00:01
Don't it.
00:06
We are told that we have a body centered cubic unit cell and our specific gravity, which is going to be equivalent in this case to our density, and our specific gravity is 10 .200 at 25 degrees c.
00:42
And we're told that it crystallizes into a body centered cubic with a cell edge length of 3 .147 angstroms.
01:07
We need to find the atomic weight, as far as i like to call it, atomic mass, identity of the metal, identity of the metal, and the radius in angstroms.
01:46
And we're told whoever did this that they already got the atomic weight of 97 .5, or 0 .72 grams per mole.
01:57
But i'm going to go ahead and show how to do that.
02:00
And they want to do the radius.
02:02
So i'm just going to very quickly go through how to get this.
02:08
So this is the atomic weight.
02:11
Maybe i won't.
02:14
And we're told it's molybdenum.
02:26
That's all given.
02:29
So they said not sure how to get the radius.
02:42
So that's all we're going to focus on is how to get the radius.
02:46
That's pretty simple.
02:47
To get the radius, radius, we are going to use 4 d squared equals 4 r squared, and that'll be about it.
03:08
And d is our edge length and our edge length in centimeters.
03:27
So what i'm going to do here is i'm going to calculate our edge length in centimeters from our 7 .147 angstroms.
03:41
And i'm going to, well, i'm going to go ahead and convert this.
03:47
Angstroms, there are one times 10 to the 10th angstroms and 100 centimeters.
04:01
This will equal 3 .147 times 10 to the 8th centimeters.
04:11
I'm going to verify that...