# Half Life Accuracy?

1. Jul 12, 2012

### mram10

I was debating a friend and we started running numbers for the statistical accuracy of half-lives. I am a numbers guy(Accountant/Statistical Analysis), not a chemist. He is a scientist and his wife is a chemical engineer. Here is my question:

If we have been studying half lives of radioactive particles for less than 200 years, how do we know exactly what they are? We came up with 1.1764e-7 for the percentage of time we have studied the half life of Potassium. That is assuming 200 years of study/1.7billion years for the half-life. In the statistical world, that is not enough to even discuss, however I understand that we have to use what we have. These where just quick numbers, so please correct errors. What are we missing? Why are they so sure these half-lifes are correct? Thanks.

ps- Yes, I googled "half life accuracy, radiometric dating" and used the search function :)

2. Jul 12, 2012

### Staff: Mentor

You don't measure half life by waiting, but by measuring activity of the sample. Knowing how many atoms fissioned in a given period of time you can calculate half life - and the accuracy of the result of calculation depends on the accuracy of the activity measurement.

3. Jul 12, 2012

### mram10

If I have a small bowl of potassium and a large bowl, wouldn't they both lose half of their respective potassium in the same amount of time to decay? I was under the impression it is a set rate, thus we would need to be able to watch a specific amount of this decay occur to come up with a rate. Of course, assuming there was a known amount of argon in the first place. Keep the explanation coming please. I want to have a firm grasp on this.

4. Jul 12, 2012

### Staff: Mentor

Sounds like you don't know what it means to measure activity.

Decay is described by the formula:

$$N(t)=N_0e^{-\frac t \tau}$$

where N0 is the initial amount of a substance (at t=0) and τ is the half life. Imagine you were observing a sample of known mass (thus known N0) for time t. During this time N0-N(t) atoms decayed. We can count these decays using some kind of radiation measuring device (like Geiger counter) - that means we measured sample activity. We know initial number of atoms (N0), we know number of decays (N0-N(t)), we know how long we observed the sample (t). Plug everything into the equation - there is only one unknown, half time, which can be easily solved for. We can measure all three parameters (mass, time, activity) with a very high accuracy and precision, so the error of the half life determination is usually pretty small.

Sure, the more active the sample, the better (unless it fissions too fast, which is a different problem). But you don't have to wait for billions of years.

5. Jul 12, 2012

### tiny-tim

hi mram10!

if the half-life is H, then after time 2H only 1/4 is left, after 4H, 1/16 is left and so on

we can also go the other way … after time H/2, 1/√2 is left, after time H/4, 1/√√2 is left, and so on

so we don't need to wait for the half-life, we can wait for any time, and then do a calculation

the number of decays of a piece of potassium can be counted accurately enough to find the half-life to 4 or 5 significant figures

6. Jul 13, 2012

### mram10

Makes more sense. After a little more reading, it is clear that decay is an average based on the law of large numbers, not a constant, meaning each atom decays at a different rate. As for the T in the equation, it seems like 10 years of observing and testing a known quantity would still render a large margin of error when we are using millions and billions of years.

I will continue to study this, but please keep the basic analogies coming to aid in my understanding. You guys have been very helpful thus far.

Last edited: Jul 13, 2012
7. Jul 13, 2012

### epenguin

We would not agree that "each atom decays at a different rate". Each atom decays at a different time, maybe. You cannot have a rate of something that happens instantaneously only once. You can have a time in which it has half a chance of happening.

Last edited: Jul 13, 2012
8. Jul 13, 2012

### Staff: Mentor

...which makes accuracy a function of the size of the sample and decay rate. Fortunately, atoms are small so you can watch a lot at once. Ie, if the half life is one year and you watch 100 atoms, you'll only see 50 decay events. The key to accuracy is seeing enough decay events that the rate becomes regular.

This is also the same statistical problem that exists with neutrino detection.

9. Jul 13, 2012

### Staff: Mentor

Exactly. Question was about potassium, which makes dealing with large samples pretty easy. 40 g sample of potassium contains about 6x1019 atoms of K-40.

For some other isotopes it won't be that easy.

10. Jul 13, 2012

### mram10

Good discussion guys. How on earth can they watch a sample size that large?? Also, if a small amount like that has that many atoms to watch, does that make an even better case for lack of statistical sample size?? Just spit balling here, but every time I talk with my friend, we come up with more questions. I guess that is the nature of science though.

11. Jul 13, 2012

### Staff: Mentor

Where do you see a large sample? 40 g of metallic potassium is a two inch diameter ball.

No idea what you mean. You don't watch each atom separately. You put sensors around the sample and count emitted beta particles (it is more complicated, but let's not muddy water now). And it is not a problem to weight the sample with 10-6 accuracy, so that's how precisely you know number of atoms.

12. Jul 13, 2012

### mram10

Borek,

Thank you. for taking the time again to explain this. "Large sample" was referring to the number of atoms associated with 40g of potassium. By your response, it is not considered to be a large number of atoms to keep track of.

I would love to hear how they measure the beta particles. I have been watching online courses to try and understand chemistry better. If you don't want to type that much, please give me a good link that explains it easily :) Thanks.

13. Jul 13, 2012

### Staff: Mentor

14. Jul 14, 2012

### mram10

Another "dumb" question:
Have we been able to observe a chunk of new radioactive material(short half life) from inception for a significant amount of time to verify that the rate is the same from inception till decay is complete?

15. Jul 14, 2012

### Staff: Mentor

Many of the isotopes (including those used routinely in medicine) have half lives measured in hours or days, and they were researched thoroughly. The earliest samples of artificial isotopes (if they still exist) are zillions of half times old.

16. Jul 14, 2012

### mram10

Great info. What kind of this would effect the half lives of isotopes? Would heat increase or decrease the half life? Would atmospheric pressure? Water? Etc.

17. Jul 14, 2012

### Staff: Mentor

Very high temperatures could change the half life, but we are talking about tens if not hundreds of thousands Kelvins minimum. As far as I know no other factors can change half life - with one exception. Electron capture (which is sometimes treated as a variant of a beta decay) depends on the electron density around nucleus, so speed of decay can be a function of what is the compound in which the isotope is present. But it is not very common.

Last edited: Jul 14, 2012
18. Jul 14, 2012

### tiny-tim

cool! :tongue2:

19. Jul 14, 2012

### Staff: Mentor

1. There is no such thing as "complete decay" for most substances: the universe would end before every atom decayed. This is the nature of the half life.
2. Also due to the nature of the half life, there is no "age" for a single radioactive particle, so no basis for a rate change. If you have a particle with a half life of 10 years and you wait 10 years, there's a 50% it will have decayed. If it didn't decay and you wait another 10 years, odds are still 50%. Just like with flipping a coin -- it has no memory.

20. Jul 14, 2012

### Staff: Mentor

Sigh, I ate "thousands". Corrected.