All Questions
Tagged with inorganic-chemistry halides
105
questions
-1
votes
3
answers
123
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If LiF is ionic in nature, why can't it dissolve in water?
LiF is prominently ionic compound. I also know polar substances can be dissolved in water as "like dissolves like". Why is then LiF only weakly soluble, in comparison with LiCl, or LiBr, ...
- 37
4
votes
0
answers
100
views
With two reagents common on Mars, fluorite and CO2, how would I produce carbon tetrafluoride?
The hypothetical terraforming of Mars would require the heating of the atmosphere. A commonly suggested method is the in-situ production of fluorocarbons, powerful greenhouse gases.
For example, ...
- 141
5
votes
1
answer
400
views
Thermal instability of sulfur and selenium iodides
After recent question about non-existent pnictide(V) iodides, I stumbled upon a similar issue in oxygen group. For example, $\ce{SI2}$ was reported to be found… but at the temperature as low as $\pu{9 ...
- 4,606
9
votes
2
answers
2k
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Why does potassium bifluoride exist whereas bichloride does not?
Why does the reaction \eqref{rxn:R1Q} take place, but the reaction \eqref{rxn:R2Q} does not?
$$
\begin{align}
\ce{HF(aq) + KF(aq) &-> KHF2(aq)}\label{rxn:R1Q}\tag{R1} \\
\ce{HCl(aq) + KCl(aq) &...
- 101
2
votes
1
answer
775
views
Why is Hg2Cl2 less soluble in water than HgCl2?
I learned that $\ce{Hg2Cl2}$ is almost insoluble to hot water and $\ce{NH3}$ water in my textbook, but $\ce{HgCl2}$ dissolves well in water.
I wanted to know the reason and searched for it. It's ...
- 677
-1
votes
1
answer
457
views
Which Group 16 elements form stable dihalides?
My textbook says that "except oxygen, all elements of group 16 form dichlorides and dibromides", while other sources quote that only Oxygen and Sulphur form dihalides and dibromides.
Whereas,...
- 1
9
votes
1
answer
1k
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How does xenon react with O₂F₂?
This reaction was asked in my college entrance exam. I searched through the entire Internet, but I couldn't find any papers/sources.
I suspect since O₂F₂ is a strong fluorinating agent, one of the ...
- 141
5
votes
1
answer
261
views
Has tellurium(II) iodide been properly characterized ever?
According to Wikipedia, tellurium tetraiodide decomposes on heating:
$$\ce{TeI4 ->[\Delta] TeI2 + I2}$$
However, the reaction is somewhat wrong as according to this 2008 paper:
Solid tellurium ...
- 26.3k
2
votes
1
answer
96
views
Can nitric oxide (NO) reduce xenon fluorides
I came across the following question:
$\ce{XeF4}$ on reaction with gaseous nitric oxide forms xenon gas and (P). Find the total number of lone pairs present in one molecule of P.
As far as xenon ...
2
votes
1
answer
224
views
Why is it technically inaccurate to say that the decrease in reactivity of halogens is due to decreasing electronegativity?
I came across the following information in this post.
Below the infographic there is a paragraph with a disclaimer:
As another disclaimer, the reactivity of the halogens decreasing down the group ...
- 305
2
votes
1
answer
1k
views
Can aqua regia/royal water dissolve lead? [duplicate]
As known aqua regia can't dissolve $\ce{Ag}$ because formation of $\ce{AgCl}$ precipitate. Similarly will aqua regia precipitate $\ce{Pb}$ as $\ce{PbCl2}$? OR It is not possible to observe this ...
- 802
1
vote
0
answers
594
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How are 3 center-4 electron bonds any different from 2 center-2 electron bonds? [closed]
How are the bridge bonds in $\ce{Al2Cl6}$ different from the terminal bonds?
We could have just mentioned the bridge bond formed by $\ce{Cl}$ as a coordinate bond. Why introduce this extra concept?
I ...
- 454
2
votes
0
answers
371
views
Does Copper(I) Iodide have a dimer?
A qualitative test for the iodide ion involves reacting the salt solution with copper sulphate. This is said to yield the triiodide ion and the white precipitate of $\ce{Cu2I2}$.
I haven't been able ...
- 1,134
0
votes
0
answers
77
views
Solubility of Beryllium Compounds in Water [duplicate]
Why is $\ce{BeF2}$ is highly soluble in water but $\ce{Be(OH)2}$ is insoluble?
Both release $\ce{Be^{2+}}$ ion so this means they both have high hydration enthalpies and can easily overcome their ...
- 93
5
votes
1
answer
597
views
What qualifies to be considered as a lone pair-lone pair repulsion?
Referring to, NCERT Chemistry Part I, Textbook for Class XI[1].
Here the text puts forward three structures of $\ce{ClF3}$.
My teacher said to me that (b) structure is unstable due to lone pair lone ...
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