Determination of the atomic radius of an Al atom

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Discussion Overview

The discussion revolves around determining the atomic radius of an aluminum (Al) atom using measurements from a piece of aluminum foil. Participants explore various methods and assumptions related to the atomic structure and volume calculations.

Discussion Character

  • Homework-related
  • Exploratory
  • Mathematical reasoning

Main Points Raised

  • One participant seeks assistance in calculating the atomic radius of Al using the mass and dimensions of aluminum foil, mentioning the molar mass of aluminum.
  • Another participant suggests treating the atom as a cube for simplification and proposes "stacking" cubes to find the radius, indicating they have calculated the number of moles and atoms in the sample.
  • A third participant proposes that from the number of Al atoms and the total volume occupied by these atoms, it may be possible to find the volume of each atom.
  • A later reply emphasizes the importance of visualizing the atomic structure, suggesting that if the atoms are imagined as cubic, the radius could be derived as half the length of a side of the cube.

Areas of Agreement / Disagreement

Participants do not appear to reach a consensus on the best method to calculate the atomic radius, with multiple approaches and assumptions being discussed.

Contextual Notes

Participants rely on various assumptions, such as the atomic structure of aluminum and the treatment of atoms as cubes or spheres, which may affect the calculations. There is also an implicit dependence on the purity of the aluminum sample.

dajugganaut
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hi everyone,

im trying to find the atomic radius of an Al atom using a few measurements i have. i had a piece of aluminum foil its measurements were [ 10cm*9.9cm*0.0014cm ]. The mass of the aluminum foil was 0.40 grams. Is there any possible way i can find the radius of an Al atom? I know i might have to use the molar mass 26.98 g /mol somwhere, but i don't know where. If you could help me, that would be greatly appreciated!

thanks =)
 
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i was told that the atom is spherical, but for simpler purposes to pretend it as a cube. then i would "stack" the cubes to find the radius of it. so i found out how many mols of Al there were in 0.4 g. and then i found the # of molecules in 0.4g of Al [assuming that it is pure Al] i can't be exactly sure what to do next
 
From the number of Al atoms, and the total volume (from the dimensions) occupied by this many atoms, can't you find the volume of each atom ?
 
It would be helpful if he could imagine the structure of Al in terms of cubic atoms...After all,atoms are not spherical...This part could help you find the radius...It's half of the length of a side of a cube...

Daniel.
 

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