00:00
As time has gone by within
the last 100 to 150 years
the scientific knowledge
of mankind has increased
and matter has been found to be made
up of smaller fundamental particles.
00:13
In particular,
if we look at subatomic particles
which you may be
familiar with such as
protons, neutrons and electrons,
they themselves are actually
made up of even smaller
particles falling into the
quark and lepton class.
00:32
But as we will see when we
are discussing chemistry,
we are principally
looking at the movements
and the interactions
of electrons.
00:41
Anything which indeed goes
beneath that in terms of size,
typically speaking we leave
in the realms of physics.
00:49
Chemistry is about the
movement of electrons.
00:52
Nuclear physics is about how nuclear
particles interact with each other.
00:57
And therefore knowledge
of the latest developments
in this discovery of these
fundamental particles
isn’t necessarily essential
for an appreciation of
how electrons move around
and how ionic
covalent molecules and
formerly units can be
formed respectively.
01:17
As indicated in
the previous slide,
there are certain small fundamental
particles such as leptons and quarks
which are really unnecessary at this
level for understanding about chemistry.
01:29
Chemistry in its very heart,
as I mentioned before,
is about electrons and not
necessarily about the nucleus.
01:37
If you look at the board, you’ll be
able to see three fundamental particles
that you are expected
to be familiar with.
01:44
They are the proton,
the neutron
and the electron.
01:50
The proton and the neutron are both
nucleons, that is to say they are
subatomic particles which
reside within the
nucleus of an atom.
02:00
Protons have a charge of +1,
neutrons have a charge of 0.
02:06
And they both have a
mass of 1 atomic unit.
02:11
1 atomic unit, as you can see
at the bottom of the board,
is given as 1.67 × 10^-24 grams.
02:20
And what is worthy of note, if you
look at the table, is the third entry:
the electron.
02:26
Electrons have a charge of -1 but they
have a substantially smaller mass.
02:32
The mass of an electron is
given relative to an AMU
of 5.48 × 10^-4.
02:41
However,
the reality of this in kilograms
is that an electron has a mass
of 9.11 × 10^-31 kilograms.
02:50
So very much smaller
than those nucleons.
02:54
Most of the atom is
actually empty space
with the protons and the neutrons
clustered together in the centre.
03:02
And this is something that was actually
detected experimentally by Thomson
and Rutherford.
03:10
The electrons seemingly form a
cloud around the central nucleus.
03:16
And it is these electrons
which engage with each other
to form matter as we
currently understand it,
whether it’s ionic
or whether it is
indeed covalent.
03:30
And what we’re going
to be going through
is how these individual arrangements
of electrons, protons and neutrons
come to form the elements that
we see within the periodic table,
a very important index
for the elements that
we find on this planet.
03:49
The analogy which is often used
for the structure of an atom
is that the nucleus
is the ball on the centre
spot of a football field
with the electrons actually
being the tiny specks of dust
blowing around the stands.
04:09
Since within an atom there are equal
numbers of protons and electrons,
the overall charge of an atom
as its element
is 0.
04:20
It has to be 0
because the number of
protons with a charge of +1
equals the number of electrons
with a charge of -1.
04:30
So only certain combinations
of fundamental particles
can form stable atoms.
04:37
And this goes back to what I
was saying about the nucleus.
04:40
Was this is not necessarily essential
for us to understand it in the context of
compound formation,
it is important to be aware of
the existence of things called
isotopes.
04:51
You have probably heard of
the term ‘radioactive’ isotope
and this, for example,
would be where you have an
unstable configuration of protons
and neutrons within the nucleus
that are liable to
undergo a disintegration
involving the loss of more of one
of these fundamental particles.
05:10
And it is the nucleus
that decays in this case.
05:13
It is also the origin,
as we will see, of isotopes.
05:18
These are elements which have
the same chemical characteristics
but a different number of
neutrons within the nucleus.
05:28
And radioactive decay,
to give you an example,
would be not too dissimilar
to that which you observe in
the decay of uranium to thorium.
05:36
Or used in the fission
process – in nuclear fission
– the breakdown of uranium-235
to barium and krypton.
05:46
And this process would be
known as a nuclear reaction
and the previous to one I just
mentioned is radioactive decay.
05:54
So let’s get back to where we were
originally: talking about the atoms
and talking about the elements
that we see in the periodic table.
06:02
There is some nomenclature that
you should also be familiar with.
06:05
And that is shown here on the board:
Z, N and A.
06:12
Z correlates to the atomic
number or element number
and this relates to the number
of protons in the nucleus
and defines which element within the
periodic table the atom actually is.
06:26
N is the number of
neutrons which is,
obviously as you would
expect, the neutron number.
06:34
And finally A,
which is the combination of
neutron number, N,
and atomic number, Z.
06:43
So this gives you
the mass number.
06:46
Since, as we’ve indicated earlier, electrons
have a very, very, very small mass
they are largely ignored from
the overall mass of an atom.
06:55
Instead, we tend to look at the
combination of protons and neutrons
when considering
the atomic mass.
07:05
So here we have an
example of an atom.
07:08
To properly identify
it, it is written thus.
07:11
Note we have the chemical symbol
for this particular element – Cl.
07:18
This correlates to chlorine.
07:20
As you will see if you
interrogate the periodic table,
you will often see elements which,
ostensibly, don’t make any sense in English
or indeed in any other
European language
because they are actually derived
from the Latin or the Greek.
07:37
So, for example,
Cl – chlorine, chlóros
– comes from the
Greek, meaning green.
07:46
And, as we will see
a little later on,
there are a number of other
elements which also don’t make sense
in the context of
their English name
or their standard IUPAC names.
07:57
So anyway, as I was saying,
if you look here we have an
example of the element chlorine.
08:02
Note the larger number
at the top is A.
08:05
This is the atomic mass number.
08:09
The lower number is Z,
which is the atomic number.
08:13
And whenever you’re looking at this
if you’re getting confused as to what
is an atomic number and what
is an atomic mass number,
the atomic mass number is always
larger than the atomic number.
08:23
So, if you can’t remember whether
it’s top or bottom, don’t worry.
08:27
Just find the largest
number: that is the mass,
which correlates to the number of
protons and also the number of neutrons.
08:35
Z is the atomic number, which correlates
to the number of protons, as we indicated
but also just as important
in elemental form
must therefore correlate
to the number of electrons
in the shells of that atom in
order for it to have a charge of 0.
08:51
Now I’ve shown chlorine
here for a good reason
because it is one of those elements
which exists as two stable isotopes
within the periodic table.
09:01
This is isotopes where you have
the same chemical activity,
because you have the
same number of protons
and therefore electrons in an atom,
but a different number of neutrons.
09:14
And, as you can see here,
we have – or I’m
showing you here
– three different isotopes,
of which one is actually unstable.
09:22
They are 35Cl
and 37CL and 36Cl,
which is the
unstable radioisotope
with a half-life
of 308,000 years
and is negligible in concentration
within the environment.
09:39
The ones which are stable
are 35 and 37.
09:45
As you will see sometimes
with periodic tables,
the Z is often omitted because the
this chemical symbol
of a particular element
automatically defined
in the periodic table
further defines the number of protons
and electrons it must possess.
10:02
If we look at 35Cl as a stable
isotope, it is found in 75% of
all chlorine in the environment.
10:12
37Cl, on the other hand,
is found in 25% of chlorine
in the environment.
10:20
And so therefore,
when we are calculating the
relative overall atomic mass,
we need to take into consideration the natural
occurrence of both of those isotopes.
10:33
And we’ll come onto an equation that
deals with this a little later on.