystallizes into a body-centered cubic unit cell and has a radius of 2.89 Angstrom. What is the density of this metal in g/cm3? B) A metal (FW 339.6 g/mol) crystallizes into a face-centered cubic unit cell and has a radius of 2.84 Angstrom. What is the density of this metal in g/cm3?

Calculating the packing fraction (The percent space occupied by atom) for a hexagonal unit cell requires...

Calculating the packing fraction (The percent space occupied by atom) for a hexagonal unit cell requires a bit more trigonometry than the same calculation for a cubic cell. However, based on your observations, which of the cubic cells would you expect to have the same packing fraction as the hexagonal cell? Explain your reasoning?

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