00:01
Okay, so let's talk about quantum numbers
in a little bit more detail. We introduced
the concept in the last lecture, where we
talked about their importance in understanding
where electrons were. But when we are building
up electrons within the periodic table, and
we are moving from left to right, and we are
adding electrons, as we increase the groups,
we go up the group from sodium on one side
to the noble gases on the other, what we need
to do is understand more about where the electrons
are for each individual atom.
00:34
So I introduced the idea of the principle
quantum number, which has the letter n associated
with it; the orbital quantum number, l; and
also the magnetic quantum number, m. Okay?
So what we are going to be doing now is to
better understand how electrons are filling
these orbitals as we go across the periodic
table and also as we go down the periodic
table.
So we have a picture of where electrons need
to go: obviously, nowhere near the nucleus;
that's the preserve of the neutron and the
proton. And we know how many electrons there
should be in any atom of any element. But
we now need to understand some way of telling
us where the electrons will go. And there
are three rules that we are using in this
case to understand how this happens: the Pauli
exclusion principle, the Aufbau principle,
and also Hund's rule. And each of these will
enable you to predict the electron configuration
of any atom or ion.
01:42
The Pauli exclusion principle states that
in any atom, no two electrons may have a set
of quantum numbers with the same values. But
there is a problem. In a 1s orbital, there
can be two electrons, so both will have the
same quantum numbers, surely, which is n,
principle quantum number 1; l, because it
is an s orbital; and, of course, ml, because
it is spherical, and therefore, it is not
possible to have more than one orientation.
02:14
And that is where we consider the magnetic
spin quantum number, or ms. If we imagine
an electron, for a second, as a particle,
it can rotate on its axis, and this is shown
by the diagram on the board. As you can see,
you have positive spin configuration and negative
spin configuration. This is where the electrons
are either rotating in a clockwise or an anticlockwise
direction. Electrons with the same spin direction
are said to have parallel spins, whereas those
with different spin directions are said to
have antiparallel spins.
03:03
So if we go back to what we said before, we
look at a simple 1s orbital, we can see, by
the incorporation of this additional quantum
value (the ms quantum value) that the first
rule is preserved. That is to say, we actually
have two different overall quantum configurations
for the electrons in this s orbital where,
as you can see at the bottom of the board,
we can denote these by two arrows: one heading
up and one heading down. This is known as
the pairing of electrons, and they are often
represented in a box form, as you can see
on the board as well, where the line running
from left to right or right to left represents
the orbital concerned (in this case, the 1s
orbital) and the direction of the electron
spin is shown by the arrows, pointing either
up or down.