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.

Filter by
Sorted by
Tagged with
-2
votes
0answers
26 views

Determine if an unknown solid is a covalent network structure or ionic solid by doing tests on it [closed]

What test could I run on the solid to find this out without melting/boiling it?
-3
votes
0answers
23 views

How can I determine if an unknown solid is an Ionic solid or a Covalent network solid? [duplicate]

What test could I run on the solid to find this out without melting/boiling it?
-1
votes
2answers
102 views

Isn't hydrogen chloride a salt, because it is an ionic compound? [closed]

So I just learned in chemistry that salts are ionic compounds. Shouldn't, $\ce{H+Cl-}$ be a salt since hydrogen ion has positive charge and chloride ion has negative charge? If $\ce{HCl}$ is a salt ...
-1
votes
2answers
52 views

What is the correct molecular, total ionic, and net ionic reaction equation of reaction between magnesium nitrate and sodium chromate? [closed]

From the question, I think that the reactants are $$\ce{Mg(NO3)2(aq) + Na2CrO4(aq)}$$ But the problem is, I am confused about the result of the reaction. Is it $$\ce{MgCrO4}$$ and/or $$\ce{NaNO3}$$? ...
0
votes
1answer
23 views

Databases for Enthalpy of Solution and Ionic Radii for Ionic Salts

I am looking to investigate the relation between experimental enthalpies of solution and theoretical enthalpies of solution calculated using theoretical equations for the lattice enthalpy and ...
3
votes
2answers
198 views

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 ...
0
votes
1answer
51 views

Why is the thermal stability of calcium carbonate higher than that of magnesium carbonate even though lattice energy decreases down a group?

The difference in thermal stability of $\ce{CaCO3}$ and $\ce{MgCO3}$ can be explained using Fajans' rules, but why not using the lattice energy method? Why is the thermal stability of $\ce{CaCO3}$ ...
0
votes
0answers
32 views

Determining ion charge using rate constants and ionic strength

I am given the following data: The rate constant $k$ at $\pu{25 ^\circ C}$ in a reaction of persulfate ions and iodide ions in a water solution is assumed to vary with the total ionic strength of the ...
1
vote
0answers
99 views

Why does iodine trichloride dimerize?

In which of the dimerization process, the achievement of the octet is not the driving force $\ce{2AlCl3 \to Al2Cl6}$ $\ce{BeCl2 \to BeCl2}$ (solid) $\ce{2ICl3 \to I2Cl6} $ $\ce{2NO2 \to N2O4}$ ...
1
vote
1answer
265 views

Can chemical composition be determined from elemental composition?

I have the energy dispersive X-ray spectroscopy results from a sample of salt that I produced by collecting and processing ocean water by filtering, boiling, evaporating, and additional steps to try ...
0
votes
1answer
19 views

Calculating Heat of Solution of a Compound comparing to other compound data

For example if I have a table with these data How can those data be compared with each other to find heat of solution of $\ce{KI}$?
-1
votes
1answer
74 views

Are there any coordinate covalent bonds in potassium ferricyanide? [closed]

From my analysis, potassium ferricyanide has 3 ionic bonds between $\ce{K^{+}}$ & $\ce{[Fe(CN)_6]^{-3}}$. Between carbon and nitrogen atoms of 6 $\ce{CN^-}$ ions, there are $3\times 6=18$ covalent ...
6
votes
1answer
259 views

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 ...
2
votes
2answers
488 views

Why are entries missing on a solubility data chart for ionic compounds? [closed]

There is a solubility chart in my college chemistry class text for "Solubility of Ionic compounds in water". I have copied and pasted image of chart below. I was surprised to find a dozen ...
0
votes
1answer
58 views

Calculating the ionic strength for an aqueous solution containing potassium ferricyanide and sodium sulfate

I have the $100$ microM of K$_3$Fe(CN)$_6$ is dissolved in water and the following data: $$\begin{array}{c|c} \text{Experiment} & \ce{[Na_2SO_4]}/\pu{M} \\ \hline \mathrm{A} & 0 \\ \mathrm{B} ...
5
votes
2answers
197 views

Why does the dissolution of calcium hydroxide have a negative entropy?

We had an experiment on the dissolution of calcium hydroxide and we obtained the experimental entropy value $\pu{-203 J mol^-1 K^-1}$ with a percent error of $26.7\%.$ Doesn't dissolving a solid in a ...
-1
votes
1answer
68 views

Forces operating in molten ionic solids

What type of forces exist between ions in molten ionic solids? If this force is electrostatic attraction only, then how is it different from electrostatic interaction when ionic compound exist as ...
3
votes
0answers
72 views

Calculating the ionic strength of a histidine solution

I'm trying to repeat the calculation of the ionic strength of a solution containing histidine as a buffer I recently read in a paper. In their paper, the authors calculate the ionic strength of a 20 ...
2
votes
2answers
66 views

Is ionisation an equilibrium process?

I read in a page that ionisation is an irreversible process. But, as equilibrium is always reversible would that mean equilibrium does not involve ionisation process. And than dissociation is a ...
1
vote
2answers
449 views

Determining whether a compound is ionic or molecular in nature [closed]

$\ce{HCl}$ is a molecular compound because there is a covalent bond between $\ce{H+}$(a proton) and $\ce{Cl-}$ (a chloride ion) $\ce{NH4NO3}$ is an ionic compound because there is an ionic bond ...
1
vote
0answers
124 views

What force causes an electron to jump from say Na to Cl?

Every explanation I can find says something like: valence electrons in metals have low ionising energies and non-metals ''want'' to complete their valence shell. But I can't seem to get my head around ...
-2
votes
1answer
56 views

Do hydrides, like NaH or CsH, also form H-bond? [closed]

I know that when hydrogen acts as a cation, it can form H-bonds with the electronegative ions or groups. But, is this also true for anionic hydrogens? Will they form similar bonds, other than the ...
2
votes
1answer
31 views

Would ionic conduction be halted by shielding at the electrodes?

I've done this experiment myself and seen it front of my eyes. Set up a basic circuit with a battery, an LED, and connect the circuit with a salt-water solution and copper wire. The LED lights up. If ...
5
votes
0answers
115 views

Why does beryllium have an exceptionally high hydration energy?

You would expect solubility of Group $2$ fluorides to increase down the group, as lattice energy plummets much more sharply than hydration energy does. For the most part, this is true: $\ce{BaF2}$ is ...
-1
votes
2answers
83 views

Is this analogy right? [closed]

Is my logic correct in this case ? Since the formal charge represents the charge the element possess in a covalent compounds, is it right to say that formal charge is the equivalent term for covalent ...
3
votes
1answer
78 views

Are Group 2 metal fluoride salts less soluble in organic solvents than Group 1 fluorides?

It is clear that Group 1 metal fluoride salts DO NOT readily form solutions in organic medium. The amount of solvation that can occur leading to the eventual release of a fluoride ion depends on many ...
-3
votes
1answer
112 views

How do I calculate weight percent of BaCl2

A $\pu{0.1036 g}$ sample containing only $\ce{BaCl2}$ and $\ce{NaCl}$ is dissolved in $\pu{50 mL}$ of distilled water. Titrating with $\pu{0.07916 M}$ $\ce{AgNO3}$ requires $\pu{19.46 mL}$ to reach ...
2
votes
1answer
111 views

On the exact definitions of Frenkel and Schottky defects

The wiki page on vacancy defects says; It is also known as a Schottky defect, although in ionic crystals the concepts are not identical. As far as I'm aware, they're the same. Furthermore, the wiki ...
4
votes
0answers
65 views

Dielectric constant for gases possessing van der Waals forces [closed]

I've learnt that water can dissolve ionic bonds because it possesses a high dielectric constant. In the cases of covalent compounds (especially the non-polar covalent compounds), where the molecules ...
2
votes
1answer
961 views

Finding the atomic packing factor (APF) of Sodium Chloride and other FCC ionic compounds

For a piece of coursework I am doing, I need to calculate the atomic packing factor of some ionic compounds. I have had no formal teaching in this area, so what I know comes from information I have ...
1
vote
2answers
238 views

charge density as a measure of lattice enthalpy & polarizing power?

My official CIE A level textbook, and some mark schemes mention the following: Ions with the same charge have a lower charge density if their radius is large. This is because the same charge is ...
1
vote
2answers
610 views

Understanding strong acid titrated with weak base graph

I don’t understand why the conductivity doesn’t change after the equivalence point. To my understanding, at the equivalence point there is $\ce{NH3}$, $\ce{NH4+}$ and $\ce{Cl-}$ in the solution. As ...
2
votes
1answer
242 views

Why is the ionic radius of hydride so large?

The order of ionic radii for halides and hydride is apparently as follows: $$\ce{F-} < \ce{Cl-} < \ce{Br-} < \ce{H-} < \ce{I-}$$ Why is the hydride ion so large, even larger than bromide ...
2
votes
0answers
44 views

A trick to find resultant pH [duplicate]

Consider the following problem: Find the $\mathrm{pH}$ of the solution formed by the mixing of two solutions of $\mathrm{pH}$(s) $2$ and $3$ of equal volumes. The normal way: Since the resulting ...
2
votes
1answer
71 views

Is there a notion of generalized acidity for lithium ions?

From my understanding, the basic notions of acidity can be explained by considering a cup of pure water, and then adding a substance to it which creates either free $\ce{H+}$, or free $\ce{H3O+}$ and $...
3
votes
0answers
44 views

Expression comparing the Solubility of Ionic compounds

In chemical bonding, I am taught an expression that compares the Solvation Energy and the Lattice Energy of an ionic compound which is being dissolved in a polar solvent (could be water, could be ...
4
votes
1answer
548 views

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 ...
2
votes
1answer
443 views

Order of solubility of sodium halides and potassium iodide

Order the following ionic compounds in decreasing order according to their ease to dissolve in water. a) NaBr; b) KI; c) NaF; d) NaCl. d > a > b > c a > b > c > d b > c > d &...
-1
votes
1answer
95 views

Is there a room temperature ionic liquid permanganate [closed]

I need to figure out a permanganate based ionic liquid that is usable at room temperature. Unfortunately, information on which compounds could be usable and which ones aren't is scarce. That's why I'm ...
0
votes
1answer
53 views

When converting between a hydrated electrolyte amount in mass and in milliequivalents (meq), why are the water molecules taken into account?

A textbook I'm reading called "Ansel's Pharmaceutical Calculations, 13th edition" defines the milliequivalent (meq) thus (p. 187): This unit of measure is related to the total number of ...
1
vote
0answers
30 views

What kind of bond exists between a metal and a non-metal with a difference in electronegativity of less than 1.7? [duplicate]

I'm being taught that the kind of bonds that exist between elements depends on the electronegativity difference between the elements. A difference less than 1.7 is covalent and a difference higher ...
-4
votes
1answer
132 views

How does a body lose electrons? [closed]

If there is a Na and cl in solid form , There will be atoms inside of them.How do they lose electrons ?.We know solid body has a structure and covering.Just like you can touch is the covering of table ...
2
votes
2answers
116 views

When writing the net ionic equation, if one of the products ionizes, what is the most appropriate way to account for this in the answer?

Take these two practice problems and their solutions from Ebbing (8th ed) that involve completing the molecular equation, then writing the net ionic equation: 4.42a: $\ce{Ca(OH)2(aq) + 2H2SO4(aq) ->...
1
vote
1answer
191 views

Why does lattice enthalpy decrease with increasing ionic size?

Lattice enthalpy decreases as ions get larger, but I have found two explanations: The charge density is greater in smaller ions, so greater attraction The ions are themselves able to get closer ...
-1
votes
1answer
56 views

bonding in polar covalent bonds

I have recently learned that pure ionic and covalent bonds are just the extremes of a spectrum of bonds from this article from Chemguide. But I can't seem to square this with my understanding of how ...
1
vote
0answers
335 views

How to determine the van't Hoff factor for different salts in water experimentally?

How do I experimentally determine the van't Hoff factor for different salts in water? I'm going to dissolve each of sodium chloride, potassium chloride, and lithium chloride in $\pu{20 mL}$ of water ...
2
votes
2answers
299 views

What exactly is lattice energy?

I was going through my chemistry textbook (Chemistry, 10th Ed. by Raymond Chang) when I encountered this explanation of lattice energy. 9.3 Lattice Energy of Ionic Compounds We can predict which ...
2
votes
0answers
806 views

why does lithium fluoride have a higher lattice energy than lithium iodide?

Based on my knowledge, lattice energy is proportional to the multiplcation of the charge of the ions, divided by the sum of the radius of ions, as follows. Since iodide has a larger radius than ...
-3
votes
1answer
89 views

Lewis structures and chemical-compound formulas [closed]

In the Lewis structures listed below, M and X represent various elements in the third period of the periodic table. Write the formula of each compound using the chemical symbols of each element: a. b. ...
0
votes
0answers
156 views

When you melt an ionic compound, do you "break" its electrostatic force of attraction, or its lattice energy?

I know that the melting point and the boiling point of ionic compounds are very high. However, when I was trying to find the reason for this, I found that this is because of the high electrostatic ...

1
2 3 4 5
9