00:01
To name all of these compounds, you must have memorized the naming rules, all of them, for ionic compounds and for non -ionic binary covalent compounds.
00:13
Otherwise, you're not going to be able to understand the chemical formulas from the names and vice versa.
00:19
In addition, you must have all your polyatomic ions memorized with their charges, or it won't make sense either.
00:27
So the first one is sulfur, diphloride.
00:31
Sulfur has a 2 -minus charge because it is in group 7a.
00:38
And, yeah, you also need to know your charges of the representative elements based upon their group number.
00:44
And fluoride has a 1 -minus charge.
00:47
So to get a neutral compound, well, actually, hold on a second.
00:50
This is not an ionic compound.
00:53
So forget the whole charge thing i just said.
00:55
This is a binary covalent compound, so the number of atoms corresponds to the prefix.
01:02
So we have sulfur dye fluoride, so we have one sulfur, dye means two, two fluorides.
01:08
Sulfur hexafluoride, one sulfur, hexa means six, six fluorides.
01:14
Next we have sodium dihydrogen phosphate.
01:16
Dihydrogen phosphate needs to be a polyatomic ion that you have memorized.
01:20
That is h2, p .o .4, one minus.
01:22
Sodium has a one plus charge, so we just need one.
01:25
Sodium and one dihydrogen phosphate.
01:29
Next we have lithium nitride.
01:31
Lithium has a plus one charge, nitride.
01:34
It has a three minus charge based upon its position in the periodic table.
01:38
So we're going to need three lithiums for every nitride.
01:42
Then we have chromium three carbonate.
01:45
Carbonate's a polyatomic ion, that's co3, two minus.
01:49
So if it has a two minus charge and chromium has a three plus charge, then you get a neutral compound we're going to need two chromium's and three...