Cristaline structure: simple solid state physics problem

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SUMMARY

The discussion focuses on calculating the distance between atoms in Nickel (Ni) using its atomic mass of 58.7 amu and density of 8.86 g/cm³. The user initially calculates the number of atoms per cm³ as approximately 5.3356 x 10²⁴ atoms/cm³ but struggles with the next steps due to uncertainty about the unit cell type. The solution requires identifying the correct unit cell structure for Nickel to determine the distance between adjacent atoms accurately.

PREREQUISITES
  • Understanding of atomic mass and density calculations
  • Familiarity with unit cell concepts in solid state physics
  • Knowledge of crystal structures, specifically for Nickel
  • Proficiency in using the formula for calculating the number of atoms per volume
NEXT STEPS
  • Research the crystal structure of Nickel, focusing on its face-centered cubic (FCC) arrangement
  • Learn how to calculate the length of the side of a unit cell from atomic density
  • Study the relationship between atomic radius and interatomic distance in crystalline solids
  • Explore solid state physics textbooks for detailed examples of unit cell calculations
USEFUL FOR

Students studying solid state physics, materials scientists, and anyone interested in understanding atomic arrangements in metals like Nickel.

Jalo
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Homework Statement



The atomic mass of Niquel is 58.7 amu (atomic mass unit), and it's density (at 90ºC) is 8.86 g/cm³.

(a) Find the distance from one atom to the closest one from him.

Homework Equations



1 amu = 1.66053*19⁻²⁷

The Attempt at a Solution



I started by finding the number of atoms per cm³, N:

[itex]N = \frac{8.86*10^{24}}{1.66053} = 5.3356*10^{24} atoms/cm^{3}[/itex]

This is where I lose myself. Am I supposed to solve this without knowing the type of unit cell? If I knew it, since I know the number of atoms per cell, I would be able to get the length of the side of the unit cell, and from there I could work out the distance between two atoms next to each other.

Is there a way to solve this without knowing the unit cell before hand? Or am I supposed to solve it by searching the correct unit cell and following the line of thought I wrote?
Thanks ahead.
D.
 
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Jalo said:

Homework Statement



The atomic mass of Niquel is 58.7 amu (atomic mass unit), and it's density (at 90ºC) is 8.86 g/cm³.

(a) Find the distance from one atom to the closest one from him.

Homework Equations



1 amu = 1.66053*19⁻²⁷

The Attempt at a Solution



I started by finding the number of atoms per cm³, N:

[itex]N = \frac{8.86*10^{24}}{1.66053} = 5.3356*10^{24} atoms/cm^{3}[/itex]

This is where I lose myself. Am I supposed to solve this without knowing the type of unit cell? If I knew it, since I know the number of atoms per cell, I would be able to get the length of the side of the unit cell, and from there I could work out the distance between two atoms next to each other.

Is there a way to solve this without knowing the unit cell before hand? Or am I supposed to solve it by searching the correct unit cell and following the line of thought I wrote?
Thanks ahead.
D.

You can browse for "Crystal structure of Nickel" or see the Periodic Table http://en.wikipedia.org/wiki/Periodic_table_(crystal_structure)

When calculating the number of atoms in 1 cm3, you have to consider the atomic mass of Nickel. Your result is wrong.

ehild
 

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