The radius of a barium atom is 217 pm. How many barium atoms would have to be laid side by side to span a distance of 4.33 mm?

Well, we could start by converting the radius of a barium atom from picometers to millimeters. So, 217 pm is equal to 0.217 nm or 0.000217 mm.

Now, to find how many barium atoms can span a distance of 4.33 mm, we divide 4.33 mm by the diameter of a barium atom (which is twice the radius).

So, the diameter of a barium atom is 0.000434 mm (0.000217 mm multiplied by 2).

Now, we can simply divide 4.33 mm by 0.000434 mm to get the number of barium atoms.

But why stop at barium atoms when we can have a little fun?

If my calculations are correct, you would need approximately 9,982,567 barium atoms laid side by side to span a distance of 4.33 mm. That's quite an atom party!

To find out how many barium atoms would have to be laid side by side to span a distance of 4.33 mm, we need to convert the radius of a barium atom from picometers (pm) to millimeters (mm).

1 pm = 1 × 10^-3 nm
1 nm = 1 × 10^-6 mm

So, we can convert the radius of a barium atom from pm to mm as follows:

217 pm = 217 × (1 × 10^-3) nm = 0.217 nm
0.217 nm = 0.217 × (1 × 10^-6) mm = 2.17 × 10^-7 mm

Now, to calculate how many atoms would span a distance of 4.33 mm, we divide the given distance by the converted atomic radius:

Number of atoms = (4.33 mm) / (2.17 × 10^-7 mm)
Number of atoms = 1.99 × 10^7

Therefore, approximately 19,900,000 (or 1.99 × 10^7) barium atoms would have to be laid side by side to span a distance of 4.33 mm.

To find out how many barium atoms would have to be laid side by side to span a distance of 4.33 mm, we need to convert the given radius from picometers (pm) to millimeters (mm).

1 pm = 1 × 10^-9 mm

So, the radius of the barium atom in millimeters is:

217 pm * (1 × 10^-9 mm/1 pm) = 2.17 × 10^-7 mm

Now, we can calculate the number of barium atoms required by dividing the total distance by the radius:

Number of barium atoms = (4.33 mm) / (2.17 × 10^-7 mm)

Number of barium atoms = (4.33 mm) * (1 / (2.17 × 10^-7 mm))

Number of barium atoms = 1.99 × 10^7 barium atoms

Therefore, approximately 19,900,000 (or 1.99 × 10^7) barium atoms would have to be laid side by side to span a distance of 4.33 mm.

All right, you've got the radius of an atom. Whenever you get a problem asking for the volume, density, etc. you assume the atom is a sphere. The diameter of a barium atom would then be:

217pm * 2 = 434pm

Either convert 4.33mm to pm or 434pm to mm. I'll convert 4.33mm to pm:

4.33mm * 1.0*10^9pm/1mm = 4.33 * 10^9pm

So how many atoms with a diameter of 434pm fit in 4.33 * 10^9pm?

4.33 * 10^9pm * 1 Ba atom/434pm = 9976959 Ba atoms