00:01
So as I mentioned to you before, covalent
bonds between atoms of the same type tend
to facilitate electrons being in the center
between the two hydrogens. Or rather, the
probability of that happening—at the highest
95%—is within those two atoms. However,
different electronegativity can polarize a
covalent bond. That is to say electrons can
be moved more to one atom than to the other,
depending upon the electron charge density
of the atoms involved. Large atoms tend to
have low affinity for electrons, and this
is for a number of reasons. The electrons
are a long way from the positive nucleus.
00:48
The core electrons actually shield the outer
electrons from the nuclear charge, allowing
them to be pushed further away. Going across
the periodic table, as you'll see in a moment,
the affinity for bonding electrons increases
from group 1 through to group 7, because the
nuclear charge increases. And as we'll see,
as we go down the periods from period 1, 2,
and 3, as we increase the number of shells,
we are pushing the electrons further and further
away and decreasing the effective nuclear
charge that can be brought to bear in polarizing
a sigma bond. Here we have a representation of
the periodic table. Note the arrows. As we
go across from group 1 to group 7, we're increasing
electronegativity, and we reduce electronegativity
as we go from the lowest period to the highest
period.
01:52
Let's have a look at another sigma bond. This
one, however, involves 2p orbitals. Remember,
as we said before when looking at HF: We need
to have in-phase overlap. That is to say,
we need to have lobes of the right phase interacting
with each other in order for a bonding orbital
to be formed. So, as we discussed before,
we have two atomic orbitals: the 2s and 2p
set, and particularly, I want to look at the
2p set for fluorine. Because what's happening
here, as you can see, when the orbitals are
correctly aligned with the correct geometry,
it's possible for the in-phase overlap of
the two lobes of 2p orbitals from two fluorine
atoms to occur, and the result is the same:
A sigma molecular orbital is formed. Again, I
draw your attention to the fact that the outer-phase
lobes have been reduced in size.