This content explains the concept of ionic bond strength, focusing on lattice energy as a measure of the attractive forces between ions in a solid, and how this strength influences properties like solubility.
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so we were mostly uh concerned with
calent bonding in the previous example
uh and now we are going to be concerned
about ionic bond strengths and remember
ionic bonds is when we have a positive
and negative charge uh together and
those have an attractive forces so our
ionic solids is about this this ionic
kind of interaction the positive and
negative charges that are balancing each
other to cause the compound to become um
to to exist uh particularly in a solid
so the first thing we want to think
about is a lattice energy so our
definition of lattice energy is looking
at the reaction of some sort of ionic
solid and it's going to form its ions in
the gaseous state so it might form some
sort of charge on there and we have to
make sure it's about the gaseous state
and then we form the negative anion so
it's going to be some sort of negative
charge in there as a gaseous thing and
this is our Delta h of our
lattice so our Delta h of the
lattice is also due to this ionic
interaction so there's a lot of these
ionic interactions there's a constant in
here so it's the charge of the positive
ions times the charge of the negative
ions divided by the distance between
those positive and negative
charges and we call that R notot so for
example if we look at something like zinc
zinc
oxide versus something like sodium
chloride so zinc oxide is what we have
in sunscreen and we know when we go
swimming with sunscreen um the sunscreen
doesn't dissolve away so zinc oxide
doesn't dissolve um but why is that but
we if we take salt salt does dissolve
but if we just simply look at the
charges zinc is a plus two charge in
this compound oxygen is a minus
two our sodium is a plus one and the
chloride is a minus one so we have here
um lots of positive and negative charges
in zinc oxide so our Delta h of the
lattice of zinc oxide is going to be
greater than the Delta h of the lattice
of sodium chloride and because this
Delta H is actually very large it
doesn't dissolve so it's harder to break
up those ionic interactions when there's
this huge enthalpy of of lattice Energies
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