Main content

## Physics library

### Unit 17: Lesson 4

Nuclei- Mass defect and binding energy
- Nuclear stability and nuclear equations
- Types of decay
- Writing nuclear equations for alpha, beta, and gamma decay
- Half-life and carbon dating
- Half-life plot
- Exponential decay formula proof (can skip, involves calculus)
- Exponential decay problem solving
- More exponential decay examples
- Exponential decay and semi-log plots

© 2022 Khan AcademyTerms of usePrivacy PolicyCookie Notice

# Half-life and carbon dating

Carbon dating is a real-life example of a first-order reaction. This video explains half-life in the context of radioactive decay. Created by Sal Khan.

## Video transcript

SAL: In the last video we saw
all sorts of different types of isotopes of atoms
experiencing radioactive decay and turning into other atoms or
releasing different types of particles. But the question is, when
does an atom or nucleus decide to decay? Let's say I have a bunch of,
let's say these are all atoms. I have a bunch of atoms here. And let's say we're talking
about the type of decay where an atom turns into
another atom. So your proton number
is going to change. Your atomic number is
going to change. So it could either be beta
decay, which would release electrons from the neutrons and
turn them into protons. Or maybe positron emission
turning protons into neutrons. But that's not what's
relevant here. Let's say we have a collection
of atoms. And normally when we have any small amount of any
element, we really have huge amounts of atoms of
that element. And we've talked about moles
and, you know, one gram of carbon-12-- I'm sorry, 12
grams-- 12 grams of carbon-12 has one mole of carbon-12
in it. One mole of carbon-12. And what is one mole
of carbon-12? That's 6.02 times 10 to the 23rd
carbon-12 atoms. This is a ginormous number. This is more than we can, than
my head can really grasp around how large of
a number this is. And this is only when we have
12 grams. 12 grams is not a large mass. For example, one kilogram
is about two pounds. So this is about, what? I want to say [? 1/50 ?] of a pound if I'm
doing [? it. ?] But this is not a lot
of mass right here. And pounds is obviously force. You get the idea. On Earth, well anywhere,
mass is invariant. This is not a tremendous
amount. So with that said, let's go back
to the question of how do we know if one of these
guys are going to decay in some way. And maybe not carbon-12, maybe
we're talking about carbon-14 or something. How do we know that they're
going to decay? And the answer is, you don't. They all have some probability
of the decaying. At any given moment, for a
certain type of element or a certain type of isotope of
an element, there's some probability that one
of them will decay. That, you know, maybe this guy
will decay this second. And then nothing happens for a
long time, a long time, and all of a sudden two
more guys decay. And so, like everything in
chemistry, and a lot of what we're starting to deal with in
physics and quantum mechanics, everything is probabilistic. I mean, maybe if we really
got in detail on the configurations of the nucleus,
maybe we could get a little bit better in terms of our
probabilities, but we don't know what's going on inside of
the nucleus, so all we can do is ascribe some probabilities
to something reacting. Now you could say, OK, what's
the probability of any given molecule reacting
in one second? Or you could define
it that way. But we're used to dealing with
things on the macro level, on dealing with, you know, huge
amounts of atoms. So what we do is we come up with terms
that help us get our head around this. And one of those terms is
the term half-life. And let me erase this
stuff down here. So I have a description, and
we're going to hopefully get an intuition of what
half-life means. So I wrote a decay reaction
right here, where you have carbon-14. It decays into nitrogen-14. And we could just do a
little bit of review. You go from six protons
to seven protons. Your mass changes the same. So one of the neutrons must have
turned into a proton and that is what happened. And it does that by releasing
an electron, which is also call a beta particle. We could have written this
as minus 1 charge. Relatively zero mass. It does have some mass,
but they write zero. This is kind of notation. So this is beta decay. Beta decay, this is
just a review. But the way we think about
half-life is, people have studied carbon and they said,
look, if I start off with 10 grams-- if I have just a block
of carbon that's 10 grams. If I wait carbon-14's half-life--
this is a specific isotope of carbon. Remember, isotopes, if there's
carbon, can come in 12, with an atomic mass number of 12, or
with 14, or I mean, there's different isotopes of
different elements. And the atomic number
defines the carbon, because it has six protons. Carbon-12 has six protons. Carbon-14 has six protons. But they have a different
number of neutrons. So when you have the same
element with varying number of neutrons, that's an isotope. So the carbon-14 version, or
this isotope of carbon, let's say we start with 10 grams. If
they say that it's half-life is 5,740 years, that means that
if on day one we start off with 10 grams of pure
carbon-14, after 5,740 years, half of this will
have turned into nitrogen-14, by beta decay. And you might say, oh OK, so
maybe-- let's see, let me make nitrogen magenta, right there--
so you might say, OK, maybe that half turns
into nitrogen. And I've actually seen this
drawn this way in some chemistry classes or physics
classes, and my immediate question is how does this
half know that it must turn into nitrogen? And how does this half know that
it must stay as carbon? And the answer is
they don't know. And it really shouldn't
be drawn this way. So let me redraw it. So this is our original block
of our carbon-14. What happens over that
5,740 years is that, probabilistically, some of these
guys just start turning into nitrogen randomly,
at random points. And over 5,740 years, you
determine that there's a 50% chance that any one of these
carbon atoms will turn into a nitrogen atom. So that after 5,740 years, the
half-life of carbon, a 50% chance that any of the
guys that are carbon will turn to nitrogen. So if you go back after a
half-life, half of the atoms will now be nitrogen. So now you have, after
one half-life-- So let's ignore this. So we started with this. All 10 grams were carbon. 10 grams of c-14. This is after one half-life. And now we have five
grams of c-14. And we have five grams
of nitrogen-14. Fair enough. Let's think about what happens
after another half-life. Well we said that during a
half-life, 5,740 years in the case of carbon-14-- all
different elements have a different half-life, if they're
radioactive-- over 5,740 years there's a 50%-- and
if I just look at any one atom-- there's a 50%
chance it'll decay. So if we go to another
half-life, if we go another half-life from there, I had
five grams of carbon-14. So let me actually copy
and paste this one. This is what I started with. Now after another half-life--
you can ignore all my little, actually let me erase some
of this up here. Let me clean it up
a little bit. After one one half-life,
what happens? Well I now am left with five
grams of carbon-14. Those five grams of carbon-14,
every one of those atoms still has, over the next-- whatever
that number was, 5,740 years-- after 5,740 years,
all of those once again have a 50% chance. And by the law of large numbers,
half of them will have converted into
nitrogen-14. So we'll have even more
conversion into nitrogen-14. So now half of that five grams.
So now we're only left with 2.5 grams of c-14. And how much nitrogen-14? Well we have another two and
a half went to nitrogen. So now we have seven and a half
grams of nitrogen-14. And we could keep going further
into the future, and after every half-life, 5,740
years, we will have half of the carbon that we started. But we'll always have an infinitesimal amount of carbon. But let me ask you a question. Let's say I'm just staring
at one carbon atom. Let's say I just have this
one carbon atom. You know, I've got its nucleus,
with its c-14. So it's got its six protons. 1, 2, 3, 4, 5, 6. It's got its eight neutrons. It's got its six electrons. 1, 2, 3, 4, 5, 6, whatever. What's going to happen? What's going to happen
after one second? Well, I don't know. It'll probably still be carbon,
but there's some probability that after one
second it will have already turned into nitrogen-14. What's going to happen after
one billion years? Well, after one billion years
I'll say, well you know, it'll probably have turned into
nitrogen-14 at that point, but I'm not sure. This might be the one
ultra-stable nucleus that just happened to, kind of,
go against the odds and stay carbon-14. So after one half-life, if
you're just looking at one atom after 5,740 years, you
don't know whether this turned into a nitrogen or not. This exact atom, you just know
that it had a 50% chance of turning into a nitrogen. Now, if you look at it over a
huge number of atoms. I mean, if you start approaching, you
know, Avogadro's number or anything larger--
I erased that. Then all of a sudden you can use
the law of large numbers and say, OK, on average, if each
of those atoms must have had a 50% chance, and if I have
gazillions of them, half of them will have turned
into nitrogen. I don't know which half,
but half of them will turn into it. So you might get a question
like, I start with, oh I don't know, let's say I start with
80 grams of something with, let's just call it x, and it has
a half-life of two years. I'm just making up
this compound. A two-year half-life. And then let's say we go into
a time machine and we look back at our sample, and let's
say we only have 10 grams of our sample left. And we want to know how much
time has passed by. So 10 grams left of x. How much time, you know, x is
decaying the whole time, how much time has passed? Well let's think about it. We're starting at time, 0 with
80 grams. After two years, how much are we going
to have left? We're going to have 40
grams. So t equals 2. But after two more years, how
many are we going to have? We're going to have 20 grams.
So this is t equals 3 I'm sorry, this is t
equals 4 years. And then after two more years,
I'll only have half of that left again. So now I'm only going to
have 10 grams left. And that's where I am. And this is t equals 6. So if you know you have
some compound. You're starting off with 80
grams. You know it has a two-year half-life. You get in a time machine. And then you didn't build
your time machine well. You don't know how well it
calibrates against time. You just look at your sample. You say, oh, I only have
10 grams left. You know that 1, 2, 3 half-lives
have gone by. And you could also think
about it this way. 1/2 to the 3rd power, because
every time you have 1/2 of the original sample-- that's the
number of half-lives-- after three half-lives you'll have 1/8
of your original sample. And that's what we have here. We have 1/8 of 80 grams. And
this is just when you're doing it with a discreet you know,
when you're right at the half-life point. In the next video we're going to
explore what if I asked you a question, how many of the
particles, or how many grams will you have in exactly
10 days? Or at two and a half years? And we'll do that in
the next video.