00:01
All right, in this question, we're going to talk about a few properties of ionic compounds.
00:05
So, first up, we have conductivity.
00:09
Ionic compounds, they're very conductive, but they're dissolved in water, but not so much when they're in solid form.
00:15
Now, let's talk about why.
00:17
When they're dissolved in water, remember, ionic compounds have a cation and an ion, and when they're dissolved in water, these cations and aniones are separated.
00:30
So we have positive and negative charges floating around.
00:37
That allows electrons to find a route through a solution of cations and anions.
00:45
When they're tightly bound in a crystal structure, they don't have that luxury because there are too many repulsion forces.
00:57
So if we think about what, let's use sodium chloride looks like, we have.
01:03
Sodium, we've got chlorine, we've got alternating sodium and chlorine atoms in a huge clump.
01:19
So as soon as the electron, it may be attracted to a sodium, as soon as the electron gets to one part, it's going to be met with repulsion forces from all the chlorines around it.
01:32
It would be very difficult for it to move through.
01:35
And in a solution, that's not a problem because the cat ions and anions are spread apart.
01:46
So electrons can come in and avoid, well, or squeeze by these negatively charged anions.
01:56
Right? next up we're talking about melting points.
01:59
So that's kind of a similar story where we have, if we look at the structure, it forms a okay, i'll draw it this way, actually.
02:11
Sorry.
02:14
So i have a compound, say, form a crystal lattice structure.
02:26
Pick one where, well, let's do, chlorine is red and sodium is black...