All language subtitles for The Modern Alchemist 1of3 Air The Elixir of Life_Subtitles01.ENG

The alchemists were a mysterious
group of medieval scientists

who believed their knowledge of
chemistry gave them magical powers.

They could summon fire,
produce mystical potions.

They even tried to turn
metals into gold.

Their magnificent feats enthralled
kings and commoners alike.

But they never revealed
their secrets.

By pushing the frontiers of science,

modern chemists can perform
equally impressive feats,

and we're happy to tell you
everything.

APPLAUSE

Chemistry gives us an understanding
of the world

that the other sciences just don't.

It's all about how one
substance interacts with another

to give us something new.

Thank you. Take this Christmas
tree here, for instance.

A nice, solid structure, but watch
what happens when I do this.

Whoa!

APPLAUSE

Well, we certainly
saw that a change took place there.

That was a flash of light,
I felt a blast of heat,

heard a whoosh of sound
and then nothing was left at all.

Trying to understand what happens

when one thing changes into another
is chemistry.

My name is Dr Peter Wothers,
and I am a chemist.

APPLAUSE

Now, the ancient Greeks thought that
everything around them

was made up of just four elements.

Air, water, earth and fire.

We see these here.

In the next three lectures,
we're going to look at what air,

water and earth
are really made up of.

But don't worry,
there will be plenty of fire
in all of the lectures.

But this brings me
to one important point.

Please do not try
these experiments at home.

By understanding the elements
around us,

the modern building blocks
of science,

we need to look at the world
in a different way,

we need to see these elements
through the eyes of a chemist.

By understanding these elements,

we can make better materials
and better medicines for our future.

We're going to start this
first lecture looking at the air.

Now, of course, this is something
that we rarely think about,

but without it, we'd all be dead.

But just to show you that
it really is here around us

pushing down on this,
I've got a demonstration,

but I'd like a
volunteer from the audience, please.

Right on the corner there,
at the back, yes,

would you like to come down
to the front, please?

OK. Now. What's your name, please?
Xavier. Xavier. OK.

Right. So, see this here?
This is just a normal oil drum.

It seems to be
covered in a bit of rubbish.

Hold this, give it a good whack.

Go on, bit harder than that. OK.

It really is quite solid, isn't
it? On the top as well, maybe. OK.

Yeah. Do you think
it's pretty solid? Yeah.

Now, watch what happens when we take
the air out of this drum.

At the moment, there is of course
a scope open at the top here,

there's air inside, air outside, but
we're going to put this pump on here

so we're now removing
the air from this drum.

OK. And... That's good. I think you
should just step back. That's it.

You stand over there.
I'll stand over here.

OK, so we're removing the air
from the inside of this drum.

To start off with,
the air molecules were pushing

against the drum, but they're also
pushing from the outside as well.

So what do you think will happen
if we remove the air from inside?

Any ideas? It will shrink.
It will shrink?

So do you think it will gradually
shrink up and get smaller?

Yeah? Well, that's a good idea.
That's what we think.

It doesn't seem to be doing
very much at the moment, does it?

So, not a lot.

Well, supposedly,
these little air molecules

are all pushing down on this can
here. We're taking...

BANG!

GASPING

Come and have a look. You feel that.
It is very solid, isn't it?

Yeah. That was just the air.

So we do forget about it,
but it really is pushing down on us.

It's quite a strong force.

It's like there's two full-grown men
standing on your shoulders.

We don't notice it because we're
used to it, we've adapted to it.

Thank you very much. Give him
a round of applause. Thank you.

APPLAUSE

But what about our tree?
What happened to the tree?

Well, what would the ancient Greeks
have thought if they had seen that?

What would they have made
of this strange substance?

Well, this, actually,
the Greeks never saw.

This is a substance
called guncotton.

It was only discovered
around 200 years ago.

It's quite remarkable.

The Greeks would've said that this
is changing into fire and air.

Maybe they would've said
this is made of fire and air.

Or maybe they would've
just said it's magic.

Either way, they would be wrong.

We now know that the air
is much more complicated.

It's a mixture
of different components.

To show exactly what the air is made
up of, again I need a volunteer.

There's a hand very quickly.
I saw your hand.

Would you like to come down,
please? Thank you.

Can we have a round of applause,
please?

OK, your hand shot up very quickly
there. What's your name? Nadia.

Nadia. OK, excellent.
Now, have you made air before?

Oh, having to think about that one.

Have you made air before,
mixed it up? No. Exactly.

Of course, the alchemist would never
have done this, either.

They didn't know what was in the
air. Do you know what's in the air?

No. No. No? Oh, come on, have a
guess. Do you know any of the gases?

Oxygen. Very good, you see, oxygen.
Do you know any other ones?

Carbon dioxide.
Carbon dioxide, exactly.

So we're going to see how many
of the different gases are in air.

Would you like to come over here?

So these are some gas cylinders,

and we've got the
different proportions of the air

you're going to add to this
cylinder of water here.

OK. Now, the first one
is the most common gas.

It's not oxygen, and it's not carbon
dioxide. Does anybody else know?

Do you want to shout it out?
Nitrogen.

Nitrogen. Yes, exactly.
So the most common gas is nitrogen,

and this is what we have here,

so I'd like you to turn the tap
for me, please. This tap here.

This is going to let
some nitrogen in.

Now, we're aiming to get to
this mark here.

This is 78%. If we get up to here,
it's 100%. That'd be 78% nitrogen.

So, there's a lot of nitrogen
in the air, isn't there?

There's all this. Look at this.
You've got to stop it.

You've got to get this red mark
here on the black mark,

so you've got to get this
just right.

This is our nitrogen, and this is
going to be 78%.

Oh, stop, stop, stop, stop, stop,
stop, stop! You've gone past. Sorry!

Oh, dear, what a disaster.
That's OK. Look, there we are.

There we are. Spot on.

78%. Well done, that's fantastic.
Excellent. OK.

Now then, the next ingredient,
what's the next ingredient?

Nitrogen? Oh, sorry. We've done
nitrogen. What's the next one?

Carbon dioxide. No. You like your
carbon dioxide. Oxygen. It's oxygen.

You're absolutely right.
Very important one.

Right. So this is our oxygen. OK?
You're absolutely right there.

You ready to go again? Yeah.
Not yet, not yet.

We've got to go to 21%.

Now, 21%,
that takes us to about here,

I think. OK, that's 21-ish. Yes.
So you're aiming for here, OK?

Go on, then.

That's it. Very good.

So there's
quite a lot of oxygen as well.

I can see the concentration now.
That's what we need. Very good.

Oh, look at that.
Just about spot on again.

Remarkable. OK. Very good.

Now, then. Now, we're coming to
the third most abundant gas.

So far, we've got 78% nitrogen,
we've got 21% oxygen.

We've almost run out of everything
else. That's only 1% left.

Does anyone know
the third most abundant gas?

You haven't mentioned this one yet.
Does anybody know? Shout it out.

SHOUTING

All sorts of different replies
there, but it is, in fact, argon.

I think some people said argon.
Pat yourself on the back there.

It is argon. Right.

This is a tricky one now,
but you're getting very good.

All right. Argon. This is
just 1%, so that's about there.

Can you see that? Yeah. About here,
here it is, OK?

OK. Go on, then. Go on.

Oh, wrong one. The audience
are watching. The argon one.

That's it. Give it a go.

Brilliant.

There we are. Look at that. That is
very good indeed. Now, then.

APPLAUSE

We're coming to your favourite gas.
Which one's that? Carbon dioxide.

Carbon dioxide, exactly. But there's
not a lot of carbon dioxide.

In fact, it's 0.037% carbon dioxide.

Unless we did this 200 years ago,
it would've been quite a bit less.

We've increased the amount,
but anyway...

So carbon dioxide, we just need
a quick burst from that, so
quick burst. That's it. That'll do.

That's your carbon dioxide.

Hardly any at all,
but nonetheless, very important.

All the plants need that.
So that's our carbon dioxide.

You still haven't made
perfect air yet.

We could breathe this, that would be
OK, but there are some other gases,

and these are some rather rare gases

but we've put all of these
in this little syringe here.

Would you like to just
add your last bit of gas,

so just push the plunger down
and watch for the bubble.

That it is, there we are.

There, excellent.
That's the last gases.

This is neon, helium,
krypton, and xenon.

They make up just a tiny proportion
of the gas.

You did very well there.

Thank you very much.
Give her a big round of applause.

APPLAUSE

OK, so now then we know that air
isn't just one element,

but a mixture of many.

Before we look at these different
elements from air in more detail,

we want to see all of the elements
that occur in nature.

Now this is where you come in.

You've got your cards here
for different elements

so, if you're a member of
the periodic table, get ready,

but to help us with this,
would you please welcome,

straight from the West End,
the cast of the musical Loserville?

APPLAUSE

# There's antimony, arsenic,
aluminium, selenium

# And hydrogen and oxygen
and nitrogen and rhenium

# And nickel, neodymium,
neptunium, germanium

# Iron, americium,
ruthenium, uranium

# Europium, zirconium,
lutetium, vanadium

# And lanthanum and osmium
and astatine and radium

# And gold and protactinium
and indium and gallium

# And iodine and thorium
and thulium and thallium

# There's yttrium, ytterbium,
actinium, rubidium

# And boron, gadolinium,
niobium, iridium

# And strontium and silicon
and silver and samarium

# And bismuth, bromine, lithium,
beryllium, and barium... #

Barium - very good!

# There's holmium and helium
and hafnium and erbium

# And phosphorus and francium
and fluorine and terbium

# And manganese and mercury,
molybdenum, magnesium

# Dysprosium and scandium
and cerium and cesium

# And lead, praseodymium
and platinum, plutonium

# Palladium, promethium,
potassium, polonium

# And tantalum, technetium,
titanium, tellurium,

# And cadmium and calcium
and chromium and curium

# There's sulphur, californium
and fermium, berkelium

# And also mendelevium,
einsteinium, nobelium

# And argon, krypton, neon, radon,
xenon, zinc and rhodium

# And chlorine, carbon, cobalt,
copper, tungsten, tin and sodium

# These were the only ones they found
back when this song was written

# There are another 60 - now we'll
show you where they're sitting... #

Stand up, as well? Excellent!

APPLAUSE

You did very well. My whole periodic
table should be standing now

but would you please give a round of
applause for the cast of Loserville?

Thank you very much.
APPLAUSE

OK, well, that was certainly chaotic

but you did fantastically well
there.

If you'd like to take your seats.

Now, what about this
sort of random order?

You were springing up all over the
place. Was it really a random order?

Well, actually, it's not.

There is some logic behind this,
but to understand the logic

we need to look
right into the heart of the atom.

So atoms, as far as the chemists
are concerned at least,

are made up of three
different particles.

In the heart of the nucleus,
there are positively charged protons

and neutral neutrons.
We can see these on the screen.

So the red ones are the protons,
the blue ones are the neutrons.

But then circling around,
we have these electrons.

It's the protons and the neutrons
that give an element its mass,

make it quite heavy, so if you pick
something up and say it's heavy,

well, that's because
of the protons and neutrons.

But it's these electrons that are
right around the outside,

and whenever you touch anything,
what you're touching there is
electrons.

I bet you've never thought of this
before, but if we shake hands
we're shaking electrons there.

OK, that's our electrons touching
each other there. Anyway, right!

So, here we have our atom.

We now understand what atoms
are made of

but what's that got to do
with the periodic table?

Well, what makes an element unique
is the number of protons
in the atom.

We don't really care
about the neutrons

and if it's a neutral atom,

of course the number of protons are
balanced by the number of electrons.

Hydrogen, where are you? If you'd
like to stand up, hydrogen.

You are the first element,

in fact the most abundant
element in the universe.

You've got one proton.
That's what makes you hydrogen.

One proton and one electron for
the neutral atom. Sometimes neutrons
but we don't care about those.

The next element, on the same row,
we go all the way round to here

and we find helium. You have two
protons - that's what makes you you.

Then we come back over here to the
periodic table. You're very good.

Lithium, you've got three protons
and that's what makes you you,
and so on.

That's what we do when we go
from one element to the next.

We increase the number of protons
by one and the number of electrons

in the neutral atom,
and maybe throw in a few neutrons.

Now, the question is, though,
we've got 118 elements

but we've got literally tens
of millions of different compounds

so how can we get such complexity
out of just these 118 elements?

In fact,
in this cup of coffee alone,

over 2,000 different compounds
have been detected so far -

so loads of compounds,
only 118 elements.

There's a nice analogy between
letters and words with these
elements and their compounds

so I could be saying hundreds
of thousands of different words now

but these are all made up of the
same 26 letters of the alphabet.

Words like "I" and "a"
are made up with a single letter.

There are some words that have
two of the same letter.

Aa is a type of Hawaiian lava.

What a silly word that is. But then
there's another Hawaiian word.

This is aaa, or something like that,

which is an insect
also found in Hawaii.

Our elements have
the same sort of thing.

The letters then correspond
to the elements,

and there are some elements
that just stay by themselves,
like these letters.

Helium, can you put your card up,
please? Where are you? There you
are. And neon, and argon.

All of you,
you just stay by yourselves,

just single letters if you like.
Single elements.

Then we have other elements that go
around in pairs. Where's nitrogen?
Put your card up.

Oxygen, fluorine,
all of you go around in pairs.

Chlorine, you go around in pairs
as well, so you go around in pairs

and occasionally oxygen - just stand
up again, oxygen - occasionally

you have three oxygen atoms that
make up a molecule of ozone.

OK, thank you very much, elements.

But most of the periodic table,

you are loads of these single atoms
together, joined together to form

big masses of metal or non-metals,
or whatever you are,
if you're solid.

So this would be like a word
like "aaaaa" going on for ever,

with so many letters
we couldn't count them.

That's not how we usually
find the elements.

How we usually find them

is combined with one another
to form compounds

so if the letters correspond
to our elements,

the words that we use,

these correspond to different
combinations of the elements -
these are the compounds.

So, the elements want to combine
with one another to form different

molecules and we are going to try
an experiment now to show this,

to show the combination
of two elements

and this is the element oxygen,
one of the elements from the air.

Oxygen, where are you again?

There's oxygen. And between
phosphorus. Phosphorus.

Can you please stand up, phosphorus.

OK, now, do you know how you were
first discovered, phosphorus? No.

OK, well, we'll give you a bit
of a clue. What's your symbol?

P.

P. Any idea? No?
Does anyone else know?

OK, there's a chap
right at the back there.

So where do you think phosphorus
was first discovered? From wee.

From wee, yes, exactly.

OK, so thank you, phosphorus.
You can take a seat now.

I've got some urine here -
it's only mine so it's not too bad.

AUDIENCE: Eurgh!

It's all right! Smells quite nice.

Do you want a sniff? Oh, you do! OK!

LAUGHTER

It's fine!

Don't worry -
it's only apple juice, really!

But...OK,

but back in 1669,

the German alchemist Hennig Brand
did take his own urine

and he heated this up
and this amazing substance came out.

This was phosphorus. How come
phosphorus was discovered so early?

Not just because it was disgusting,

but also because once you found it
you couldn't miss it.

It just screams out to you,
"Here I am!"

OK, let's try this.

We've got some phosphorus
in this flask here

and I'm just going to
let the air into this.

We've removed the air
and heated up the phosphorus,

and watch what happens here.

Maybe we can have the lights down
just a little bit here.

So, as soon as the air comes in,
it combines with the phosphorus.

This is phosphorus
reacting with air,

and this amazed the alchemists.

When they saw this,
they were truly stunned.

In fact, they were so impressed
by this amazing light

that the reaction has given out,
they named this element phosphorus,

which means "the light giver".

This discovery was commemorated
with a painting by Joseph Wright
of Derby, that's on the screen here.

It has a really catchy title.

It's called "the alchemist in search
of the philosopher's stone

"discovers phosphorus and prays
for the successful conclusion

"of his operation,
as was the custom of the ancient
chemical astrologers".

Snappy, but it sort of says what
it is, and you can see this,

this amazing look in the alchemist's
eyes as he's made
this fantastic discovery.

This was far brighter than any of
their lamps or candles at the time.

I have a description here.
This is from a book from 1692.

It describes phosphorus.

It says you need to store it
underwater because
it reacts with the air,

but it also says here,

"If the Privy Parts be therewith
rubb'd, they will be inflamed and
burning a good while after."

Now there's one that you really
shouldn't try at home!

Please don't go smearing phosphorus
on your privy parts. It's not fun.

Anyway, but the alchemists made this
discovery. They found phosphorus.

They knew it was reacting
with the air

but they didn't understand
fully what was going on

because they didn't know
what the air was made of.

Chemists now know
that it's a mixture of gases

and a mixture of different elements
that makes up the air.

Now, we're going to have
a look again at the different gases
that are in the air.

In fact, first of all, can we have
all the elements that are gases?

So, all the gaseous atoms.
Can you stand up, please?

So, where are all the atoms that are
gases? We have hydrogen over here.

Well, it's a good job there's not
too much of you in the air

because that would make it very
flammable, so if you sit down.

It would all explode
if there was too much hydrogen

and that wouldn't be very
good at all. Who else?

Nitrogen and oxygen, we know
you're the major components,

but we've also got fluorine
and chlorine.

Fluorine and chlorine,
you are incredibly reactive,

which also makes you incredibly
toxic so it's a very good thing

that you're not in the air as well
so perhaps you can sit down as well,
please.

Look where the gases
that we do find in the air are.

We've got nitrogen and oxygen,
we've seen you, but then we've got

all of you sitting here -
well, standing here -
with the white cards.

You are the so-called noble gases.
Why are you all sitting together?

This is not a coincidence, it's
because you all have very similar

chemical properties and there's this
amazing pattern when we arrange

the elements in a certain way,
that every so often

elements with the same chemical
properties are found
grouped together.

So if we just have our periodic
tables up, please.

That's it, fantastic, very good.

We can see these coloured patterns
here.

What a beautiful display this is.
Excellent.

All of you with the purple cards
here, you are group one.

You're all really reactive metals,
you explode with water.

Really violently, OK?

You all have similar properties,
you're all grouped together.

If we come over here, all you with
the green cards for instance,

you're called the halogens.

You're really poisonous,
rather unpleasant substances,

but you combine with these over here
with the alkali metals,

and you form salts
very violently indeed.

OK, at ease, periodic table.

We're going to look, though,
at our noble gases.

So, if everyone sits down, but I'd
like the noble gases now
to come down to the front.

We've got some samples for you.
A balloon of krypton.

Hold the string and hold it out.
Beautiful.

OK. Xenon, again, hold the string,
there we are.

And then we come... Ah! We have
a slight problem with radon,
I'm afraid.

Radon is incredibly radioactive

so health and safety wouldn't let us
give you a balloon full of radon.

You would go home glowing, so we'll
just put this one on you there.

That's great.

And ununoctium, I'm afraid
ununoctium hasn't even got a name

and this is because there's so few
atoms of ununoctium that were made,

or we're not even sure
if they were made,

but we couldn't fill a balloon
full of you. But you got
a balloon anyway!

LAUGHTER

OK, so, mm-hmm, right.

Now, you've all got your balloons

and after a countdown from three,
I'd like you to release
your balloons.

Keep hold of the strings, though,
and we'll see what happens.

So three, two, one, go.

Ah! Look at that.
Now, what do we see here?

We all know
that helium balloons float

so you've got a nice light element
there, helium. What about this neon?

Neon, hmm, it's about the same.
You've dropped your string.

Keep hold of the string. It's about
the same sort of density as air.

It's the balloon that's making
it sink. Argon is getting pretty,
er... Whoops! More dense there.

Keep hold, thank you.
Krypton is really quite heavy.

And xenon, hmm, you wouldn't want to
go to a party with that, would you?

You would be dragging
this along the floor!

It's a very expensive gas -
it's about £100, this balloon,

but yes, it's very heavy indeed.
What does this tell us, though?

Each of these balloons actually
has the same number of atoms

because equal volumes contain
the same number of particles.

It tells us that the atoms of helium
are much lighter
than the atoms of xenon

and that's because of the subatomic
particles that make up these atoms.

The helium just has two protons
and two neutrons

all the way down to ununoctium -
you have 118 protons
and loads of neutrons.

I think you've done
fantastically well.

Would you like to return
to your seats? Thank you.

APPLAUSE

We've seen that we've got different
densities of these gases,

they have different masses,

but they also have
very similar properties

and each of these elements is a gas

and we've filled these signs up
with these gases.

We can see that
you're all colourless.

You're also all odourless gases,
which is a good thing.

You don't smell at all,
but not very exciting to look at,

until you pass a few thousand
volts through you.
Watch what happens then.

They all become much prettier.

This is the normal neon
signs that we see.

This sign here is filled with neon
gas, but when it gets excited

with the electricity there,
the electrons are leaping up,

and as they come back down
we get this fantastic red colour.

Each element has its own
unique colour

so we can see, then,
that some of these gases have uses.

Neon is used in neon signs.

But some of them have even more
important uses, and I went to the

University of Sheffield to have a
look at one of the uses for helium.

So what's in this little bag
here that I've got then, Jim?

What you've got in there
is essentially a bag
with some helium atoms,

which are magnetically
aligned or polarised.

They are contained within the bag.

If we were to actually image
the bag, you'd see

just the boundaries of the bag
and the air space inside the bag

filled with the gas and nothing
on the outside and, similarly,

when you breathe it in we will
see the gas inside your lungs.

The scanner is actually a giant
magnet with radio detectors

which detect the specially prepared
helium atoms as they return

to their natural state
within this magnet.

This allows Jim
to build up a picture of where
the gases are in my lungs.

Your scan is here.
Those are my lungs?

There's your bronchus, trachea,
and your two bronchi,

main feeding bronchi
coming off the bronchus.

These are your blood vessels.

So the amazing thing about this
is that we are only seeing

the air inside my lungs,
aren't we? Exactly.

You're just visualising
the air spaces there.

It's very exciting to be
looking at my own lungs!

It's nice to know they're not
too bad, even though

I know I've got a bit of a cough
at the moment.

Nonetheless, they're reasonably
healthy, you think? They look pretty
healthy. That's all right, then.

So this is pretty cutting-edge
science here.

We're actually using this
form of helium, helium three,

to image the workings,
how our lung works.

And actually on the screen we
can see here, these are two lungs.

This is a lung of a patient who has
asthma on the left-hand side here.

You can see some black regions.

But after they've taken their
inhaler, the lungs have opened up,

the airways have opened up, and the
helium has gone into those regions.

We can see all the places
where the air is now reaching.

So this just shows
the medicine in action.

OK, now, it's not just helium
that has exciting properties.

If we go right the way down to the
bottom of the periodic table here,

the heavy stable element xenon,

this has some truly remarkable
properties as well.

We have a tank here and we've filled
this with some xenon, I understand.
A little, yes.

A little xenon so we just keep
putting a little bit more in there

and I have a very delicate,
very fragile foil boat.

I'm going to see if we can
actually balance this,

if we can float this on the xenon
in this tank.

Try this one.
Shall we try this one first?

Yes, we'll try our new boat.
Just slide this over.

And try our new boat.

Ah! That's it. Look at that.

That really is...
APPLAUSE

..floating on the xenon.

There are no strings.
It's a little bit fragile here.

I think I need a volunteer to just
come and very carefully help me

add some weight into this.

We'll have somebody from, er, the...
Yes, right on the end.

Would you like to come down?
Thank you.

OK, thank you very much.
Give her a round of applause.

If you'd like to come round here.

I'm just trying to keep my boat
level here.

Just add a little bit more xenon.
What's your name, please? Bethany.

Bethany, excellent.

Now, you are going to be probably
the first person in the world

ever to try this -
we haven't even practised this.

Have a look at this.
What do you think this is? Hold it.

Foil. It's foil.
Does it feel like normal foil? No.

No, it feels strange, doesn't it?
That's because it's pure solid gold.

Right?

This is pure solid gold so let's
just screw it up a little bit

and I'd like you
to put this in here.

Just see if you can put it
in that corner.

That corner is a little bit unstable
at the moment. That's it.
Oh, look at that!

Now you have made this thing float
perfectly. That's pretty amazing.

Add some more. Will you sink it?

Not quite. Oh, there it goes.

Fantastic! A world first.

Thank you very much, excellent.

APPLAUSE

OK, xenon is very dense and I'm very
pleased that worked, but it also has

some really remarkable properties
that can be used in medicine.

Now, while I was at
the University of Sheffield,

we took a chance to experience
what it's like to breathe in

some xenon and it has very
strange effects on the body

but it can be very useful as well,
so let's just see what happens here.

If you take a deep breath in, Peter.
Breathe out.

Deep breath in.

Breathe out,
and now breathe from the bag. OK.

Breathe in, breathe in, breathe in,
breathe in, breathe in, breathe in,

breathe in, breathe in, breathe in,
breathe in, breathe in, breathe in.

OK, and hold your breath.

It will be interesting
if you talk as you breathe out,

we'll see if we can hear the, er...

DEEP VOICE: That's amazing.
I feel really relaxed

and I can hear that my voice
has changed.

It's gone quite deep now
but I feel very happy and relaxed

and calm. Oh, it's wearing off now.

Wow, so that's xenon,
these individual atoms of xenon,

interacting with my brain
in some way, isn't it? Mmm.

So it's going into my bloodstream
and interacting with my brain

and making me feel slightly
light-headed. Mmm. And that's...

At higher concentrations,
that acts as an anaesthetic

and I would just pass out,
is that right?

People do use it as an anaesthetic
in a clinical setting,

but clearly at higher
concentrations than these.

If we'd have retuned the scanner
slightly, we'd have actually seen

the xenon atoms dissolved
in your blood as well.

That's where we're going
with this at the moment.

We'd love to actually be able
to pick up the xenon

dissolved in the brain
and image the xenon in the brain.

That might give us
some insight into how these

anaesthetics are actually
working in the neural system.

Incredible. Yeah.

Now, that was certainly very strange
when I was breathing in this gas

and the latest research that Jim
is doing allows the individual atoms

of xenon to be followed
around the brain, even.

Now, I'd like you to welcome three
incredibly important guests

to the RI. Would you please welcome
Dave, Sarah and Riley Joyce?

APPLAUSE

Good to see you.

Thank you very much. Hello.
Thank you.

Ah! He's very shy in front
of the cameras here.

I was wondering if...
Could you tell me your middle name?

What's your full name?
Can you tell me your full name?

A bit shy. He's a bit shy, but what
is his full name, then, please?

It's Riley Xenon Joyce.
I think this is great.

I would love to have an element
for a middle name, I must say.

So why is Riley's middle name
Xenon, then?

Well, Riley was the first
baby in the world to receive xenon,

and he received it at St Michael's
in Bristol,

due to when he was born
he didn't have a pulse

and they had to resuscitate him
so he was starved of oxygen.

This could have caused complications
if he didn't get this
treatment at the time,

so this was acting
as an anaesthetic.

Would it just gently put him to
sleep and allow the metabolism
to slow down?

It has given his brain time to
recover and he had it alongside

the head-cooling treatment,
which works on the same principle.

I must say that he's very shy
at the moment in front of everybody

but earlier he was running around
all over the place

so he's clearly perfectly healthy
now, isn't he? Is that right? He is.

In March this year
he had his two-year check-up

and he was discharged as a
perfectly normal, healthy child.

When he was born, he was given
a 50% chance of having
permanent brain damage

so to come from there to where
we are now is incredible.

That is absolutely fantastic.

So would you please thank them
for coming in?

APPLAUSE

If we just have our periodic
table up for a moment.

Have our periodic table up.

We've seen that we
have our noble gases here.

You're all individual atoms,

you don't really want
to combine with the others,

but this isn't the same throughout
the periodic table as a whole.

We're trying to understand what
makes some of the gases in the air
so special,

but in order to understand these,
how they're bonding with each other,

we need to look across
the periodic table as a whole.

I have a sample of one
of the elements here.

This is the element potassium.
Potassium, can you stand up?

There you are.

So you're in this first group,
the same group as lithium, sodium,
potassium. Thank you.

You're a solid, and in here
we have the solid potassium.

Potassium is a metal,
and we've got this in the flask.

At ease, periodic table. Thank you.
Cards down. Very good.

We've got a little piece of
potassium here, and we've taken
the air out of this flask.

And I'm just going to gently
warm the flask up.

So potassium is a metal.

The potassium atoms
want to bond to each other

but they don't bond to each
other very tightly.

So it is a solid, though,
not a gas like our noble gases,

but watch what happens
if I just warm it up rather gently.

Potassium is... Oh, look at that.

What's happened here, all of the
potassium atoms have separated

from each other and given this
fantastic coating over the inside.

In fact, we've made an instant
Christmas bauble, which is great!

But this is a Christmas bauble
coated with potassium,

which is probably not so great.
But anyway, very beautiful,

but we didn't need to put a lot
of energy in to pull those apart.

How can we understand this?
We're going to go back to...

If we have the periodic table
back up,

we're going to go back to the top
element in this second row.

This is lithium,

and we're going to move round the
periodic table from lithium

through beryllium, all the way -

boron, carbon, nitrogen, oxygen,
fluorine, neon - and see
how the bonding changes.

We have our elements lined up
and bringing down electrons

so can we have the first two
lithiums, please?

Could you come down to the front,
and you're bringing some electrons
with you.

So these are our yellow electrons

and could you put them
in the energy level here, please?

That's it, put them in there,

and if you return to your seats,
that's great. Thank you very much.

What's happened here,
as the electrons have gone
into this region here,

into these shelves here,
these have pulled the atoms together

and this is because these
negatively charged electrons

are helping pull the nuclei together

when they're concentrated
in between the two atoms here.

Can we have our next elements?

We have beryllium -
could you come down?

Now, on beryllium we see
on the screen here
the bonds are much stronger.

Let's see why this is.
We add your electron here.

That's it, these are moving
the atoms closer together,

so even stronger still.

So beryllium has two electrons,
creates a stronger bond now.

Lithium, beryllium. The beryllium
atoms are held more tightly.

OK, boron, on the screen here,
we have three electrons.

Can you come down please, boron?
You've got one more electron here
than the beryllium had

so you're going to add
your electrons. Could you add
your electrons in here?

And again, these... Oh! That really
did move, that was pretty good.

So you've a very strong bond
now for the boron -

much stronger than the beryllium.
Very tightly held.

We've got three electrons bonding
these boron atoms together.

Can we have carbons now, please?
OK, and that last one.

OK,
so the atoms move closer together.

Thank you very much, carbons.
We've got some very strong bonds
indeed now.

In fact carbon there requires most
of the energy of all of the elements
to try and rip them apart.

If we were trying to remove the same
number of atoms apart,

we need more energy
for carbon than any other.

This makes carbon incredibly strong.

I have a sample of carbon here
to show you and demonstrate this.

This is a diamond, we can see this
here. This is a real diamond.

Very, very strong
because of these strong bonds.

I nearly dropped it there.
But it is also incredibly hard.

So hard, in fact, that
I can actually cut this glass.

The glass is incredibly hard, of
course, but diamond is even stronger

because of the strong bonds
between the carbon atoms. So...

It's definitely cut into the glass.
In fact, it looks like
it's pretty deep.

There we are. It's cut down this
crack where it's been scored
with the glass there.

So a diamond, incredibly strong,
because of all these
bonding electrons

keeping the carbon atoms together.

We've still got further to go
along our periodic table.

We've gone to carbon,
we're going to keep on going.

So nitrogens,
you have five electrons in total,

so let's see where these have to go.
We've run out of room here.

You're going to have to put
your electrons in these ones

so this is a slightly different
thing going on here.

Would you put your electrons
in here? That's great.

And these, actually, now are
concentrated outside of the middle

and these electrons are pulling
the atoms further apart again.

In fact, these do not help
the bonding. These are called
anti-bonding levels.

Thank you very much, nitrogens.

OK, we have our next element -
this is oxygen.

Let's see what happens as we keep
going, adding another electron.

Oxygens, you have to put yours
in this level here,

and again these are in these
anti-bonding levels,
pulling our atoms apart.

So oxygen is a weaker bond
than nitrogen.

Let's go to our next atom.
We've got two fluorines coming.

Let's see what happens when you get
together. OK. Add them in.

That's great. Again, a very weak
bond now. It's pulled further apart.

Fluorine has one more electron,
weakens the bond here

and the fluorines are really
weakly held together.

This is the one of the reasons
that makes fluorine

so incredibly reactive.
It's because of these weak bonds.

Finally, we have
our last element, neon.

So, neon has eight
outermost electrons,

so it has one more
than the fluorines had.

Let's see where these have to go
in the remaining level here.

So if you add your electrons into
these last anti-bonding levels...

And it pulls the atoms
completely apart.

So, this means the atoms do not
bond to each other.

Thank you very much indeed
for your help there. Thank you.

APPLAUSE

So, if we just see our periodic
table again. Just have you up.

That's great. Thank you very much.

We're looking at these ones
over here.

We see carbon,
very, very strong bonds.

Nitrogen, not as strong as carbon,
but still pretty strong.

Fluorine, very weak bonds.
Neon not bonded at all.

But oxygen, you're just
about the right strength.

You're still reactive because the
bonds aren't too incredibly strong

between the oxygen atoms.

Makes you very,
very reactive indeed.

Oxygen, you really are
the elixir of life.

It's you that keeps us all alive.
I'm going to demonstrate this now.

So, at ease, periodic table.
Thank you.

So, I have some breakfast
cereal here.

This is just normal breakfast
cereal.

I'm just going to put some
in the bowl.

This is just the sort of thing
that you would normally do.

But now instead of adding my milk...
Oops.

Instead of adding my milk,
I'm going to add some liquid oxygen.

So this is not the sort of thing
you normally do.

We've cooled the oxygen down.
So this is oxygen gas

that's been cooled down.
It has this beautiful blue colour.

I'm just going to pour
this onto our Rice Krispies.

OK. Now, I'm also going
to add a light.

Just put my goggles on.

This is also something
you don't normally do.

An incredible amount of energy
is released there.

This is as the Rice Krispies,
the breakfast cereal here...

As our breakfast cereal combines
with the oxygen from the air.

And believe it or not,
this is actually what happens

inside our bodies.
Not quite like this.

We don't have flames
coming out of our ears.

But nonetheless, it is the reaction
between our breakfast cereal

and the oxygen that we're breathing
in that gives us

the energy to stay alive.

And we have Laura here
to demonstrate this.

She's been specially trained
in breathing

with this rather delicate
apparatus here.

OK. Would you like to put this on?

Now, what's happening here?

Laura is breathing in.
So if you breathe in...

Breathing in normal air
and it's coming in through here,

bubbling through this solution.
In the flask here,

we have something called
lime water.

Then Laura's breathing out through
this one. So the out air

is coming out through here.

Now, lime water reacts
with carbon dioxide.

There's very little
carbon dioxide in the air,

so there's no change
taking place here.

When lime water reacts
with carbon dioxide,

it turns cloudy due to
the formation of calcium carbonate.

No calcium carbonate forming here.
But in the out...

Well, we can begin to see already...
Keep breathing. Very good.

You're breathing beautifully there.
OK. In the out, we can begin

to see that it is going cloudy.
And this is because inside Laura,

it is the same reaction
we saw taking place there.

The breakfast cereal Laura
had this morning is reacting

with the oxygen she's breathing in.
It's releasing a lot of energy

and that's keeping her alive, but
she's breathing out carbon dioxide

that is formed during
this process as the oxygen reacts

with the fuel to produce
carbon dioxide.

Thank you very much.
Give Laura a round of applause.

APPLAUSE

So, oxygen is incredibly important
just to stay alive.

But we've seen that there's
only 21% of oxygen in the air.

So, wouldn't it be better if there
was much more oxygen in the air?

Well, probably not.

I'm going to demonstrate this now
with the help of my volunteer here,

sausage man. OK. Now, sausage man
is made of the same sort of things

that I'm made up of.
He's made up of meat, of course.

And I'm just going... We've
connected him to a heating wire.

I'm just going to turn up this
heating wire here. So, there we are.

The heating wire is just...

Just turn it on
a very low voltage there.

It's just beginning to heat up.

Now, it's not really causing
too much of a problem.

But watch what happens if I increase
the amount of oxygen in the air.

Again, we're going to use the
liquid oxygen to do this.

It's just to provide a lot
of oxygen gas in the environment.

So he's just with
the heating coil there.

Is anything beginning to happen?

His leg's smoking a bit
as the wire's heating.

So this is like you're
on a different planet

and there's a lot of oxygen
on the planet here.

You accidentally lean
against a cooker...

And look what's happening here.

Poor sausage man is now in flames.

He's gone up rather
drastically here.

This is because of the increased
oxygen in his environment.

So, yes, of course,
we do need oxygen to stay alive.

It does provide us with our energy.

But too much would
definitely be a bad thing.

I need to put out our sausage man.
I think it might be very difficult

to put him out since there's
so much oxygen in there.

Let's try... We've got
some tomato ketchup here.

LAUGHTER

It's...

Wow.

It leaks as well. Great. Somebody
didn't put the top on properly.

There we are. We've put him out.

Oops. What a mess. OK.

OK. So, you get the idea

that too much oxygen would
certainly be bad for us.

But on a serious note, it's
incredibly difficult to put out

a forest fire.

These are incredibly difficult to
put out, even with just 21% oxygen.

If it was 100% oxygen,
there would be no chance.

So 21% of the air
is made up of oxygen.

This is how much we need to breathe.

But what happens if you reduce
the amount? Can we still stay alive?

Well, I went to a place
just outside Cambridge

where they've reduced the amount
of oxygen in their rooms there

from 21% down to 15%.

And they say that things just
can't burn in this environment.

Well, let's see what happened.
Can I have a fire? Yes.

Can I set fire to your newspaper?
I've got a newspaper here

and you try to light my newspaper.
OK. All right.

See if it works. Shall I use
a lighter? Use the lighter.

I'll try the lighter first of all.
OK.

Oh. Empty? I don't think
it's a very good one.

Try mine if yours is empty.
This is a new one, is it?

OK. OK. Doesn't work. Matches.
Matches. OK.

Ah! This is better.

OK. Try again.

Of course, the matches
are still lighting

because they have their own oxygen
built in here.

That's what's allowing them
to strike,

but there's not enough oxygen
to allow your newspaper

or the match to actually burn.

It's only the match head with
oxygen there. Absolutely correct.

The newspaper could not burn
by itself. Impossible.

Of course, we can breathe fine
in here. It doesn't affect us.

It doesn't affect us at all.
We could live in here for ever.

Very impressive.

We've come outside to try a slightly
larger-scale version of the lighter.

The lighter couldn't start a fire
in the room because it didn't bring

any oxygen with it and there wasn't
enough oxygen in the room itself.

So this should... This is petrol.

I've soaked this torch
here in petrol.

It should light nice and easily.

Yes. Look at that.
So, this is burning rather well.

The question is,
will this go out in the room?

Well, let's find out.

And the fire has instantly gone out.

There really just isn't enough
oxygen in this room to allow this,

my torch here, to carry on burning.

But there is enough for me
to carry on living.

So that's pretty good and I'm happy.

So, this fire prevention system
works by decreasing

the amount of oxygen and increasing
the amount of nitrogen.

Nitrogen is a very important
component of the air

because it's so inert,
because of these very strong bonds.

So we're now going to look
at some of the properties

of this inert gas, nitrogen.

And this is one of the components
in many explosives

such as this nitroglycerin here.

This is a very dangerous explosive.

In fact, Alfred Nobel...

earned his money in trying to work
out how to make this more stable.

I need to put on some special kit
here, some protective clothing

and some ear protectors. OK.

And I'm going to add a drop of
nitroglycerin to the filter paper.

Now then. Adding a drop
of nitroglycerin.

There we are. That's it.

And I think I'll just remove
this nitroglycerin from here.

I don't want to be too close
when this goes off.

So I'll hand this to Mark.
Thank you. Right.

Now, the nitroglycerin contains
a lot of nitrogen locked up

into its chemical composition.

And it's the sudden release of this
that gives it its explosive power.

BANG!

That really was quite violent,

the sudden release
of that nitrogen gas.

And that's what makes
an explosive explosive.

Most of them contain
nitrogen built in.

But remarkably, this reaction, this
explosive release of nitrogen gas,

has been used to save
thousands of lives.

For this, I need a car.

Have you got a car there,
please, Chris?

OK. Well, it's not exactly
a real car.

But it is a real steering wheel. OK.

So, this contains a compound
with nitrogen in it.

It's nitrogen combined with sodium.

Can we have our periodic table
up for a second, please?

So, we have nitrogen over here
combined with sodium over here.

But it's the formation
of our very, very strong

nitrogen-nitrogen bonds that leads
to the rapid inflation

of this air bag.

Now, I need a volunteer
from the audience for this, please.

Er, who shall we have? Yes, would
you like to come down the front?

Thank you very much. Would you
like to stand all the way over here?

And your name is...?
Fred. Fred. OK, Fred.

Now, you are going
to trigger this air bag.

So if I just take this from Chris.
Is this primed?

Just going to make sure
it's all OK to trigger.

OK. Thank you very much.
Now, if you stand over here.

He's very keen to get
a hand on the trigger here.

Now, we're going to count down
from three. OK. If you hold this.

Don't press the button yet. OK.
Now, when we've counted down,

I want you to press the button.

But don't blink.
If you blink, you'll miss this.

It's a very quick reaction. OK.
So, three, two, one.

BANG!
There we are.

OK. Thank you very much indeed.
A round of applause for Fred.

APPLAUSE

So, this air bag works here

because the nitrogen really wants
to bond to itself to form

these nitrogen molecules and it's
this explosive release of nitrogen

that inflates the air bag so
quickly. We can see this here

in slow motion. Actually, when
the crash test dummy hits the bag,

this bag is actually deflating.
The air is coming out of this.

But it needs to be released
so quickly,

that's why an explosive is needed.

So nitrogen here saving lives.

But actually, nitrogen
is vital for life.

We couldn't live without it.

Every protein in every cell in our
body is made up of amino acids.

And every one of these amino acids
contains nitrogen.

So somehow we need to take
the nitrogen from the air

and get it to combine with other
elements so we can form compounds

that are useful to us.

Now, plants have learnt how to do
this over millions of years,

but it took chemists
a long time to do this.

And the first way this was achieved
was by emulating nature...

THUNDER
..a process in nature

where nitrogen and oxygen
are beginning to react.

During this electrical storm,

the lightning here is providing
sufficient energy to split apart

these molecules and this can allow
nitrogen and oxygen to recombine.

We're going to try and do this
in the lecture now. And I have...

Well, this is what every
mad scientist should have.

It's a Jacob's ladder
and here we see it switched on.

So what we're doing here
is passing thousands of volts

between these two electrodes
and this is causing the molecules

in the air to be ripped apart,
ripping their electrons out.

This heats up the air just above it,

making it easier to pass the
electric current through that,

which is why this thing
is gradually rising.

But how will we know if there is any
chemical reaction taking place here?

Well, we're going to keep
an eye on this

and look for signs of a reaction.
We should see a colour change.

Now, I can demonstrate the colour
change that we're going to see.

I have two flasks here.

This contains a compound
called nitric oxide.

This is just air.

But when the two come together...

..we form...

..a new compound that we can see,
that isn't colourless.

There we are. And this is the gas
nitrogen dioxide.

So, this is what we're looking
for in our Jacob's ladder.

So the nitrogen,
if it combines with the oxygen,

we may be able to see this
coloured gas nitrogen dioxide.

We'll keep an eye on the tube
there. It just contains air.

I'll just get rid of that.

But this isn't really
real lightning.

This is only a very small spark
here.

We can maybe begin to see
hints of some colour change,

but we'll keep an eye on it.
We need a bigger spark.

We need something to produce
about a million volts.

And this is what this is for.

This is a Tesla coil

and it can generate
a million volts.

We've had some problems
with this bit of kit.

It basically fries all the cameras,
all the electrics, all the lights.

So this really should give us
some rather impressive lightning.

Now, I must ask everyone just
to remain in your seats

for this demonstration.
Let's see how we go.

BUZZING

Phew.

CHEERING AND APPLAUSE

That really... That really is quite
nerve-racking, I must say.

And what we are seeing here
with all that energy

was causing the nitrogen molecules
and the oxygen molecules

to be ripped apart
and then they recombine

to form nitrogen dioxide
and that's what we can see,

this brown colour here now
in our Jacob's ladder.

And we can also
form molecules of ozone.

That's three oxygen atoms together.
So, what have we learnt here?

We've learnt that the air is more
complicated than we ever thought.

The alchemists thought it was
made up of just one element

but they were wrong. It's made up
of a number of different elements,

of nitrogen, oxygen. We've seen
how important they are to our lives.

Without the oxygen,
we'd all be dead.

But with too much,
we couldn't survive either.

We've also seen how the very rare
gases, the noble gases, can be used

to save lives in hospitals.

Now, the alchemists spent their
lives trying to master the elements.

But they only scratched the surface.

They might have been able
to play with fire,

but they couldn't control it
or understand what it was made of.

Nor could they pick out the elements
from the air and use them

to make the world a better place.

This is where the modern alchemist
takes over.

Join us in the next lecture
where we'll investigate

how a glass of water contains
the remnants

of the most violent reactions
in the world.

Good night. Thank you.

Subtitles by Red Bee Media Ltd