Inorganic Chemistry - Science topic

Yes in Copper(II)acetate monohydrate have one metal-metal (δ bond) bond involving

dx²-y² orbital. Also in more detailed way we can say it is due to this interection the two unpaired electron present in each dx²-y² orbital of each Cu centre will undergo antiferromagnetic superexchange interection. AS a consequence the system becomes diamagnetic. Also we can explain interms of molecular orbital theory.

Dear Leshan Usgodaarachchi

The golden example of this topic is the morphology changes of alumina nano particles as a function of their phase transformations and crystalline structure. In [1] you find what you looking for.

Best regards ]

[1]

It is a China made low-field NMR Company, which has the special products for crosslinking density measurement.

Dear Jamal Nasir,

Below is the option to see the error/s.d. in Topas v6, as Marcella Bini pointed out.

This is a typical calibration procedure. You will need multiple concentrations to develop a quantitative response relation that you will use to estimate concentrations in your samples

Many chemicals have several names: trivial and systematic (IUPAC nomenclature, red book), and in this case there can be two nomenclature names - anionic and oxide form. In this case, delafossite is a trivial name (from mineralogy, but it can be from technology, everyday life ...), copper (I) ferrite is an anionic form (there is another copper ferrite CuFe₂O₄ - copper (II) ferrite) and copper oxide (I)-iron(III)) - oxide form of the systematic name.

Harald G. Dill

... If names are not right, words do not fit. If words do not fit, affairs go wrong. ...A gentleman is nowise careless of his words. ... Confucius. Analects XII.3.

Hello Darren,

many thanks for sharing this very interesting chemical problem with the RG community. Since you have a reaction system with three different components, it is rather difficult to say what has formed as orange / pink precipitate without having any analytical data. What can be said is that sodium hypophosphite (NaH₂PO₂) is a strong reducing agent, so that the formation of trivalent iron species like Fe(OH)₃ can be ruled out. You mentioned that your "orangish precipitate isn't dissolving". Dissolving in what?

I suggest that you should have an elemental analysis of your precipitate done. You can also digest your precipitate in concentrated HNO₃ and than do quick tests for cobalt, iron, and phosphorus. It cannot be ruled out that the precipitate contains phosphorus.

Good luck with your experiments!

Hello Viraj,

thank you for posting this very interesting technical question on RG. We work in the field of synthetic inorganic chemistry, so that I would not call myself a proven expert in the field of heterogeneous catalysis and transesterification. However, I can suggest to you two very instructive review articles which will certainly help you in your analysis. Thus please have a look at the following references:

Fortunately this paper has been posted by the authors as public full text on RG, so that you can freely download it as pdf file.

The other paper can also be accessed as public full text as it has been published Open Access:

(Please see the attached pdf file)

I hope this helps. Good luck with your work!

Nalidixic acid - A NSAID grs of drugs or pain killer .REF : en.wikipedia.org ( Image Source ) .

The subject of specialisations does not depend on the feature income rather your subject if interest . Organic chemistry has too much scopes as a synthetic( R&D) chemist in multinational pharmaceutical houses like Chem biotech , Pfizer , DRL labs etc etc. Even in post doc level abroad from India very high scope in organic nano synthesis like CNT . So scope of income is naturally very high in organic chemistry indeed . But in analytical chemistry the scope is narrow compared to organic chemistry . Since analytical and quality control laboratories are also guided by organic chemists / phyto chemists / petrochemicals for mainly UV-Visible spectrophotometric analysis / Chromatography like GC , HPLC , HPTLC , GC-Mass spectrophotometer and fluroscence spectroscopy .Yes analyical chemists are useful in effluent treatment / waste water analysis as well as drinking water analysis of trace heavy metals like Cu , Cd, As , Pb , Hg ( II , I ) by AAS ( Atomic abs Spectrophotometry ) AES ( Atomic emission spectrophotometry. In drinking / waste water lab there are so many important analytical parameters like B.O.D , C.O.D , D.O , pH , TDS , TSS and limit tests for heavy metals in trace metals .

Dear Ikram Ullah thanks for your kind response. It might also be worth checking the following link which provides access to free books on "Environmental Chemistry":

The following book entitled "Environmental Chemistry Fundamentals" is also freely available as public full text on the internet (please see attached pdf file). I hope that these links will be useful for you.

With best wishes, Frank Edelmann

use lamp

I work as a mineralogist and I am not a specialist in NASICON phases, but the reason that these substances have not yet been found in nature will most likely be the strong hydrating ability and oxygen affinity of Ti and Zr. In even slightly hydrothermal environment there is anatase, resp. zircon (resp. hydrated zircon phases, gelzircon etc.) strongly stable. It is necessary to assess under what conditions, from which input components NASICON are synthesized and whether it is at least a little realistic for a similar synthesis to take place in nature. However, some Zr and Ti phases with PO4 or SiO2 have been found in nature. It is possible to use the search at: https://www.mindat.org/chemsearch.php

Dear Florian and Chen Jingwen unfortunately Alfa Chemistry does not sell quinalizarin either. When you check their website for the term "quinalizarin" you receive a message saying that the product is currently not available (please see attached screenshot).

With best wishes, Frank Edelmann

Extrement important

Dear Muhammad Ali Tariq ,

Would you pleased tell us how do you deposited the Cu2O?

This will benefit much!

Thank you for your positive response!

Best wishes

Dear Cheng Yun Wu many thanks for sharing this very interesting technical question with the RG community. It might be worth a try using acetonitrile to recrystallize your ionic ruthenium complexes. Often such compounds show a good solubilty in hot acetonitrile and form nice crystals upon cooling of the solution to room temperature. Hot water alone might also be worth a try. If your compounds are very soluble in acetone, you could also try a vapor diffusion technique in which you let diethyl ether diffuse into the actone solution. For more potentially useful suggestions please also have a look at the attached guides to growing single crystals.

Good luck with your experiments and best wishes, Frank Edelmann

Hello Harsha,

this is a very good technical question. In the strict sense all simple insoluble silver(I) compounds like AgX ( X = Cl, Br, I), AgCN and AgSCN are coordination polymers. They all consist of polymeric chains in which the silver cations are bridged by the anionic ligands. A traditional application of silver(I) cyanide, AgCN, is its use in silver-plating solutions.

Nowadays, silver coordination compounds are mainly used as antimicrobial / antibacterial agents. This is also true for silver(I) coordination polymers. For typical examples please see the attached Open Access articles. They describe more complicated silver(I) coordination polymers. Please note that there are many more literature references about this topic available.

Good luck with your research and best wishes, Frank Edelmann

Dear Nagapradeep N. that's a really interesting technical question. As an inorganic chemist I'm certainly not a proven expert in this field. In fact, without running a detailed internet search, no such compound immediately come to my mind (at least no naturally occurring ones). For a very good overview on the chemistry of organic phosphonates (including bis- and tris-phosphonates) please have a look at the following useful review article:

This article is freely available as publiic full text on RG.

The situation looks much brighter when it comes to commercially available compounds of this type. For example, please check benzene-1,3,5-tris(phosphonic acid) and benzene-1,3,5-tris(sulfonic acid).

Good luck with your research!

Hello Gideon,

this is certainly a technical question of fundamental importance. In fact, hydrogen chloride (HCl) is a covalent molecule and not an ionic material like NaCl. It is also important not to get hydrogen chloride confused with hydrochloric acid. Pure hydrogen chloride is a gas, while hydrochloric acid (also often described just as HCl) is an aqueous solution of hydrogen chloride. The bonding in the HCl molecule can be described as an overlap of the singly occupied hydrogen 1s orbital with the half filled 3pz​ orbital of chlorine. Thus we have here an s-p overlap. For more information please refer to my courses on inorganic chemistry which are all available as public full texts on RG.

Good luck with your work!

i m work on thisd field

Dear Pejman Rahmani Nejad many thanks for asking this very important technical question, which is certainly of broad general interest to many RG members. I'm afraid that my answer is not what you want to hear, but of course you are absolutely free to ignore it. My initial thought was: Why should an undergraduate student write a scientific article? In my personal opinion (which might be somewhat old-fashioned) the main job of an undergraduate student is to attend lectures, courses, and seminars, collect basic knowledge and pass exams. Especially in your discipline, chemistry, you can only write a scientific article if you have new results to report, and new results can normally be achieved only in the lab (if it is not theoretical chemistry). Moreover, you need to have a supervisor / senior scientist / principal investigator who conceicves the research and acts as corresponding author. Writing of a review article is also not a good idea at the undergraduate stage, as you must be a proven expert in the field covered by the review. Thus, in the end, why don't you just be patient and wait until you worked on an own research project and have sufficient new results to publish?

Good luck and best wishes, Frank Edelmann

Please open the below link of article (https://www.researchgate.net/publication/352830671or http://dx.doi.org/10.13140/RG.2.2.27720.65287) which practically explains the structures of different materials; structural analyses of different materials validate new atomic structures; study further discusses that crystalline materials do not require primitive cells in order to explain the structures and the distance between electronic states is relevant rather than the lattice constant; study reveals the preliminary detail of crystallinity, non-crystallinity, porosity, texture and noise factors along with overall characteristics of peaks; study further categorizes the residual and thermal stresses; shift in peak, hkl values, Miller Indices, planes, d-spacing, Bragg diffraction, Scherrer equation, pdf card are also explained in this study. Overall, the study suggests to re-investigate the materials at all scales. (This article is not peer reviewed yet.)

Dear Nagapradeep N. this is a very interesting technical question. In this context it might be interesting for you to now that thiophenol, C₆H₅SH, has been reported to be extremely stable to thermal decomposition. According to the article cited below, pyrolysis of thiophenol (= benzene thiol) does not start below 500°C:

The chapter has not been posted as public full text on RG, but the Abstract already contains essential information.

Please also have a look at the following potentially useful patent, in which the synthesis of metal sulfide nanocrystals using thiols as precursors has been claimed:

Good luck with your research and please stay safe and healthy!

This Question which interested me a lot, thank you very much

Suggested Readings

Study Hume-Rothery Principe

Generally when the dilute HCL acid reacts with sodium carbonate then sodium chloride, carbon dioxide and water are formed. A brisk effervescence is seen in the release of carbon dioxide.

and as far as the reaction is considered then The excess NaOH is immediately titrated with standard HCl to determine how much HCO3 - was present. From the total alkalinity and bicarbonate concentration, you can calculate the original carbonate concentration.

Dear Gideon Ibekwute I think this is a technical question which can be easily answered by searching the general internet. As typical examples please have a look at the following useful links:

1. Experiment on the analysis of a mixture of carbonate and bicarbonate

and

2. Analysis of a Mixture of Carbonate and Bicarbonate

(see attached pdf file)

In any case the procedure involves two titrations.

Moreover I strongly suggest that you should go to your university library and get hold of a textbook on quantitative chemical analysis.

Good luck! 👍

P.S. What is Mml ? According to the link cited below, "Mml" can mean anything from "Michigan Municipal League" to "Mobile Man Lift":

I think you will get more qualified answers to your technical question when you avoid such lab jargon as already indicated by Paul Milham. 😊

See this link

Dear Arina Levina thanky you again for your interesting technical question. You also asked "I suppose QABs extract REE by anion exchange mechanism." Let me answer with a question: What are "QABs!"?

As mentioned earlier by Thomas Jüstel complexes of the type [LnX₆]^3– (X = Cl, Br, I) are generally kinetically not very stable. To the best of my knowledge they are not readily formed in aqueous solution, but can be prepared through solid-state chemistry or in special organic solvents (e.g. nitriles or nitromethane). Isolation of the hexahalide complexes normally requires the use of organic cations such as pyridinium, tetraethylammonium, or tetraphenylphosphonium cations. One of the most stable and readily isolable hexachloro complexes is the tetravalent cerium complex [pyH]₂[Ce^IVCl₆] (py = pyridine), which is often used as precursor in the synthesis of other tetravalent cerium compounds. For more information about the trivalent lanthanide hexahalide complexes please look for the article entitled "Weak or Unstable Iodo complexes. I. Hexaiodo Complexes of the Lanthanides" published by J. L. Ryan, Inorg. Chem. 1969, 8, 2053-2058. For more general information on lanthanide coordination chemistry try to get hold of the highly recommended book "Lanthanide and Sctinide Chemistry" by Simon Cotton.

Dear Adam da, yes it is possible, but since you are targetting end groups (low concentration) may be the efficiency will be low. Please check the attached files. My Regards

Recrystalisation of a derivative of 2-acetyl gamma butyrolactone, you can try ethyl acetae or acetonitrile.

Greetings Dear Prof. Frank T. Edelmann

Yes, I would love to study in Germany if I can get fund and scholarship

Thanks a lot for sharing this links and information

Kind regards

Dear Pejman Rahmani Nejad thank you for your interesting technical question. In addition to the useful link provided by Lukas Schulig please also have a look at the following relevant article entitled

The paper is freely available as public full text on ResearchGate. According to this article "the most common functional group is the hydroxyl, as its occurrence frequency in all databases is the top one. Moreover, -COOR or -COOH are the second most common functional groups."

I agreed well with dr. Balakrishna Maravanji, gray selenium usually used in synthetic methods in the laboratory.

Dear Gabris Mahamid thank you for this interesting technical question. As an inorganic chemist I'm not really familiar with this topic, but I can try to suggest to you a few potentially useful articles. Please have a look e.g. at the following papers:

1. Can a single molecule trap the electron?

This article can be freely downloaded as pdf file from the general internet.

2. Functional group dependent dissociative electron attachment to simple organic molecules

This article is freely available as public full text on ResearchGate.

Dear Sumit Bhowmick ,

You asked a very broad question, but I hope my answer will undercover the understanding of some of the subquestions =)

Due to DFT is a tool, which operates with small atomic systems up to a couple of hundreds of atoms (you can consider and larger cell up to 400-500 atoms, but you lose in CPU time or accuracy of calculations), you can consider either single-phase atomic structures (solid solution or stoichiometric phase) or supercells with an interface between two different phases.

As for mechanical properties, you can estimate them using special equations, which have bulk moduli of considered phase as input parameters.

Bulk moduli can be easily calculated using DFT.

For example, you can read how I recently did that for Mo-Ni-B-C cermet.

From experimental data and mechanical properties measurements, we obtained that precipitation of κ-phase Mo10Ni3C3B decreases a hardness with increasing of stress intensity factor.

Then we calculated elastic constants of precipitated Mo10Ni3C3B and existed Mo2NiB2 and Mo2C phases and estimated bulk properties and hardness using special equations (See Supplementary https://lettersonmaterials.com/Upload/Journals/32862/boev_et_al_supplementary_material.pdf).

The bulk modulus, shear modulus, Young’s modulus, and Poisson’s ratio were estimated according to Hooke’s law and the Voigt-Reuss-Hill (VRH) model. For hexagonal polycrystalline crystal:

B=[2(C11+C12)+4C13+C33]/9,

G=(C11+C12+2C33−4C13+12C44+12C66)/30,

E=9BG/(3B+G),

ν=(3B−2G)/2(3B+G),

The Vickers hardness (HV) was calculated according to the empirical formula: HV= 2(K^2 G)0.585−3,

K=G/B

So, we obtained that the new Mo10Ni3C3B phase has a lower hardness and is able to decrease the hardness of the whole material.

Ratio B/G is an indicator for ductility properties.

Bond analysis using electron localization functions (provided in VASP) allowed us to define the nature of the bonding in considered phases.

Covalent bonding means stronger hardness and metallic bonding - more ductility/plasticity.

Also, it is important to analyze the anisotropy factors. That will be able to undercover different useful things.

If you have any questions, do not hesitate to ask me =)

The trends are well known, but it is difficult to say in a single sentence, why this trends exist. The following can, however, be stated:

-Mn, Fe, Co deviate from the trend because of the magnetic contribution to the thermodynamic functions.

-the total cohesive energy is much larger than the differences between the energies of the crystal structures. So there are non-obvious subtle effects which are responsible for the energy differences and which determine the observed crystal structures. Some quantitative thoughts can be found in

(quick find by google scholar)

Frank T. Edelmann can you please also answer this question

This question is also related to a relativistic effect in atoms sir.

Today i did some experiment like this. I added a random amount of sulfur and sodium hydroxide in a test tube and aded a drop of water, then i heated until the water was evaporated and the sulfur stopped melting (this produces Na2S + Na2S2O3) . Then once the products were cooled, i added a few mililiters of acetone and rapidly turns into a green solution wich desapears once HCl is added. I think the green color is due to the presence of polysulfides wich forms in adding elemental sulfur (my source of sulfur was the unreacted one)

Dear Frank T. Edelmann

It is sad, but it is true. Your valuable suggestion was not recommended. In contradistinction, the banal response -- Good question --- got one recommendation. I have already seen that such a banal and unjustified response gets 7 or more recommendations. It is happened to me on several occasions Someone says that my post brings very good points. This someone gets 7 or more recommendations, whereas my post gets none. There will be "recommendation teams" ? To put things right, in name of justice and intellectual probity, I decided to recommended your post, not because of you, but because of what it contains.

Could you please not to recommend this my post?

good question

Dear Asim A. Balakit please also see this potentially useful article in which the authors employ the 3,4,5-trihydroxyphenyl substituent in their ligand. The work is entitled

The paper is Open Access and freely available as full text from the general internet.

Dear Gabris Mahamid, the following documents are extremely important in case you want to go deeper in this subject. Also it is nice if you take a look at 'Israelchevilli's book' on intermolecular forces. My Regards

Dear Mahmoud Najm Abid I just came across this potentially useful article entitled

Unfortunately I don't have access to the full text.

P.S. Please find attached an interesting review article entitled

"CLAYS, CLAY MINERALS AND CORDIERITE CERAMICS - A REVIEW"

In this review article "The nomenclature and characteristic structural properties of clays, clay minerals talc, kaolin, vermiculite, ceramic raw materials, cordierite ceramics, cordierite and cordierite polymorphs were summarized.

Mineral phases in clay mixtures and cordierites sintered at 1300°C were compared."

Dear Ayub Khan to the best of my knowledge the book "Selected Topics in Inorganic Chemistry" by Wahid U. Malik, G.D. Tuli, and R.D. Madan. cannot be freely downloaded as pdf from the internet. Why don't you just go over to your university library and ask if you could borrow a copy?

Kamaleldeen Nassar

Common options:

1- Try to increase the basis set gradually. first, preoptimize your system at lower level like PM6 semiempirical method... and later using these results as a guess in subsequent computations.

2- Try to increase the maxcycle number for SCF. For example, scf=(maxcycle=512) option.

2- The SCF=QC option is often helpful (slower, but more reliable algorithm)

Dear Maninder Singh ,

It is possible to analyze unknown phases with Rietveld analysis. Naturally, it is necessary to do a Pawley extraction; It is typically used with powder patterns derived from a crystal structure whose unit cell contents are not or insufficiently known.

In classic Rietveld refinement, each Bragg reflection's intensities are calculated from the atoms' scattering intensities in the unit cell.

By contrast, the Pawley procedure uses the Bragg intensities as freely varying refinement parameters and disregards the underlying atomic structure.

The extracted integrated intensities can, in theory, be used in traditional methods of structure determination.

Pawley refinement of an experimental powder pattern is an essential step before attempting crystal structure determination.

If the lattice parameters and space group are unknown, indexing is necessary to determine possible lattice candidates.

The procedure helps identify the most likely lattices and space group settings corresponding to the experimental pattern.

Once the powder experiment is indexed, it provides the proposed set of lattice parameters' fundamental values for the experimental data.

At this stage, perform refining of the integrated Pawley intensities for exporting the integrated intensities correcting the scale factor and base line contributions of the unknown phase.

These procedures can determine the cell parameters and a bare low symmetric space group for the unknown by observing diffraction peak absences.

Once partially characterized, there are no atoms in the symmetric site description; the known phase is fitted, and the unknown lattice is characterized for further atoms inclusions and association.

In case of a completely unknown phase, some other methods are possible to be applied, such as Patterson's method to extract the heavier atoms positions in the first place and fulfill the asymmetric unit step by step.

Best regards,

WNM

There are a few things to distinguish here, i.e.

1) full equilibrium partitioning among all phases (and making sure that all phases present are really known and not overlooked, for instance because they are very small), considering full thermodynamic equilibration for all of the elements (viz the fast ones such as C, N, H etc and the slow ones such as Mn and Si etc) - this does not happen very often. Most low temperature equilibrium partitioning coefficients are extremely difficult to measure.

2) equilibrium partitioning among phases only for fast diffusers; rest same as above

3) partial equilibrium partitioning only at the interface, but decaying concentrations far away from the interface, due to kinetics.

4) equilibrium partitioning NOT only among the two (or more) phases, but also among the interface itself and the adjacent phases (the interface is a thermodynamic trapping site of its own, due to the adsorption isotherm, and may elements in steel also partition to them (and not only to the phases)).

All of the resulting partitioning coefficients depend substantially on kinetics and composition of course.

Some of them can be obtained directly from multi-component phase diagrams (full equilibrium required, is practically never the case in steels) and some not (kinetics, then u have to use dictra of phase field etc).

In all of these cases exact values for multi-component partitioning coefficients can experimentally usually only be obtained by using atom probe tomography.

Taking partitioning coefficients from the concentration profiles very close across the hetero-interfaces is particularly helpful as the atoms can maintain local equilibrium (equal chem. potential across the interface) with only a few atomic diffus. jumps - when probing far away from the interface partitioning coefficients are usually wrong, due to kinetics.

Good luck.

Here are some references, but this is a wide and really complex field…

some example pictures are also attached, just to give a rough impression

etc

Dear Sumit Bhowmick, you can use the semiclassical and geometrical approach of Lifshitz and Kaganov to explain conductivity in normal metals.

I don't know any related works in ceramics, where the Fermi surfaces can be open. However, there are the so-called molecular conductors.

Electron theory of metals and geometry by M. I. Kaganov and I. M. Lifshits Usp. Fiz. Nauk 129, 487 529 (November 1979)

Can we use potassium dichromate instead of potassium chromate as an indicator for the determination of chlorides in water? please suggest

Dear Dr. Sumit Bhowmick ,

the etching reagents for macroscopic examination or chemical polishing have been under study for many years, as shown by one of the texts most dear to me:

-Smithells Metals Reference Book, Edited by E. A. Brandes and G. B. Brook of which I am attaching the link to the 7th Edition (1992):

Available at: http://pmt.usp.br/academic/martoran/notassolidificacao/Smithells%20Metals%20Reference%20Book%207e.pdf

Smithells is the only single volume work which provides data on all key aspects of metallic materials.

Smithells has been in continuous publication for over 50 years. The 8th Edition represents the major revision:

by William F. Gale, Terry C. Totemeier, Elsevier, (2003) - 2080 pages.

In the metallography part, you can find quite precise indications on the reagents to be used for a specific material. Starting from this base and using the advice in the notes, to obtain an acceptable result it is necessary to make several attempts using different attack times, possible dilutions, etc.

If you have to get a result in a reasonable time, it is not useful to do other tests ....

My best regards, Pierluigi Traverso.

The refractive index of polymers directly related to the polarizability and depends on the wavelength of light.

If a material is structurally isotropic, then it is optically isotropic, and a single refractive index typifies the refraction behavior.

In crystals and anisotropic materials, the refractive index takes different values along different principal axes, and the material is said to be doubly refracting.

The molecular weight of polymers affects their refractive index, but its effect is not significant. In some polymers, as the molecular weight increases, the refractive index increases. For example, for Poly(ethylene oxides), when the molecular weight change from 303 to 9523, the refractive index increases 0.8% (from 1.44592 to 1.45392). While, for polycarbonate, as the molecular weight increases (from 228 to 7196), the refractive index decreases 0.95% (from 1.6021 to 1.5868).

As a result, the relation between refractive index and structural and physical properties is complicated.

I have attached one text about refractive index of polymers. I hope it would be useful.

HI,

The two software options I would suggest are Gaussian and Hyperchem. Both are usable for calculations. Gaussian is the much bigger name but both are usable for building structures and so much more. Hyperchem should be something you could get cheaper. There are some other software's out there that I have heard of but not had exposure to. That said their are some SW that are "free" but I am not sure how easy they are to work with. Also, if you can find some similar files that are close to what you want, it might be worth trying to get a copy and modify to your needs.

Frank T. Edelmann Melchior Menzel Ifiok Ekwere , thank you very much. It helped me a lot.

Srividya Swaminathan d-d transitions are symmetry forbidden (Laporte selection rule), and therefore less intense. MLCT (or any charge transfer) transitions are far more intense. Typically, molar extinction coefficients for d-d transitions are in the range of 200-500 M-1 cm-1 whereas that for the MLCTs is >1000 M-1cm-1.

Hello,

In general, no. Pt(II) likes to be square planar. There are some examples of 5-coordinate Pt(II). Also, you can have Pt(II) with hydrogen bonding to the open sites above and below the square plane, but that's not technically ligand coordination.

Sincerely,

Kyle

Hlw good day I want to make DES choline cholride +MAA with molar ratio 1:2 can any one share the precise calculation for these moaor ratio..thanks

Almost all ligands are sigma donor, though the extent of donation varies from ligand to ligand. Now the question is when a ligand will act as a pi acceptor or donor. Pi donor ligands are those which have extra non bonding electrons in their valence orbitals (simple example iodine). Now the extent of pi donation depends on the symmetry and energy of those orbitals. The energy difference between vacant metal orbitals and filled ligand orbitals should not be very high and both must have same symmetry. Now to be a pi acceptor a ligand needs to have an empty orbital and here too the extent of pi accepting tendency depends on the energy difference and symmetry of the empty ligand orbital and filled metal orbital.

ref: The Organometallic Chemistry of the Transition Metals by Robert H. Crabtree

Copper(I) thiocyanate, CuSCN, is a white powder when pure, but often the material of commerce is yellow. It is soluble in ammonia solution, alkali thiocyanate solutions, and diethyl ether, but it is only slightly soluble in water and dilute mineral acids. It is stable in air in the absence of moisture, but it slowly decomposes in the presence of moisture in air.

It seems that the sample has a very low background profile than that of control. It might be caused by the incorrect white background reference. Have you measured it several times? You can measure both samples at the same time

Mostly pH is affected.

In addition to all interesting answers in this thread Prof. Magnus Schlösser .

I will add 2 classical references for triplet superconductivity, also called unconventional superconductivity: