If we take a look here, we can actually classify different types of compounds as either being
strong electrolytes, weak electrolytes or non-electrolytes.
Let's look at the strong electrolytes.
Our strong electrolytes belong into three categories.
First things first, we have our strong acids.
Strong acids are considered strong electrolytes.
So they break up completely when they're dissolved in water.
Examples here, we have HCl, we have a blank and then we have HI.
Now if you take a look at your periodic table, you'll notice that chlorine and iodine are
both in the same group number.
Both of them are in Group 7A.
Take a look at your periodic table, what element is in between chlorine and iodine?
It will be Br, so HBr is considered a strong acid as well.
HF is not considered a strong acid.
It's actually considered a weak acid.
It's because it possess hydrogen bonding.
You'll learn about that later on.
But just realize because of the hydrogen bonding it has present in it, HF is a considered a
weak acid.
So HCl, HBr, HI so far, HNO3 is another strong acid, then the last three will be H2SO4, HClO4,
and HClO3.
Those are considered your seven major types of strong acids.
Now the second type of strong electrolyte we can have our strong bases.
Now, we're going to say strong bases fit into two major types of categories up to this point.
Later on, when we learn more in depth analysis on acids and bases, we're going to open up
two more and more different types of acids and bases.
For this point right now, this is all you really need to know when it comes to electrolytes.
For strong bases, Group 1A metals when they're combined with OH-, H-, O2- or NH2-, they will
be strong bases and they'll be considered strong electrolytes.
Remember what's the charge of Group 1A ions?
They're all +1.
So we combine each of these with one of these ions.
Na+ OH-, their charges just cancel out and you get NaOH.
Here the charges just cancel out, you get CsH.
The two from here is going to move down here.
The one from here is going to move over here, so this would be K2O.
Then, finally, you'd have LiNH2.
So all of these are good examples of strong bases.
Now, any one of these four ions could combine with any one of the Group 1A metals to create
a strong base.
Now, the next one we have Group 2A metals.
Here we're going to say Ca or lower when they're combined with these same four ions creates
strong bases.
But what do I exactly mean by calcium or lower?
Group 2A on our periodic table has beryllium, magnesium and then, calcium you have, strontium
and barium.
I'm saying calcium and lower, so calcium, strontium, and barium, when they're with one
of these guys they create a strong base.
All of them are in Group 2A, so they're all +2.
If we combine some of them with some of these ions --
just remember the two from here will move down here, the two from here will move over
here, the two from here will move over here.
So, we get CaOH2, SrH2, Ba(NH2) 2.
These are all common examples of strong bases from Group 2A.
Finally, we're going to say soluble ionic compounds are considered strong electrolytes.
What do I mean in this section?
Here, this is basically ionic compounds that follow the solubility rules.
For example, we're going to say that Na is a Group 1A metal.
Group 1A ions are soluble with whoever they're with.
So I could have Na with NO3.
This will break up into Na+ plus NO3-, breaks up fully into its ions, so it's a strong electrolyte.
We could also have LiCl.
Group 1A metal, Cl is soluble with everyone also except for certain metals.
So, our three categories for strong electrolytes are strong acids, strong bases and those that
follow the rules for being soluble when we look at the solubility rules.