Jan 7, 2017 · I find that $\ce{AlF3}$ is okayish soluble in water, see Wikipedia, so I am curious under what conditions it is insoluble in HF, because if we talk about an aqueous solution, then I doubt that this is true. Otherwise the question is more or less why $\ce{AlF3}$ is so much more soluble in the presence of $\ce{KF}$. $\endgroup$

Jan 16, 2021 · As $\ce{AlF3}$ is a Lewis acid, I expect it to have higher solubility in solvents which have lone pair containing donor ; possibly the fluoride ion from $\ce{KF}$ may be such a species Further, in aqueous acidic solution, I expect a lower solubilty owing to common ion effect lowering the solubility

Dec 28, 2019 · However, the melting point of $\ce{AlF3}$ $(\pu{1291 °C})$ is larger than that of $\ce{AlCl3}$ $(\pu{192.4 °C}).$ I think the huge melting point difference is because $\ce{AlCl3}$ is more covalent, while $\ce{AlF3}$ is more ionic. That being said, does lattice energy account for the covalent and ionic character of compounds? References

Apr 10, 2019 · Smaller cations can better hold small anions like fluoride. The larger the lattice enthalpy factor, the tougher thermal decomposition becomes. As atomic size decreases across a period, the order of stability is AlF3 > MgF2> NaF.

Mar 20, 2020 · Which compound has largest amount of lattice energy among $\ce{AlF3}$ and $\ce{AlN}$. I think it should be $\ce{AlF3}$ because lattice energy in inversely proportional to radius and size of flourine is quite small as compared to nitrogen.

Nov 25, 2018 · 1.Between $\ce{AlF3}$ and $\ce{MgO}$ (In $\ce{AlF3}$ product of ionic charge is $3\times1$ and in MgO it is $2\times 2$. So,according to me $\ce{MgO}$ should have higher lattice energy but the opposite is true.

Jun 21, 2020 · According to Ref.1: The order of Lewis acidity of gaseous halides of aluminum is established to be $\ce{AlF3(g) < AlCl3(g) < AlBr3(g) \approx AlI3(g)}$. The order of Lewis acidity of molecular and solid group 13 halides is $\ce{AlX3(g) > GaX3(g) > …

Jan 8, 2017 · Ahh, Thallium is a very nice element. Because it's weird.. The +3 oxidation states are favorable except for the heavier elements, such as Tl, which prefer the +1 oxidation state due to its stability; this is known as the inert pair effect.

Jan 11, 2023 · $$\ce{AlF3 + NaF \to Na3[AlF6]}$$ My question is why don't we get $\ce{Na[AlF4]}$, since when we do the same thing with hydroxides instead of fluorides ($\ce{Al(OH)3}$), we end up with $\ce{Na[Al(OH)4]}$. I know that it is a 3rd period element so it can expand its octet, so boron being in the same group forms $\ce{NaBF4}$. I've also heard …

Jan 24, 2018 · Actually, there are three reasons why BF3 is more acidic than AlCl3. BF3 is smaller in size and can easily attract the incoming pair of electrons.