Question

Aluminum has a density of 2.699 g/cm^3. The atoms are packed in a face centered cubic...

Aluminum has a density of 2.699 g/cm^3. The atoms are packed in a face centered cubic crystal lattice. What is the radius of an aluminum atom?

a) 143.2pm b) 286.4pm c) 422.1pm d) 0.2254pm

Please show and explain work if possible. Thanks.

Science   Chemistry   
0 0
Add a commentTranscribed image text
Next >

Homework Answers

Answer #1

0 0
Know the answer?
Your Answer:

Post as a guest

Your Name:

What's your source?

Earn Coins

Coins can be redeemed for fabulous gifts.

Log In

Sign Up

Not the answer you're looking for?
Ask your own homework help question
Similar Questions
Copper crystallizes with a face-centered cubic lattice and has a density of 8.93 g/cm3. a.) Calculate...
Copper crystallizes with a face-centered cubic lattice and has a density of 8.93 g/cm3. a.) Calculate the mass of one unit cell of copper (in grams) b.) Calculate the volume of the copper unit cell (in cm3). c.) Calculate the edge length of the unit cell (in cm). d.) Calculate the radius of a copper atom (in pm).
1) For a metal that has the face-centered cubic (FCC) crystal structure, calculate the atomic radius...
1) For a metal that has the face-centered cubic (FCC) crystal structure, calculate the atomic radius if the metal has a density of (8.000x10^0) g/cm3 and an atomic weight of (5.80x10^1) g/mol.  Express your answer in nm. 2) Consider a copper-aluminum solid solution containing (7.82x10^1) at% Al. How many atoms per cubic centimeter (atoms/cm^3) of copper are there in this solution? Take the density of copper to be 8.94 g/cm3 and the density of aluminum to be 2.71 g/cm3.
A metal crystallizes in a face-centered cubic closest packed structure. The radius of the metal atom...
A metal crystallizes in a face-centered cubic closest packed structure. The radius of the metal atom is 2.14x10^-8 cm. calculate the density of solid metal if the atomic mass of the metal is known to be 87.62 g/mol. Identify the metal. Thank you!
Aluminum metal crystallizes in a face-centered cubic unit cell. If the atomic radius of an Al...
Aluminum metal crystallizes in a face-centered cubic unit cell. If the atomic radius of an Al is 1.43Angstroms, what is the density of aluminum (in g/cm^3)
1. Rubidium metal has a body-centered cubic structure. The density of the metal is 1.532 g/cm3....
1. Rubidium metal has a body-centered cubic structure. The density of the metal is 1.532 g/cm3. Calculate the radius of the rubidium atom. Assume that rubidium atoms are spheres. Then note that each corner sphere of the unit cell touches the body-centered sphere. 2. Copper metal has a face-centered cubic structure. The density of the metal is 8.93 g/cm3. Calculate the radius of the copper atom. Assume that copper atoms are spheres. Then note that the spheres on any face...
The very dense metal iridium has a face centered cubic structure and density of 22.56 g/cm3....
The very dense metal iridium has a face centered cubic structure and density of 22.56 g/cm3. use this information to calculate the radius of an iridium atom.
Rhodium crystallizes in a face-centered cubic unit cell. The radius of a rhodium atom is 135...
Rhodium crystallizes in a face-centered cubic unit cell. The radius of a rhodium atom is 135 pm. Determine the density of rhodium in g/cm3. please show all work and units!
A metal crystallizes in a face-centered cubic cell and had a density of 11.9 g/cm3. If...
A metal crystallizes in a face-centered cubic cell and had a density of 11.9 g/cm3. If the radius of the metal atom is 138 pm, what is the molar mass of the metal? What metal is it?
Metallic magnesium has a hexagonal close-packed structure and density of 1.74g/cm^3. Assume magnesium atoms to be...
Metallic magnesium has a hexagonal close-packed structure and density of 1.74g/cm^3. Assume magnesium atoms to be spheres of radius r. Because magnesium has a close-packed structure, 74.1% of the space is occupied by atoms. Calculate the volume of each atom; then find the atomic radius r. the volume of a sphere is equal to 4π^3/3.
A certain element crystallizes in a face-centered cubic lattice. The density of the crystal is 22.67...
A certain element crystallizes in a face-centered cubic lattice. The density of the crystal is 22.67 g·cm–3, and the edge of the unit cell is 383.3 pm. Calculate the atomic mass of the element. (a) 192 g·mol–1 (b) 40 g·mol–1 (c) 183 g·mol–1 (d) 70 g·mol–1 (e) None of the above
ADVERTISEMENT
Need Online Homework Help?

Get Answers For Free
Most questions answered within 1 hours.

Ask a Question
ADVERTISEMENT