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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Rock salt structure: chloride lattice or sodium lattice?

Source From this diagram of the rock salt structure ($\ce{NaCl}$) we see that both the chloride and sodium ions have the same environment. That is to say, they each have the same number of neighbours ...
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Why are the ozonides of heavier elements more stable?

The ozonides of $\ce{Cs}$, $\ce{Rb}$, $\ce{K}$ are well known and relatively stable, but there is little mention of the ozonides of $\ce{Na}$, $\ce{Li}$. Why is this?
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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 do we experimentally know the strength of bonds?

How do we experimentally measure the strengths of covalent versus ionic bonds? Also, for a given molecule, how can we know if two pairs of atoms is covalently or ionically bound? Related question: ...
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Ionic bonds- are electrons transferred?

In an ionic bond, are electrons actually transferred from one atom to the other to form a positive and a negative ion OR are ionic bonds just extremely polar covalent bonds? Sorry if this seems like a ...
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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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1answer
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Why are electrons transferred in an ionic bond?

I've been taught at school that in an ionic compound like $\ce{NaCl}$, electrons are transferred from the $\ce{Na}$ to the $\ce{Cl}$ to form $\ce{Na+}$ and $\ce{Cl-}$ which both have full outer shells....
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269 views

How do you solve a net ionic equation without a balanced equation?

In class, my professor went over a method for finding the net ionic equation without determining the balanced equation (e.g., if finding the balanced equation was too difficult for us students). It ...
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How is the dichromate anion generated from potassium dichromate? [closed]

How does $\ce{K2Cr2O7}$ become $\ce{Cr2O7^2-}$ when dissolved in water?
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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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Ionic compounds dissolve in nonpolar compounds?

I think ionic compounds dissolve in just about any compound including nonpolar. My reasoning is this: Neutral electric charge attracts both positive and negative (This I know from doing things with ...
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468 views

Are non-ionic compounds generally as dehydrating as ionic compounds in drinking water?

In order to turn sea water into drinkable water, virtually all of the salt must be removed. By definition, salts are ionic compounds. I am assuming that there are other non-ionic compounds devolved ...
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Why does a Fluoride ion only have a -1 charge and not a -2 charge or more?

Transition elements can form ions with different charges. Why can't elements other than transition elements form ions with different charges? If it is a Fluoride ion, why does it have to be an anion ...
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Dipole moment - calculation of percentage ionic character

Question: The dipole moment of $\ce{HBr}$ is $2.60 \times 10^{-30}$ and the interatomic spacing is $1.41$. What is the percentage ionic character of $\ce{HBr}$? What I know is that the percentage ...
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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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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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Chemical bonding - lattice energy

Question: Why is ionic lattice energy inversely proportional to the radius of the atom? Most heterogeneous covalent molecules are polar to some extent. The degree of polarity, or the dipole moment, ...
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Why is Aluminium Chloride a Lewis Acid if it's an ionic compound?

In my textbook it says in the reaction $\ce{AlCl3 + Cl- -> AlCl4-}$, Aluminium Chloride ($\ce{AlCl3}$) has six valence electrons and accepts a lone pair from $\ce{Cl-}$, but wouldn't that mean the ...
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Solvent for copper(I) iodide, copper(I) thiocyanate, silver iodide for HTM deposition; safety for methylammonium lead iodide

I'm a student working in a high school laboratory that is looking to pursue research into perovskite cells for next year, but I have some solubility and safety questions. What would be a good solvent ...
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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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Chemical Equation: Sulfuric acid and powdered sodium carbonate

I was asked to write a balanced chemical equation for the reaction between sulfuric acid and sodium carbonate. The balanced equation isn't the problem. The question asks to also show all the state ...
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Find the pH of a sodium chloride solution using the extended Debye-Huckel equation

Question Use activities to calculate the pH of each of the following solutions, being sure to use $\mathrm{\alpha}$ values and the extended Debye-Huckel equation. The first one the ...
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1answer
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Why does NaCl dissolve in H2O despite its strong ionic bond? [duplicate]

If $\ce{NaCl}$ is such a strongly bonded ionic compound, why it does it disassociate so readily in $\ce{H2O}$? One would think that because of the very strong ionic bond it would not disassociate it ...
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The Crisscross method for finding the chemical formula

I am reading this wikipedia article that I don't understand. What I don't understand is: suppose we have two elements $X$ and $Y$ having oxidation numbers $x$ and $y$ respectively. Can we prove ...
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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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Can an organic compound have an ionic bond?

Is there any organic compound that has another type of bond other than the covalent bond?
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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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1answer
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Ionic Strength of 0.1M of HEPES?

HEPES, the buffer, has the chemical formula $\ce{C8H18N2O4S}$. Using the Ionic Strength formula from Wikipedia. I have calculated that $0.1M$ of HEPES would have a strength of $1.7M$, would it be ...
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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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Is melting of NaCl a physical and chemical process?

If I melt $\ce{NaCl}$, I get a molten salt. This means a liquid formed only by ions ($\ce{Cl^-}$ and $\ce{ Na^+}$). That could mean that the crystal $\ce{NaCl}$ experimented a chemical change: $$\ce{ ...
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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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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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Can polyatomic ions (CO₃, PO₄, SO₄, NO₃) be considered conjugated systems?

From my perspective these resonance structures allow these specific polyatomic ions to act as donor-acceptor molecules. Many donor-acceptor molecules also tend to be conjugated systems because they ...
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Why are cations ordinarily smaller than anions?

I'm reading on ionic crystal structures and am confused by this from my textbook: Because the metallic elements give up electrons when ionized, cations are ordinarily smaller than anions I ...
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Epsom salts - heavy metal contamination myth?

This recipe for home-made handwash (liquid soap) consists of bar soap, water, Epsom salts, and coconut oil. The author specifically warns against using 'artificial' Epsom salts, preferring the ...
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Ionic or covalent bond

Which bond is stronger, ionic or covalent? I have a lot of confusion about this.
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How to identify ionic compounds

I have a Chemistry lab in which I must design and carry out an experiment to determine the compound in each of eight numbered vials. Each vial contains one of these ionic compounds: BaCl2 CaCO3 Ca(OH)...
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Why do ionic compounds dissociate whereas coordinate complexes won't?

An ionic bond is the bonding between a non-metal and a metal, that occurs when charged atoms (ions) attract after one loses one or more of its electrons,and gives it to the other molecule, for example ...
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Why is zinc deposited on copper when boiling an aqueous zinc sulfate solution?

I did an experiment where I dissolved 30 grams of zinc sulfate in water and boiled it with strips of solid zinc metal and strips of copper metal and a layer of zinc was deposited on the copper. I ...
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How did Halogens become known as Halogens? They are not the only elements that form salts!

Having never given it a though before, I recently discovered (in a different context) that the prefix halo- actually means 'salt' or 'sea' and the suffix -gen means 'to form' or 'to generate'. So the ...
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What does “/2” in the structure of calcium benzoate mean?

Please see the following figure. This is from the high school chemistry book of my son. He wants to know what does that /2 after $\ce{-COOCa}$ mean. The book is a non English one. And I have changed ...
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Would dissolving a salt and letting it sit for 48 hours have an effect on the solution?

If one were to dissolve magnesium citrate (about $100~\mathrm{mg}$) in water (about $70~\mathrm{ml}$) and let the solution sit for 48 hours, would the solution be exactly the same as one dissolved and ...
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How are pure substances (elements, compounds, etc) produced? [closed]

How are large quantities of the substances we use in the lab generally produced? (As in the process from getting the stuff out of the ground to use in the lab) How 'pure' are they? Also: is it ...
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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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How to solve this contradiction?

I am getting confused about this the more problems I do on it. My understanding was that only strong acids and strong bases will react to produce water and a salt. Something like this: Molecular Eq: $\...
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2answers
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How many valence electrons does the azide ion have?

We had a test and and we had a question asking the number of valence electrons in an azide ion, $\ce{N3^{-}}$. I find out that the answer is 16 but I could not understand how. I saw the structure. ...
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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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Chemically removing rust without leaving any unwanted residues

I have this iron pan that got rusty from not being properly dried. Scrubbing it I was able to get rid of most of the rust, but there's still some I just can't remove. I thought I could chemically ...
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How to rationalise the coordination number of CsCl versus NaCl?

Question: Suggest an explanation for the coordination number in the $\ce{CsCl}$ lattice being different from those in $\ce{NaCl}$. Standard answer: Caesium ion is larger than sodium ion, hence ...
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Effect of light on ionic compounds

If I had an ionic molecule which needed $\pu{4 eV}$ to break the ionic bond, a $\pu{7 eV}$ photon is shot at it. If it is absorbed by the molecule and breaks, where does the rest of the energy go?

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