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The question [Does H2SO or H2CO have a higher dipole moment?](https://chemistry.stackexchange.com/q/123020/41328) left me wondering whether $\ce{H2SO}$ has already been synthesized.
There are experimental evidences that both [hydrogen thioperoxide](https://en.wikipedia.org/wiki/Hydrogen_thioperoxide) $\ce{HSOH}$ (**... |
Does sulfoxide H₂SO exist? |
I am trying to understand the history of how Marcus theory moved from describing electron exchange reactions in aqueous ionic solutions to also being applied to describe transport in organic semiconductors. As in who and when was the connection made and justified? |
What is the justification for using the Marcus rate equation to model charge transport in organic semiconductors? |
> How many kilojoules are needed to react $\pu{25.0 g}$ of mercury(II) oxide?
> $$\ce{2 HgO -> 2Hg + O2}\quad ΔH = \pu{+182 kJ}$$
Correct answer is $\pu{20.5 kJ}.$ I get $\pu{10.5 kJ}.$ Here's how I did it:
1. Grams to moles: $200.59 + 16 = \pu{216.59 g}$ (using molar masses)
$$\pu{25 g} × \frac{\pu{1 mol... |
So I was doing analysis of Ag salts and I found Agbr is curry white partially soluble in ammonia , AgI is yellowish and insoluble . BUT silver phosphate is also yellow . So can anyone tell whether or is soluble in ammonia or not ? |
Sorry for the confusing title, I didn't know how to describe this better. So, if we douse rubber, say, a bicycle tire or a certain type of rubber glove, with organic solvent (n-heptane), we can find n-alkanes being dissolved in the solvent. Why is this? I'm talking especially about gas chromatography to analyse the par... |
Why n-alkanes can be found in organic solvent extract of rubber? |
*Study check 9.11* from \[1, p. 298\]:
> Mercury(II) oxide decomposes to mercury and oxygen.
> $$\ce{2 HgO -> 2Hg + O2}\quad ΔH = \pu{+182 kJ}$$
> […]
> **b**. How many kilojoules are needed when $\pu{25.0 g}$ of mercury(II) oxide reacts?
Correct answer is $\pu{20.5 kJ}.$ I get $\pu{10.5 kJ}.$ Here's how... |
Sorry for the confusing title, I didn't know how to describe this better. So, if we douse rubber, say, a bicycle tire or a certain type of rubber glove, with organic solvent (n-heptane), we can find n-alkanes being dissolved in the solvent. Why is this? I'm talking especially about gas chromatography to analyse the par... |
I'm trying to understand how to predict ground state term symbol of atoms.
After finding the biggest S, why the biggest L will be $L = |M_L|$, where $M_L = \sum m_l$?
I know this rule works to predict the total L, but it doesn't make sense to me that it will give the biggest L, to me it seems like this is the minim... |
Ground state term symbol, why is $L = |M_L|$, if L must be a maximum? |
I am trying do that what the title depicts, but I keep running into errors creating the executable script. Is it even possible to automate the docking of multiple ligands to multiple receptors?
**Below is the script that I have.** Right now I tried to get it to read from a configuration file, because the software c... |
Using AutoDock Vina to dock multiple ligands to multiple receptors? |
I am trying do that what the title depicts, but I keep running into errors creating the executable script. Is it even possible to automate the docking of multiple ligands to multiple receptors?
Below is the script that I have. Right now I tried to get it to read from a configuration file, because the software could... |
The question [Does H2SO or H2CO have a higher dipole moment?](https://chemistry.stackexchange.com/q/123020/41328) left me wondering whether $\ce{H2SO}$ has already been synthesized.
There are experimental evidences that both [hydrogen thioperoxide](https://en.wikipedia.org/wiki/Hydrogen_thioperoxide) $\ce{HSOH}$ (**... |
Sodium and potassium salts often can be used interchangeably - it these cases the difference in price and accessibility can be important. For example one can easily buy cheap sodium chloride in shop, but not potassium chloride, which isn't as cheap or accessible as NaCl. Other differences can be however very important.... |
In the 19th century, Na metal was isolated by heating up Na2CO3 + carbon to 1200 C and distilling and capturing the Na vapor under oil.
I tried it a few years ago with a small steel tube welded at the end as a retort and indeed vapors appeared burning with bright yellow (or purple in the case of K2CO3) flame, but c... |
Make Na or K using carbonate + charcoal? |
This is not an answer to the question "can the sulfoxide be synthesized in significant yield" (and under which conditions). Instead, this is a "naive" prediction based on the data you provide and two assumptions:
1. The predicted thermodynamic values in the articles you cite are accurate at 298 K.
2. The hea... |
This is not an answer to the question "can the sulfoxide be synthesized in significant yield" (and under which conditions). Instead, this is a "naive" prediction based on the data you provide and two assumptions:
1. The predicted thermodynamic values in the articles you cite are accurate at 298 K.
2. The hea... |
A nitro group is a strong deactivator whereas a halogen is a weak deactivator. The directing effects of these groups oppose each other: Nitro is meta directing whereas halogens are ortho/para directing. It is said that the strongest **activator** determines the directing effects in a disubstituted benzene ring. In a ri... |
I came across a statement saying,
> "Consider a **Octahedral** coordination compound of type [MA2X2]. Then,
> if the compound is in a cis form, it shows optical activity as there
> is no plane of symmetry and hence is non-superimposable on its mirror
> image. On the other hand, a trans form is symmetric and super... |
Question, with IR spectrum: https://i.stack.imgur.com/MQoUD.jpg
H-NMR spectrum: https://imgur.com/a/max7Rba
C-NMR spectrum: https://imgur.com/a/U2ohwuS
Based on the IR value, I reasoned that it is a ketone. Nothing else in the IR spectrum really stood out to me, so I stuck to the idea that it must be a ketone.... |
Am I using these spectra to identify the compound correctly? |
I see a lot of questions on electron configurations from students at various levels here. Students mechanically remember how to fill orbitals and sorry to say many teachers. Not a single general chemistry or even undergraduate physical chemistry book discusses the "why" part of orbital filling and what is the experimen... |
"Which oxidizing agent is more powerful" seems to depend on *what* is getting oxidized.
Consider for example oxygen vs chlorine. It is my understanding that chlorine is the more powerful agent for oxidizing sodium metal. The enthalpy of formation of sodium chloride is almost twice as negative as the oxide on a per-s... |
Rayleigh scattering occurs when the dimensions of the scatter is much smaller than the wavelength of the incident electromagnetic radiation.
Mie scattering occurs when the dimensions of the scattered is much larger than the wavelength of the incident electromagnetic radiation. An example is when light is scattered ... |
Does Mie Scattering occur in Liquid or is Rayleigh scattering? |
> So does Rayleigh or Mie scattering occur in liquid or bulk water? So why does Rayleigh scattering (?) occur in liquid/bulk water when the particles are much larger than the wavelength of light?
What is the approximate size of water molecule? It is on the order of 2.7 Angstroms or 0.27 nanometers. When we are talki... |
"Which oxidizing agent is more powerful" seems to depend on *what* is getting oxidized.
Consider for example oxygen vs chlorine. It is my understanding that chlorine is the more powerful agent for oxidizing sodium metal. The enthalpy of formation of sodium chloride is almost twice as negative as the oxide on a per-s... |
What exactly are Van der Waals forces? How do they arise and how can an instantaneous dipole cause another dipole? Shouldn't this make a chain reaction that causes all matter to eventually become polar? |
So I got myself a large Erlenmeyer flask, some steel wool and the bleach from the bathroom, mixing them under safe conditions in small quantities to see the sparky reaction I'd heard about. Trouble is, I didn't know the bleach we had was non-chlorine!
EDIT: My silly mind assumed that no reaction meant I had non-chlo... |
You see that both cases are Laporte-forbidden, now how about _spin-forbidden_?
Assuming the complex vibrates so it's no longer exactly octahedral, can you make a spin-allowed transition for $\ce{[Fe(CN)_6]^{4-}}$? How about $\ce{[Fe(H_2O)_6]^{3+}}$? When you answer this you will answer your question.
>! You sho... |
The post that was [linked to you in comments][1] contains a nice, short description of the 'traditional' categories of van der Waals interactions. I suggest you take a look at that, it might just be enough to clear things up. The reason I am writing this post is that the categories introduced there are defined somewha... |
In my organic chemistry book it says that the formation of cyclic hemiacetals is energetically favorable in comparison to the open chain aldehyde as two C-O single bonds are more stable than a C=O double bond. Why is this the case?
To be more precise, I am specifically talking about monosaccharides.
|
Why are two C-O single bonds more stable than a C=O double bond (hemiacetal)? |
In *Concise Inorganic Chemistry* by J.D.Lee (Adapted by Sudarsan Guha, Fourth Edition), on page 75, under the topic "Effect of Electronegativity - When the surrounding atom is same with different central atom having lone pair" it is given:
> The effect of electronegativity as postulated in VSEPR theory explains the ... |
I presume they are talking about bond enthalpies? A C-O is worth about 84 kcal while a C=O is about 127 kcal, so 2 x C-O has a larger total bond enthalpy. In a monosaccharide there is also additional stabilization of the acetal form through the anomeric effect.
However I think "stable" is a misnomer here (or at leas... |
In *Concise Inorganic Chemistry* by J.D.Lee (Adapted by Sudarsan Guha, Fourth Edition), on page 75, under the topic "Effect of Electronegativity - When the surrounding atom is same with different central atom having lone pair" it is given:
> The effect of electronegativity as postulated in VSEPR theory explains the ... |
In *Concise Inorganic Chemistry* by J.D.Lee (Adapted by Sudarsan Guha, Fourth Edition), on page 75, under the topic "Effect of Electronegativity - When the surrounding atom is same with different central atom having lone pair" it is given:
> The effect of electronegativity as postulated in VSEPR theory explains the ... |
In *Concise Inorganic Chemistry* by J.D.Lee (Adapted by Sudarsan Guha, Fourth Edition), on page 75, under the topic "Effect of Electronegativity - When the surrounding atom is same with different central atom having lone pair" it is given:
> The effect of electronegativity as postulated in VSEPR theory explains the ... |
> Do you think this is the correct molecule?
No, for three main reasons:
1. As Ezze states in the comment, there are strong indications for phenyl groups in the NMR spectra. One phenyl group corresponds to 4 double bond equivalents, which is incompatible with your molecular formula (too many hydrogen atoms).
2... |
> Do you think this is the correct molecule?
No, for three main reasons:
1. As Ezze states in the comment, there are strong indications for phenyl groups in the NMR spectra. One phenyl group corresponds to 4 double bond equivalents, which is incompatible with your molecular formula (too many hydrogen atoms).
2... |
In my organic chemistry book it says that the formation of cyclic hemiacetals is energetically favorable in comparison to the open chain aldehyde as two C-O single bonds are more stable than a C=O double bond. Why is this the case?
To be more precise, I am specifically talking about monosaccharides.
I quote from ... |
In my organic chemistry book it says that the formation of cyclic hemiacetals is energetically favorable in comparison to the open chain aldehyde as two C-O single bonds are more stable than a C=O double bond. Why is this the case?
To be more precise, I am specifically talking about monosaccharides.
I quote from ... |
> 3. What is the structure of the molecule whose data is shown below? Explain your answer [...] EI mass specturem: The highest peak observed is $m/z$ 210 and its abundance is low. The only other significant peak is observed at 167 Th (base peak). [...]
Full question text: https://i.stack.imgur.com/MQoUD.jpg
[![en... |
> 3. What is the structure of the molecule whose data is shown below? Explain your answer [...] EI mass spectrum: The highest peak observed is $m/z$ 210 and its abundance is low. The only other significant peak is observed at 167 Th (base peak). [...]
Full question text: https://i.stack.imgur.com/MQoUD.jpg
[![ent... |
Kinetic Diameter: How to calculate it? Pressure influence? |
How do I know which alkane has the lowest combustion heat? |
> Which isomer would have the largest heat of combustion?
> **A) Propylcyclopropane**
> B) Ethylcyclobutane
> C) Methylcyclopentane
> D) Cyclohexane
> E) Since they are all isomers, all would have the same heat of combustion.
Can anyone explain why?
If you think about it, without having the data of... |
Why can't the 2 oxygen atoms donate a lone pair and hence become binding sites? Is it because of the angle made by the oxygen and Nitrogen atoms? |
Why is dimethylglyoximate a bidentate ligand and not a tetradentate ligand? |
> a C=O double bond becomes two C-O single bonds, and those C-O single bonds are slightly more stable than the C=O double bond
For completeness, these are not the only changes. In addition, the O-H bond of the hydroxyl group is broken, and the O-H bond of the hemiacetal is formed. If you are estimating bond dissocia... |
> Do you think this is the correct molecule?
No, for three main reasons:
1. As Ezze states in the comment, there are strong indications for phenyl groups in the NMR spectra. One phenyl group corresponds to 4 double bond equivalents, which is incompatible with your molecular formula (too many hydrogen atoms).
2... |
> a C=O double bond becomes two C-O single bonds, and those C-O single bonds are slightly more stable than the C=O double bond
The tables I found (e.g. [OpenStax Chemistry][1], [Wikipedia][2]) have the C=O bond with roughly twice the bond dissociation energy compared to the C-O bond, and in all cases the C=O bond is... |
In my organic chemistry book it says that the formation of cyclic hemiacetals is energetically favorable in comparison to the open chain aldehyde as two C-O single bonds are more stable than a C=O double bond. Why is this the case?
To be more precise, I am specifically talking about monosaccharides.
I quote from ... |
> a C=O double bond becomes two C-O single bonds, and those C-O single bonds are slightly more stable than the C=O double bond resulting in ΔH being slightly positive.
The tables I found (e.g. [OpenStax Chemistry][1], [Wikipedia][2]) have the C=O bond with roughly twice the bond dissociation energy compared to the C... |
I am trying do that what the title depicts, but I keep running into errors creating the executable script. Is it even possible to automate the docking of multiple ligands to multiple receptors?
Below is the script that I have. Right now I tried to get it to read from a configuration file, because the software could... |
I see a lot of questions on electron configurations from students at various levels here. Students mechanically remember how to fill orbitals and sorry to say many teachers do the same. Not a single general chemistry or even undergraduate physical chemistry book discusses the "why" part of orbital filling and what is t... |
This question was given by my chemistry professor, but I doubt that this question is not correct.
Following the lewis definition of the acid, any molecule or atom acts as a acid if it accepts an electron and according to *Inorganic Chemistry by Weller* CO is a good $\pi$ acceptor, then how it can be weak pi-acid lig... |
Why CO is a weak pi-acid ligand? |
> Arrange in ascending order of heat of combustion:
> [![substituted cyclohexanes][1]][1]
I know heat of combustion is inversely proportional to stability. Also, to solve I did try making chair conformations of the substituted cyclohexane.
In same type of, say, 1,3,5-conformations one can do comparisons by see... |
Wikipedia states: 'Kinetic diameter is a measure applied to atoms and molecules that expresses the likelihood that a molecule in a gas will collide with another molecule. It is an indication of the size of the molecule as a target.' (https://en.wikipedia.org/wiki/Kinetic_diameter)
And the following equation is given... |
[Wikipedia](https://en.wikipedia.org/wiki/Kinetic_diameter) states:
> **Kinetic diameter** is a measure applied to atoms and molecules that expresses the likelihood that a molecule in a gas will collide with another molecule. It is an indication of the size of the molecule as a target.
And the following equation... |
> Do you think this is the correct molecule?
No, for three main reasons:
1. As Ezze states in the comment, there are strong indications for phenyl groups in the NMR spectra. One phenyl group corresponds to 4 double bond equivalents, which is incompatible with your molecular formula (too many hydrogen atoms).
2... |
I'm surprised your textbook did not derive this equation from the [reaction isotherm relationship][1] between $\Delta G$ and the reaction quotient $Q$ and the [Nernst equation](http://en.wikipedia.org/wiki/Nernst_equation). The derivation is not hard.
Reaction isotherm equation:
$$\Delta_\mathrm{r} G =\Delta_\mat... |
I want to make NaOH from NaHCO3, what is the easiest way to do it without electrolysis? |
> Do you think this is the correct molecule?
No, for three main reasons:
1. As Ezze states in the comment, there are strong indications for phenyl groups in the NMR spectra. One phenyl group corresponds to 4 double bond equivalents, which is incompatible with your molecular formula (too many hydrogen atoms).
2... |
> Do you think this is the correct molecule?
No, for three main reasons:
1. As Ezze states in the comment, there are strong indications for phenyl groups in the NMR spectra. One phenyl group corresponds to 4 double bond equivalents, which is incompatible with your molecular formula (too many hydrogen atoms).
2... |
> Do you think this is the correct molecule?
No, for three main reasons:
1. As Ezze states in the comment, there are strong indications for phenyl groups in the NMR spectra. One phenyl group corresponds to 4 double bond equivalents, which is incompatible with your molecular formula (too many hydrogen atoms).
2... |
I have been looking everywhere for an explanation to a reaction mechanism concerning the oxidation of DTT (or just thiols to disulfides in general) using oxygen as the oxidant. I'm aware that oxidizing DTT with oxygen (O2) will give me the oxidized form of DTT and H2O2. However, I'm running my reaction in MeOH and KOH ... |
Reaction mechnism of thiol oxidation in basic conditions? |
Reaction mechnism of thiol oxidation under basic conditions? |
What is the relationship between the three concepts in the title?
I know all centrosymmetric molecules are achiral, but not all achiral molecules are centrosymmetric. Thus, there are no molecules that are centrosymmetric and chiral, but all other combinations exist.
What about having a dipole moment vs. centrosym... |
In my book it is given that the crystal field stabilisation energy for [Cr(en)3]Cl3 is more than that of the complex [Cr(H2O)6]Cl3. By what i have studied the crystal field stabilisation energy depends on the number of electrons in t2g and eg orbitals and the pairing energy. So the number of electrons in both the compo... |
What is the order of crystal field stabilisation energy for the following? |
1: [Ni(en)2]^+2 > [Ni(dmg)2]
2: [Fe(EDTA)]^-2 > [Fe(en)3]^+3
In the first case i think the stability depends upon the strength of the ligand so is en stronger than dmg to form a more stable compound? As the oxidation state of ni is same for both the cases.
In the second case the oxidation state of fe is +2 and... |
Which stability order is correct? |
Sorry for the confusing title, I didn't know how to describe this better. So, if we douse rubber, say, a bicycle tire or a certain type of rubber glove, with organic solvent (n-heptane), we can find n-alkanes being dissolved in the solvent. Why is this? I'm talking especially about gas chromatography to analyse the par... |
Why does not aqua regia burn filter paper? |
> Which stability order is correct?
> 1. $\ce{[Ni(en)2]^2+} > \ce{[Ni(dmg)2]}$
> 2. $\ce{[Fe(edta)]^2-} > \ce{[Fe(en)3]^3+}$
In the first case I think the stability depends upon the strength of the ligand so is $\ce{en}$ stronger than $\ce{dmg}$ to form a more stable compound? As the oxidation state of nickel is... |
In my book it is given that the crystal field stabilisation energy for $\ce{[Cr(en)3]Cl3}$ is more than that of the complex $\ce{[Cr(H2O)6]Cl3}.$ By what I have studied, the crystal field stabilisation energy depends on the number of electrons in $\mathrm{t_{2g}}$ and $\mathrm{e_g}$ orbitals and the pairing energy.
... |
What is the order of crystal field stabilisation energy for tris(ethylenediamine)cobalt(III) chloride and hexaaquachromium(III) chloride? |
Under what circumstances that LLE would be useful ?
Are the 2 top reasons -
1. Difference between the boiling points of the components are very low or similar.
2. For Temperature sensitive compounds as there is no heating which may cause thermal decomposition.
are there any other reasons ? |
Under what circumstances that Liquid-Liquid extraction would be good to use? |
\begin{align}
\ce{NaOH &-> Na+ + OH-} & \Delta H^\circ &= \pu{-44.51 kJ/mol}
\end{align}
The dissolution of sodium hydroxide in water is an exothermic process, and so, according to Le Chatelier’s principle, cooling the container should shift the reaction to the right. Shouldn’t this mean that cooling the container... |
Why is heating increasing the solubility of sodium hydroxide? |
First off I would like to say that my knowledge on chemistry, even general chemistry, is basic if not poor.
That said, I have some intuituions on this matter. I haven´t found any paper regarding this kind of system, and that is pretty much a killer for me.
Even with that I´d still like to ask the question.
Ion... |
What is the order of crystal field stabilisation energy for tris(ethylenediamine)chromium(III) chloride and hexaaquachromium(III) chloride? |
Is it possible to use the Laws of Thermodynamics for non-ideal systems? |
I was reading about different types of radius existing between atoms. It was written that If any atom can possess all types of radii, then van der Waals radius will be greater than metallic radius.... |
What if we want to take chlorophyll in a container and put it into light then chlorophyll will lose electrons and will become positive itself then we will have a solution of negatively flowing electrons and positively charged chlorophyll molecules but somehow we have to take to lose electrons and transfer them somewher... |
Topic: Chemical Bonding (Application of Bent's Rule)
> Bent's rule is also consistent with Gillespie's VSEPR model, and may provide alternative rationalisation for effect of electronegativity. So it is restated as: '*more electronegative atom not only prefers to stay in the orbital having more p character but also can... |
I have been looking everywhere for an explanation to a reaction mechanism concerning the oxidation of DTT (or just thiols to disulfides in general) using oxygen as the oxidant. I'm aware that oxidizing DTT with oxygen ($\ce{O2}$) will give me the oxidized form of DTT and $\ce{H2O2}$. However, I'm running my reaction in... |
Reaction mechanism of thiol to disulfide oxidation under basic conditions? |
What if we want to take chlorophyll in a container and put it into light . Then chlorophyll will lose electrons and will become positive itself then we will have a solution of negatively flowing electrons and positively charged chlorophyll molecules. But somehow we have to take to lose electrons and transfer them som... |
What if we want to take chlorophyll in a container and put it into light . Then chlorophyll will lose electrons and will become positive itself then we will have a solution of negatively flowing electrons and positively charged chlorophyll molecules.
But somehow we have to lose electrons and transfer them somewhe... |
The paragraph you cite does not define Bet's rule (see [What is Bent's rule?](https://chemistry.stackexchange.com/q/15620/4945), [Utility of Bent's Rule - What can Bent's rule explain that other qualitative considerations cannot?](https://chemistry.stackexchange.com/q/15671/4945)).
If you compare $\ce{H3CCl}$ and $... |
Ratio of Water to Isopropyl Alcohol? |
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