[Kryolith]

Correct.

I don't know a website, but you know the charges of the cations/anions so I am pretty sure you could create your own quiz 

[JonathanEyoon]

Ok I found a place where I can do a ton of these nomenclatures and I got stumped on one


It is Hg2F2 = I put down Mercury(II)Flouride but it's wrong.

The correct answer is Mercury(I)Flouride. 

[Kryolith]

Fluor has always the oxidation number -I (exception: F₂). So Hg must also have -I, because the molcule is neutral.

[JonathanEyoon]

Hg2F2 is not in it's empirical form right?  Can it be put in an empirical form? Well if I did it would be HgF?

[Borek]

Note - in chemistry almost every rule has some exceptions. This is one of those cases when things doesn't look as they should at first sight. If it is Hg(I) formula of fluoride should be HgF. It is not and for a good reason, there are ways (you will learn them later) of experimentally checking that the cation present in the solution is Hg₂²⁺. Once again (like with valences of transition metals), it is not a thing that you may deduce, it is a thing you have to remember.

You are right about empirical formula being HgF. Real thing is Hg₂F₂.

[Kryolith]

The empircal formula would be HgF. But it exists as a ion. Compare X₂ (X=halogen), P₄O₁₀, Na₂O₂ etc.

[JonathanEyoon]

Ok I just found this and am having a hard time understanding it

Example #1: mercury(I) chloride
The formula for this compound is Hg2Cl2. It is not HgCl. You will be marked wrong on a test for doing so.

Example #2: mercury(I) nitrate
The formula for this compound is Hg2(NO3)2. Once again, it is not reduced. Why? In nature, mercury(I) comes in a set of two atoms, NOT just one.
The corresponding mercury(II) formula for the two examples would be HgCl2 and Hg(NO3)2.

So Mercury exists as a diatomic naturally?  If it does, are there any more other than the 7 that I know of? Have No Fear Of Ice Cold Beer =)

[Borek]

So Mercury exists as a diatomic naturally?

No. Hg(I) exists as diatomic cation. So you have Hg - neutral metal, Hg₂²⁺ - diatomic cation of Hg(I), and Hg²⁺ - 'normal' cation of Hg(II).

[Kryolith]

Here is a tricky one:

What's the (empirical) formula of iron(II,III) oxide?

[JonathanEyoon]

Iron(II,III)oxide?

Sorry I was preoccupied earlier.  Let's see if i've been a good student to you guys.  Uhmmm...


Iron(II)oxide = So the Iron has 2 cations and Oxygen has 2 anions.  So would it be FeO?

Iron(III)oxide = Fe2O3?

Ok I have more questions  Hopefully you guys aren't fed up with me yet.
Can someone help me with Acid Nomenclatures?  I'm not exactly certain of the rules.  I've been trying to memorize as many polyatomics, common cations, and common anions as possible as to help me with Acid Nomenclatures 

[LQ43]

for binary acids  HX - use "hydro" as a prefix and "ic" at the end

hydro_____ ic   acid   e.g. HCl (aq) hydrochloric acid
                              e.g. H2S (aq) hydrosulfuric acid

compound should have (aq) to use acid name


For oxo (or ternary) acids  HXO

"ate" ions give "ic" acids 
e.g sulfate --> sulfuric acid
but not perfect e.g. phosphate --> phosphoric acid


"ite" ions give "ous" acids
e.g nitrite --> nitrous
again not perfect e.g. phosphite --> phosphorous acid

[Borek]

Iron(II)oxide = So the Iron has 2 cations and Oxygen has 2 anions.  So would it be FeO?

Iron(III)oxide = Fe2O3?

These are correct, but Kryolith asked about mixed oxide, that contains both Fe(II) and Fe(III) in a molecule

But this question - as posted - has no answer.