Asked by Nick
<b>Titanium metal has a body-centered cubic unit cell. The density of Titanium is 4.50 g/cm^3. Calculate the edge length of the unit cell and a value for the atomic radius of titanium.</b>
Ok, I know how to find the density using the atomic radius, but I'm having trouble working backwards using the density to find the atomic radius). I'm not really sure how to find the volume. And I know that the pythagorean theorem will help me find the radius but I'm missing some steps in between.
Ok, I know how to find the density using the atomic radius, but I'm having trouble working backwards using the density to find the atomic radius). I'm not really sure how to find the volume. And I know that the pythagorean theorem will help me find the radius but I'm missing some steps in between.
Answers
Answered by
DrBob222
I would be willing to bet you are stuck on just one step. Here it is,
1 mol Ti atoms = 47.88 g (check that on your periodic table)and that mass contains 6.022 x 10^23 atoms. Use that to calculate the mass of 1 atom of Ti, from that you have m =volume x density which allows you to calculate the volume. Take the cube root of V to obtain a, the length of the edge of the cube. Can you take it from here. The radius, if you need help there, is (1/4)*(sqrt 3)*a. I hope this helps.
1 mol Ti atoms = 47.88 g (check that on your periodic table)and that mass contains 6.022 x 10^23 atoms. Use that to calculate the mass of 1 atom of Ti, from that you have m =volume x density which allows you to calculate the volume. Take the cube root of V to obtain a, the length of the edge of the cube. Can you take it from here. The radius, if you need help there, is (1/4)*(sqrt 3)*a. I hope this helps.
Answered by
Nick
Thank you so much!
There are no AI answers yet. The ability to request AI answers is coming soon!
Submit Your Answer
We prioritize human answers over AI answers.
If you are human, and you can answer this question, please submit your answer.