Questions tagged [ionic-compounds]
Compounds in which at least some of bonds have ionic character stronger than covalent or metallic. Many compounds called salts are ionic compounds but not all of them.
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Is KF the most ionic compound?
I saw somewhere (can't recall where) that KF is the most ionic compound. I expected CsF. Does the greater polarizability of Cs allow it to more easily form covalent bonds compared to K? Does this ...
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What is Sodium Chloride like in gas state?
Since sodium chloride is sodium and chlorine atoms bonded as a lattice and there are no discrete molecules, doesn't that mean in gas state, sodium chloride is simply sodium and chlorine atoms separate ...
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Will gaseous ionic compounds be free moving ions?
I knew while learning about electrolysis that if the ionic compound is molten it becomes free moving ions.
If that is the case, what will happen if I continued heating till it reaches the boiling ...
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Can 100% covalent bonds exist?
Every covalent bond has some ionic character and every ionic bond some covalent character. I can understand why a completely ionic bond is an ideal situation. But completely covalent bonds can exist(?)...
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Does boron form compounds without covalent bonds?
I have read that boron, due to the very high sum of its first three ionization energies, it is not able to form its +3 ions, and thus it generally forms only covalent compounds. But in a popular ...
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Why do different elements form different types of carbides?
What property of the elements make them form different types of carbides like:
$\ce{Be}$ and $\ce{Al}$ - $\ce{Be2C}$ and $\ce{Al4C3}$ (Methanides) contains $\ce{C^4-}$ ion
$\ce{Na}$ and $\ce{Ca}$ - $...
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Can a organic compounds such as hydrocarbons contain an ionic bond?
Can organic compounds like hydrocarbons have types of bonds other than covalent bonds? Can they also possess ionic bonds?
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Is potassium bifluoride an ionic or a covalent compound?
The statement below is an excerpt from my textbook (Chemistry Part II, Textbook for Class XII by NCERT, ed. January 2014):
Because of the tendency of fluorine to form hydrogen bond, metal fluorides ...
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Are metallic/ionic bonds weaker than covalent bonds?
In mineralogy class, I was taught that metallic and ionic bonds are weaker than covalent bonds and that's why quartz and diamond have such a high hardness value. However, in organic chemistry class, I ...
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Why is CaCl2 called calcium chloride?
Doing a first year chem class.
Just read through the molecular naming of compounds and now I'm confused as to why $\ce{CaCl2}$ is called calcium chloride and not calcium dichloride?
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What is the meaning of "superionic"?
I see the term "superionic" applied to high pressure water in articles like Giant planets may host superionic water, but I don't understand what the term really means.
How is "superionic" ...
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Are all NO3- salts soluble in water? If so, why?
All the examples of $\ce{NO3-}$ salts are soluble in water (all that I know about).
Is it always so or there is some salt which doesn't dissolve in water?
If so what is the reason behind it?
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Reaction between zinc and sulfur
Would the reaction between zinc and sulfur be
$$\ce{Zn_{(s)} + S_{(s)} -> ZnS_{(s)}}$$
or
$$\ce{8 Zn_{(s)} + S_8\ _{(s)} -> 8ZnS_{(s)}}$$
I know that $\ce{S}$ and $\ce{S8}$ are allotropes of ...
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The impossibility of 100% ionic bond
Recently, I read the definition of oxidation state on Wikipedia. It read that a 100% ionic bond is impossible. So what does a 75% ionic and 25% covalent bond mean at all?
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Is an ionic bond more like a covalent bond or an intermolecular force?
I have asked a question loosely asking this, where I confused terms and did not specify what I wanted to know here, so I formed a new question.
What are the differences and similarities between ionic ...
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MgCl2 acidic or neutral in water?
I'm currently taking chemistry 12. On our test we were asked, when given a $0.1~\mathrm{M}$ solution of certain compounds whether the resulting solution when added to water would be acidic, basic, or ...
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What determines whether a double displacement reaction will occur?
In normal displacement reactions, reactivity plays a large role and sometimes the reaction doesn't even happen. So is there anything limiting double displacement reactions? For example $\ce{2KI + Pb(...
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Why do Magnesium and Lithium form *covalent* organometallic compounds?
Lithium and magnesium are Group 1 and Group 2 elements respectively. Elements of these groups are highly ionic, and I've never heard of them forming significantly covalent inorganic compounds.
Yet ...
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Is pyrite (FeS₂) an ionic or a covalent compound?
I have searched all over the web and found a lot of diverse explanations, but none of them are concluding exactly whether $\ce{FeS2}$ (solid - pyrite) is a covalent or an ionic compound.
From ...
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What happens when potassium iodide is added to a copper (II) salt?
$$\ce{Cu^2+ + KI -> ??}$$
I thought of this reaction:
$$\ce{Cu^2+ + 2KI -> CuI2 + 2K+}$$
But since $\ce{CuI2}$ doesn't exist, the $\ce{I-}$ ions must reduce $\ce{Cu^2+}$ to $\ce{CuI}$ and ...
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Is melting/boiling point of ionically bonded substance higher than of covalently bound?
Is the melting and boiling point of ionic bond usually higher than covalent bond?
I know that compounds with ionic bonds are usually solid at room temperature, so I want other answers than this. (...
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What is the structural formula of alkali hypohalite: MOX or MXO?
There seems to be an inconsistency in the formula. Somewhere it is written as MOX and in some places, it is written as MXO. This is what Google gives when you search sodium hypochlorite:
I think the ...
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Are all ionic compounds salts?
According to Wikipedia:
A salt is an ionic compound that can be formed by the neutralization
reaction of an acid and a base.
Are all ionic compounds salts? Are all salts ionic compounds?
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Has a carbon compound ever been found having an ionic bond?
Though it is highly unlikely, has any carbon compound been found to make an ionic bond and to exhibit ionic properties?
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Why isn't water an ionic compound?
If two alkali metal atoms join with an oxygen atom, an ionic bond forms. Since hydrogen has the same number of valence electrons as alkali metals, why can't water be ionic?
This is what I'm thinking:
$...
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Naming ionic compounds with multiple cations and anions
I have seen complex ionic compounds that have mixed anions and/or mixed cations. For Example I have seen this:
$$\ce{NaKCl2}$$
Also known as Sodium Potassium Chloride. The only information I can ...
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Is the bond in HF ionic while it is covalent in HCl?
Why would a hydrogen atom "donate" to fluorine in an ionic bond but not in $\ce{HCl}$? Why would $\ce{H}$ and chlorine share instead of $\ce{Cl}$ just stripping it away like $\ce{F}$ does?
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In my homemade electrolysis setup, only the negative end bubbles?
I've created an electrolysis setup by connecting a $6~\mathrm{V}$ battery to a cup filled with saline water via pencils; I am confused as to why only the negative pencil bubbles though. After running ...
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Difference between lattice energy and thermal stability
For an ionic compound, is it always true that the greater the thermal stability, the greater the lattice energy. E.g. for 2 ionic compounds MX and MY, if MX has a higher thermal stability than MY, ...
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Why is PbCl₄ covalent?
My answer: The inert pair effect in $\ce{Pb}$ causes it to pull back the electrons, resulting in polarisation.
My teacher's answer: An ionisation state of $+4$ is too difficult to achieve, and it is ...
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How would one compare the magnitude of covalent character between SnCl4 and SnF2 using Fajan's Rules?
It is easy to compare two ionic compounds when one of the ions is same. However, how do we compare two compounds if one of the ions is the same element but just has different charge and the other ion ...
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Why is potassium phosphate KH2PO4 in this reaction?
This is a continuation of this question because the first thing that came in my mind is that why potassium phosphate in this reaction is $\ce{KH2PO4}$ and not $\ce{K3PO4}$?
In the wikipedia article ...
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What is the difference between a Chemical Formula and Formula Unit?
In my textbook, a chemical formula is described as :
"A formula that shows the kinds and numbers of atoms in the smallest representative unit of a substance"
While a formula unit is described as :
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Calculating valence of oxides
Learning about Oxides. Basically when oxygen is combined with a metal.
$$\ce{FeO}$$
This is called "Iron Oxide (II)" according to my book.
Apparently, the II represents the valence. But how come? ...
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What is the analogue of "molecule" for ionic compounds?
In a system, if we have $\pu{18 g}$ of $\ce{H2O}$ ($M_\mathrm r = 18$), we can say we have a mole of water molecules or $6 \times 10^{23}$ molecules. But in another system, if we have $\pu{342 g}$ of $...
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Why doesn't LiHCO3 exist in solid state?
I have read that $\ce{LiHCO3}$ does not exist in solid state. Is it because of the size of anion-cation concept or is it something else? So why is it only for lithium and not for sodium too?
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Which has a greater dominance: hydration enthalpy or lattice energy?
When I was reading my notes I came up with a problem. I read that for the s block element salts, when checking the solubility, we consider the hydration enthalpy so we decide their stability in water. ...
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Are ionic bonds stronger than covalent bonds?
A covalent bond involves overlapping of orbitals while an Ionic bond involves charge separation.
Why are bonds formed by the overlapping of orbitals weaker than charge separation; why is an ionic ...
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What is the correct name for this lab technique in crystallization?
Take a glass rod and rub vigorously the wall of the flask, the substance will crystallize out of the solution.
Take a fire polished stirring rod and etch (scratch) the glass of your beaker. The small ...
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What happens to boiled (BMIM)PF6?
[BMIM]PF6, or 1-butyl-3-methylimidazolium hexafluorophosphate, is commonly used as an ionic liquid. As has been shown by the accepted answer to this question, sodium chloride that has been made to ...
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Why is benzenediazonium fluoroborate water insoluble and stable at room temperature?
Benzenediazonium fluoroborate is water insoluble and stable at room temperature.
Why is this salt, water insoluble? Also I am told that benzenediazonium salts are stable only at low temperature(<5°...
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Why exception is noted in the solubility of lead salts?
There are many exception in the solubility of lead salts like:
Lead sulfate is insoluble in cold water whereas most of the sulfates are soluble in cold water.
Lead chloride is also insoluble in cold ...
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Does water ionically bond to chloride ion?
This user absolutely insists that when a chloride ion is present in water (for example, when $\ce{NaCl}$ dissolves in water) that $\ce{Cl-}$ ion is ionically bound to the hydrogen atom:
https://...
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Is beryllium difluoride covalent or ionic?
My textbook says that despite the large electronegativity difference $\ce{BeF2}$ is covalent since the beryllium ion will have too much charge density and it will attract the fluorine electron cloud ...
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Color imparted to flame and color of coordination compounds
When we heat a ionic substance/compound, the ionic bond gets weakened and the metal is ionized. Is the color imparted to the flame due to absorption of light? i.e. Do we see the remaining wavelengths? ...
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Does lithium form ionic hydride? [duplicate]
It is stated in my chemistry textbook that lithium indeed forms lithium hydrides. However, significant covalent characters could be found in lithium hydrides (like least reactivity).
But in some other ...
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Predicting color of precipitate
Is there any way of predicting whether a precipitate will be colored? I know that for solutions, transition metal ions with unfilled d-orbitals will have color because of d-orbital splitting in the ...
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What would superionic water ice look like?
Phys.org's Giant lasers crystallize water with shockwaves, revealing the atomic structure of superionic ice links to
Nature Physics: Experimental evidence for superionic water ice using shock ...
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Why triiodide ion does not form ionic bond with cation having +2 charge?
In general, I found that triiodide ion generally forms ionic bond with cations having +1 charge like $\ce{NH4+I3-}$, $\ce{K+I3-}$, $\ce{Tl+I3-}$. But, I have never seen triiodide ion forming ionic ...
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Is there a word for a compound that has both ionic and covalent bonds?
For example, calcium carbide (CaC$_2$) has covalent C‒C bonds and ionic Ca$^{2+}$‒ C$_2^{2-}$ bonds.
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