All Questions
Tagged with ionic-compounds transition-metals
17
questions
5
votes
3
answers
279
views
Does chromium chromate — Cr₂(CrO₄)₃ — exist?
Is it possible to synthesise chromium(III) chromate/dichromate? The intended formulas are $\ce{Cr2(CrO4)3}$ and $\ce{Cr2(Cr2O7)3}$ and they feature both trivalent and hexavalent chromium. However, ...
user144956
3
votes
1
answer
332
views
Can I convert copper(II) acetate or carbonate to copper(II) sulfate?
I am a high school student who does chemistry as a hobby, and as such I really don't know very much. I managed to make some copper(II) acetate and copper(II) carbonate, and now I'd like to convert it ...
1
vote
0
answers
1k
views
How many multivalent elements are there? [closed]
According to this video there are 20 multivalent elements, and from the periodic table, I see 20, but according to multiple websites, including this, it says there are only 5. What am I not ...
- 1
0
votes
1
answer
2k
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How do we know the ionic charge of iron or elements such as iron on the periodic table?
How do we find iron's ionic charge? I was taught that we use roman numerals but I don't see any on the basic periodic table of elements (I'm using this one). So how do we find iron's charge of Fe 2+ ...
- 1
-1
votes
2
answers
136
views
Displacement Reaction [closed]
In a displacement reaction I understand that the more reactive metal essentially takes the place of the less reactive metal. But I can't seem to understand how this more reactive metal can break the ...
7
votes
1
answer
3k
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Why is it advised to use neutral ferric chloride solution while performing confirmatory test for acetate ions? [duplicate]
The reaction of $\ce{FeCl3}$ with $\ce{CH3COO-}$ is
$$\ce{3Fe^{+3} +6CH3COO- +H2O<=> [Fe3(OH)2(CH3COO)6]^{+} +2H^{+}}$$
Recently I read that a solution of $\ce{FeCl3}$ hydrolyses very quickly to ...
- 183
0
votes
1
answer
437
views
Does mercury chloride (ii) evaporate at room temperature? [closed]
if you leave mercury chloride (ii) exposed to air in a room does it evaporate to any significant level which can cause toxicity?
- 21
2
votes
1
answer
211
views
Manganates (II)
I want to ask about character of manganese(II) compounds. I read that $\ce{MnO}$ is basic, just like $\ce{Mn(OH)2}$. I started doing research and I read ions like $\ce{MnO2^{2-}}$ and $\ce{HMnO2^-}$ ...
- 89
6
votes
3
answers
6k
views
Is iron(III) carbonate stable in water?
I searched for this onsite already, and also found the following answer on Quora:
In aqueous environment, iron(III) is bound by water molecules and exists as $\ce{[Fe(H2O)6]^3+}$. Due to strong ...
- 1,201
5
votes
4
answers
9k
views
Why is MnO2 not a peroxide?
As I know, $\ce{MnO2}$ is called manganese(IV) oxide.
Why can't we name it manganese peroxide since manganese(II) exists too?
In other words, how do we know that the oxidation number of manganese in ...
- 365
1
vote
1
answer
535
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How to make γ-MnO2 in a lab?
I am working on Li-ion batteries, and I need to use γ-$\ce{MnO2}$ (electrolytic manganese dioxide). I have googled and read quite a few papers, but I am not very sure of those methods. I'd love ...
- 113
-1
votes
1
answer
866
views
Why Does Coordination of Metal Ions Happen Anyways?
I've been studying coordination chemistry, but I still have a fundamental question about the area: why do transition metals even form coordination compounds, while main group metals do not? Why can't ...
- 1,610
7
votes
1
answer
4k
views
Color of Anhydrous Transition Metal Salt
Why are some anhydrous transition metal salts colored?
Here are some examples I found.
Anhydrous cobalt(II) chloride ($\ce{CoCl2}$), with sky-blue color.
Anhydrous chromium(III) chloride ($\ce{CrCl3}...
- 544
10
votes
1
answer
7k
views
Why aren't the copper(II) ions in CuSO4 precipitated by hydroxide ions from water?
From my own experience and literature, I know that $\ce{CuSO4}$ is well soluble in water and dissociates into $\ce{Cu^2+}$ and $\ce{SO4^2-}$. $\ce{Cu(OH)2}$, however, is not: $K_\mathrm{sp} = 2 \cdot ...
- 101
3
votes
2
answers
10k
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Why are transition metal hydroxides insoluble?
From what I understand, adding $\ce{NaOH}$ to a solution containing transition metal ions gives transition metal hydroxide precipitates. Why is $\ce{NaOH}$ soluble but transition metal hydroxides ...
- 1,697