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Showing posts with label safety. Show all posts
Showing posts with label safety. Show all posts

Thursday, 17 August 2023

Advanced Manufacturing Ideas Can Be Applied to Fine Chemicals/ Pharmaceuticals

 


In their August 12th, 2023 issue pg. 63-64, the Economist magazine describes the advanced manufacturing of first, computer chips and then, cordless electric drills. Reading this brief report suggested to KiloMentor possible parallels with future advances in the scale-up for the manufacturing of complex organic chemicals.


The article points out that “chips are designed using software that directly links to the automated hardware which fabricates them.” The efficiencies that this unlocks derive from the consequence that “the constraints of the production line- even fiddly details like the positioning of screws— are encoded in their CAD (computer-aided design) programs.”


Well, how does this have any analog implications for chemical processes for making sophisticated chemicals? We don’t have automated production facilities and we don’t work out the details of process steps in computer programs.


The research laboratory functions as our design tool and the pilot plant functions as our automated fabrication hardware and our problem is too often that our designing is not sufficiently linked to our manufacturing. The problem is how do “even [these] fiddly details”, like the constraints of large-scale production get signalled back to the laboratory before valuable time is wasted?


In advanced manufacturing, these constraints are wired into computer-aided design programs. For our projects, there are two possibilities. Either our process design chemists must have these limitations wired into their chemical know-how or the whole company must adopt some form of what has been termed ‘full process vision’. I have written previously about this idea in the blog, Avoiding the Screw-up from Left Field with a Full Process Vision.


Since it is difficult to impossible to find this article I have reprinted it below.


"Some process chemists will find themselves as small cogs in large teams whose goal is to develop new specialty chemicals or pharmaceuticals.  As a scientist whose contribution is to apply highly specialized knowledge, you may be bunkered in a rather isolated trench or silo within your organization. Your mission may be defined for you rather narrowly so your undoing may come from an irrefragable requirement that comes from outside your silo and that is imposed so late in your work plan that it really means starting over.    

A powerful organizing structure for pharmaceutical product development is presented in an article by Pradir K. Basu, Ronald A Mack, and Jonathan M. Vinson, “Consider a New Approach to Pharmaceutical Process Development“ Chem. Eng. Prog., 95(8), 82 (1999).  It seems intended to reduce the likelihood of the above misfortunes.  

Process chemists, as knowledge managers, need to press at an early stage in their work for some mechanism within the wider team so that these must-have ‘requests’ from outside your core group reach you before your work is too far advanced. 

Much of the referenced article presents no more than standard reminders of the importance of cost considerations throughout discovering a synthetic method, scaling it up, and putting it into production for a process to manufacture a new pharmaceutical. This is the pharmaceutical business with the marketing, selling, and regulatory functions stripped away. Its importance to corporate profitability does not engender much debate. The importance of the article is that their concern is broader. 

The authors are concerned about the efficient execution of a plan that starts after identifying a candidate to be a commercial drug with a salutary effect on a biological target and proceeds to the validation of manufacture for that molecule at a commercial scale. 

The enhanced approach that they propose identifies what they call ‘process vision’ as the core organizing principle. The definition and exemplification of the expanded concept of ‘process vision’ is the article’s significant accomplishment. 

The authors help us understand different aspects of this 'process vision' at different points in the article. For me, I cannot say I adequately grasped what they were getting at until I drew particular phrases together from my notes. Some of these quotes, drawn from different parts of the essay are: 

 “The process vision satisfies all essential requirements, including those for safety, quality, waste minimization, cost, time, and operability”. 

“The process vision is neither the process with maximum yield nor the one that gives maximum product purity…..it is neither a chemist’s vision nor an engineer’s vision; it is not even the vision of the chemists and engineers together.” 

“It is a vision that all stakeholders in development, manufacturing, and marketing can share…..” 


Reading between the lines and amplifying certain aspects, the process vision emerged as a policy statement that provided, as a starting point, standards by which team members coming from each stage of the organization's endeavor (laboratory process, kilo lab, pilot plant, and manufacturing facility) could satisfy downstream colleagues’ concerns from the outset of their own work. The authors' specific examples of the unique orientation and emphasis that players at the different stages have and which they want to see addressed from the very outset reinforce my interpretation. 

This early overview, whose importance they emphasize, can be expected to show up inevitable cross purposes and improve the odds for early compromise and conflict resolution. 

They write:

 “Chemists think in terms of steps, reactions, yield, purity, and so on; engineers in terms of unit operations, physical properties, heat load, and the like; manufacturing personnel in terms of throughput, waste control issues, and plant modifications that may be required to run a process; and marketing people in terms of the net present value of the product, how much it can sell for, etc.” 

“It is important ….to get stakeholders to develop….agreed-upon objectives of process development.” 

“communication among….personnel is critical during process development.” 

“We need to…. provid[e] development team members with systems or tools to facilitate communications among different disciplines.”

“Unless the manufacturing team is involved in the process development, they will not have confidence in the scale-up”. 

“…manufacturing and commercial input at this stage [late stage discovery] are essential for choosing the optimum processing route”. 

“Team members need to be involved in setting targets for cost, manufacturability, waste and emission loads, development time….” 

“These alternatives must be evaluated based on….criteria agreed upon by all stakeholders….” 

“If stakeholders are involved in planning experiments, it’s likely that more useful data could be collected from fewer experiments.” 

For me, the management tool the authors recommend for achieving this widely held ‘process vision' is Panglossian. 

The authors propose that even at the experimental program level one should try to bring together a diverse project team including representatives all the way out to marketing, frequently enough to work out priorities and make decisions. This is what they recommend. 

This seems excessively optimistic as regards human nature. Instead, I suggest, one could establish a 'process vision' statement establishing some sort of median or normal starting-point performance criteria that would address recurring diverse concerns of process development, manufacturing, regulatory affairs, and marketing and that would chevvy the most common interests of the downstream project teams on the upstream collaborators. In this implementation, the process vision would be via a statement delivered with full corporate authority that would continuously challenge upstream groups with the standard core concerns of the downstream members. 

The authors illustrate marvelously this challenging interaction throughout their article. What I interpret them to be saying is that the problem is not that different elements of the project team have concerns that inevitably seem to operate at cross purposes; but that the team members can reach solutions that satisfy all parties, so long as the areas of tension are discovered early enough. 

KiloMentor has a strong preference for its alternative. The use of a process vision statement as a proxy for the perspectives and concerns of downstream project groups seems preferable to using large frequent group meetings to actually direct even the collection of particular data. For a company’s drug product projects to be successful and on time, any process’s strategy must not conflict too greatly with the psychological needs and private professional goals of the individual team members. The people downstream in the project, whether they be in late-stage process development, manufacturing, or marketing, simply will not give a project the attention it needs until it arrives at the phase where they are being held singly and personally responsible. They are too busy concentrating their attention on what is on their plate already and extinguishing the fat that is already on fire. This is human nature! Besides, pharmaceutical product projects can go on so long that some participants can realistically expect to no longer be involved when a late-stage discovery project limps into manufacturing or marketing. People may hope or plan to outrun the difficulties. Only unambiguous corporate endorsement can get everyone to give a thought to early-stage projects.

Equally problematically, the upstream professionals, working at a particular phase of the work on their own turf, would require an uncommon personal modestly to accept without rancor face-to-face demands that particular questions be answered on a priority basis. 


A corporate ‘process vision’ statement takes the personalities and egos out. At the same time, the standards proposed by a process vision statement would command authority and yet not be carved in stone. They would exist to bring a persistent awareness of particular concerns. They would bring those different needs, which may be pulling at cross purposes to early attention, and they can be expected to bring the affected team members together as needed to create or negotiate a solution." 


Wednesday, 31 March 2021

Reaction Addition Modes: Controlling Chemical Reaction Stoichiometries

 



  A + B  Gives C + D


Most chemical reactions are either unimolecular or bimolecular in their kinetics. They are either addition/condensations where there is only one product, ie C and no D, or in other instances, some transformation also provides a coproduct, D, created along with C.


Reactions proceed when the energy supplied to a system is appropriate for the free energy of the reaction. More energy being supplied to the system can cause the reaction to proceed faster and/or it can promote alternative transformations that compete with the desired one. Applying excess energy for longer than necessary can degrade any of A, B, C, or D.


If any of the reactions


 C + (A or B) gives (E or H)

or 

A + A gives F  

or

B+ B gives G


can occur, then having the correct stoichiometry present throughout the time when the system experiences the required activation energy becomes important. If the stoichiometry is wrong then starting reactant polymerizations or overreaction modes can compete to the detriment of the desired outcome. A procedure that keeps the reactants in the correct stoichiometry throughout that period when adequate activation energy is supplied is likely to give a cleaner reaction.


Standard Chemical Processing


Now in the standard mixing procedure, a solution either of reactant A or B is added slowly to a solution of the complete charge of B or A already stirring in the reactor. If the reaction proceeds so quickly that it overheats, the addition is slowed or stopped allowing the rate of reaction to slow down as the reactant being added gets consumed and no more is being added. That is, the reaction is prevented from running out of control by letting the stoichiometry inside the reactor change radically. To control an exotherm the operators in such instances are forced to let the concentration of the reactant being added into the vessel fall towards zero.


For greater clarity and to emphasize the necessary safety issue let us perform the thought experiment of mixing all of the charge of these same A and B in methylene chloride and starting to heat the reactor. When the reaction between A and B sets in, the methylene chloride will start to reflux but as the temperature rises towards the boiling point of the methylene chloride the reaction between them goes faster and faster. The methylene chloride now boils faster than it can be condensed and gaseous methylene chloride blows liquid methylene chloride and all the rest of the reactor’s content out of the reactor and probably onto the roof of the plant building!


Identifying Reactions that Could be Affected by Stoichiometry


The standard mixing procedure is unlikely to be adversely affected by the ‘in situ’ stoichiometry if the reaction rates of all steps occurring in the reactor are slow compared to the addition time. This is easily determined. When one-half of the addition of the controlling reactant has been added, an in-process check should be done. If either the product or any reaction intermediates are significant compared with unreacted starting materials then the transformation is likely to be sensitive to the reaction’s stoichiometry. If nothing significant besides unreacted starting materials (or substances produced during the quenching of the reaction before analysis) are present, then it is very unlikely that the yield will be affected by stoichiometry. When hardly any change can be detected in this test it indicates that almost the reacting occurs mainly after the reactant being added is completely in the reactor and the stoichiometry is therefore essentially fixed throughout the actual reacting period.


Importance of the Enthalpy of Reaction Calculation


If you are going to perform experiments in which all the reactants are mixed together at once, you must take appropriate precautions. 

You must do a calculation of the enthalpy of reaction based on standard bond energies; however, the enthalpy of reaction (H) is only a crude approximation to the free energy of reaction (F) since F = H - TS. The change in entropy of the reaction (S) also contributes to the reaction’s driving force. For example, if the reaction leads to more moles of products than the moles of reactants, the entropy change is most likely going to be positive and the overall free energy decidedly more negative because of (-TS). The reaction will be faster than the approximation.  It will be necessary to absorb the net free energy of reaction through the agency of first- the temperature rise of the reactor contents ( mostly solvent),  then the energy absorbed in vaporizing some part of the reaction solvent, and finally by the energy drained off by the refluxing of a part of the solvent.


Absolute Necessity for Small Scale Trials in a Laboratory Fume Hood


Theory is just theory. If you are going to perform a reaction in which all the reactants are to be mixed together and then reaction initiated (either by heat or catalyst), you must try out the method at a scale where even if you have miscalculated there will be no more than a mess to clean up, not a laboratory disaster! The reaction which you have examined might not even be the reaction that occurs. Something much more energetic could surprise you.


Get Emergency Control Means Ready


Of course, your reaction vessel must be equipped with a means to directly in real-time read the internal temperature. Otherwise, you won’t be alerted soon enough that you have a problem.


If despite your calculations the temperature of the reactor accelerates in an unexpected way you want to be prepared to intervene to slow things down. Having a cold -bath ready into which the reactor flask can be plunged often can tame a reaction that is misbehaving. The advantage of this form of moderation is that it can be removed when the danger passes and the experiment continued.


Some reactions need to be quenched by injection. In many cases that quench material can be as simple as water. Of course, such an experiment is wasted but a runaway condition is avoided. 


When a runaway reaction is the least bit possible, the experimentalist should both wear appropriate personal protective equipment and have a fire extinguisher handy. It is important to prepare by imagining what might happen. For example, are there other chemicals in the hood you will be using that could exacerbate your runaway? 


Well then—can we actually mix reactants A and B together safely so that the correct stoichiometric is maintained at all times and a runaway exotherm is prevented?


 Two Simultaneous but Separate Additions


Simple in concept but mechanically difficult would describe the simultaneous addition to one reactor of two separate solutions, one carrying the A reactant and the other carrying the B reactant. The two addition rates of each need to be controlled so that the same required molar amount of each reactant is delivered throughout the addition time. If unwanted exothermicity occurs in the reactor both reactant streams need to be slowed the same amount or stopped simultaneously. Technically this is a big ask and practically it will only be approximately successful but even if it is only achieved approximately it can provide a closer approximation to constant ideal stoichiometry. This method of reactant addition, even if performed somewhat imperfectly, can give the experimentalist an indication of whether getting better stoichiometry using a different but more practical method is likely to deliver a useful benefit.


Storage Solvent and Reaction Solvent Method


Both reactants can be dissolved together completely in a volatile solvent (storage solvent) at a temperature and concentration at which reaction will not proceed and that solution can be added in a controlled fashion to a higher boiling solvent (reaction solvent) preheated to below its own bp. but above the bp. of the addition solvent so that the storage solvent will flash distill as it is added and the reaction between A and B will occur at the set stoichiometry in the reaction solvent solution.


Flow System Method


A continuous flow system may be possible where the reactants are bled separately but in the proper stoichiometry into a heated reaction zone and the product is continuously removed from the reaction zone. The problem with the flow technique is that for many reactions operating at the lowest normal reaction temperature, the heated zone would be quite long. Such specially configured equipment is not typically available. This can be solved by operating at a higher temperature in a higher boiling solvent treated in the reaction zone near the higher boiling point of this alternative solvent. 


For example, suppose it is known that A will react with B in refluxing dichloromethane and the reaction is essentially complete in three hours. The same reaction however might proceed equally cleanly in hot propylene carbonate in one minute. Then mixing two solutions one of A and the other of B; each dissolved in hot propylene carbonate so that a correct stoichiometric ratio and delivering it into the hot reaction zone in a flow reactor so that the transition of material through that zone was one minute could produce C more cleanly than heating much longer in dichloromethane because the correct stoichiometry has been more faithfully observed and the reaction period is very abbreviated.  If the reaction time is lessened, the reaction zone length can be shortened and some standard equipment may suffice. Now, whether creating the advantage of having the correct stoichiometry throughout the reaction period outweighs the disadvantage of applying more energy to the system than is actually required to get reaction can only be answered by experiment.


Reactants- All-In Method


Another means to achieve the same result would be to mix the correct stoichiometric quantities of A and B in the bottom of a reactor and then add a high-boiling solvent to it; in our example above this would be the propylene carbonate. The reactor is then heated to start the reaction. Normally mixing all of the reactants together and then heating to start their reaction is never done at scale because, as already pointed out, the exothermicity of the reaction is likely to cause a runaway wherein the entire contents of the reactor including any solvent would overheat and potentially even explode; however, using a sufficient quantity of a high-boiling solvent with a significant heat capacity and large enough heat of vaporization will allow any exothermicity to be absorbed first by the heating of the high-boiling solvent and subsequently by the heat of vaporization (refluxing) of a small portion of this solvent.


Using High-Boiling Solvents to Control Exothermic Reactions


The advantage to using a high-boiling solvent for such a reaction is not primarily its ability to dissolve the reactants and bring them together homogeneously. Good low-boiling solvents can do that. The high-boiling solvent can use its higher heat-of-vaporization, as well as its heat capacity, as a heat sink to soak up the exothermicity of the reaction.


In fact, the high-boiling liquid in which the reaction is being conducted does not need to be able to dissolve the reactants for it to be effective as a heat sink. So long as the reactants can blend together without solvation help the liquid medium does not have to dissolve them. Reactions ‘on-water’ for example are of this type. If at least one of the reactants is itself liquid there will be a reduced need for a dissolving type solvent. Another purpose for using a high-boiling liquid medium in which the reactants are insoluble is to provide sufficient bulk volume to satisfy the minimum stirrable volume requirement for the reactor.


Sunday, 12 August 2018

The Relationship between the Risk of Catastrophic Failure and the Size of the Scale Up Steps in Chemical Process Development



What do I Mean by Catastrophic Failure?


In the context used herein, I am defining a catastrophic failure of a process step trial as a very large loss of product quality and/or isolated yield from which there is no recovery. That is, by definition, there is no patch known and reprocessing is not viable. Characteristically, the failure, when it occurs, comes as a complete surprise. Catastrophic failures at scale usually create serious financial losses and make project schedule extension necessary. It is the risk we face when we ‘put too many eggs in one basket’.

How is the Size of the Scale Up linked to the Risk of Catastrophic  Failure?


What is risked when a process step is increased in scale? It is fair l widely accepted that at first and quite normally, for any reaction step the yield is likely to fall somewhat. More serious, but still not unexpected, is that the type and quantity of impurities in the isolated product may change in unanticipated ways. Worse still and getting to the catastrophic, the reaction may create a mixture that cannot be purified enough to give an isolable physical form. Still worse, the reactor contents may become unprocessible (can’t cut, can’t stir, can’t cool, can’t filter can’t distil). When these latter things, for which there has been no preparation occur, unacceptable time and money is lost. More material must be ordered. The project milestone are missed. These possibilities limit the size of the scale up steps in development. Consequently, as the cost of the inputs at risk and/or the probability of catastrophic failure fall, the size of the steps in scale up can increase.
The approximately optimal conditions determined with laboratory equipment can still be quite different with respect to a  number of variables from what must be done in a pilot plant. Just for starters, some parameters such as heating, cooling, stirring and the times for reagent additions most often cannot be physically matched after increasing scale because of  equipment limitations. Surprises can occur as one increases the  size of operations and these lead to product with unacceptable properties.

How does One Rank Risks?


Any risk to workers’ physical safety must be made inconsequential. It would be immoral to knowingly add to risks to health and safety. Even from a completely selfish perspective, a lost time industrial accident can put a chemist manager’s professional career at risk. Safety issues are paramount and signs of a hazard dictate slow scaling.
A loss of starting material is both a loss of time and of money. The budget can perhaps be repaired but the time required for the delivery and qualification of  fresh starting materials is lost forever. If the inputs are inexpensive as a proportion of total costs and are quickly available from multiple sources, one risk of more aggressive scaling is reduced. It is usually the early steps in a process where inputs can be replaced cheaply and quickly and other things being approximately equal, early steps can be scaled up in larger increments for that reason.

Can One Estimate the Likelihood of a Particular Type of Scale-Up Failure?


Perhaps we ought to ask instead: How well am I able to  scale down the pilot plant environment and reproduce it in my laboratory equipment? Scaling down is the exercise of selecting the bench-scale equipment, operating conditions, and mathematical models to successfully simulate pilot or production scale operations in the lab.
Risk can be reduced by testing with such equipment. If the experimentation has been conducted using exactly the same quality for solvents, reagents, processing aids and catalysts, the biggest sources of deviation in scale-up are removed. If the processing times including times of addition, times for transfers, and time for filtrations approximate those necessitated in the pilot plant, risk is reduced. If the corrosiveness and abrasiveness of the reactants have been tested on the reactor’s materials of construction, it reduces risk. If the procedure is insensitive to rate over a wide range of agitation speeds then another sensitivity has been allowed for. If the sensitivity to traces of air and moisture is known and taken into consideration, life is simplified. If none of the reactants reagents or coproducts in the process step are more completely swept out of the reactor at one scale compared to the other, another frequent source of deviation is accounted for.
There are auguries of danger that can be divined while still in the laboratory and addressed before moving to higher scale:
·        Addition or removal of a gas
·        High viscosity of the reaction medium
·        High exothermicity
·        Need for a low reaction temperature
·        Drown out quenching
·        Rapid addition rates
·        Fast reaction relative to the rate of addition of a reacting component
·        Decomposition on the reactor walls
·        Presence of byproduct polymer
·        Use of polymer reagents that may disintegrate with stirring
·        High speed stirring
·        Asymmetric synthesis catalysis

When one scales up, it is advantageous if the first step is of sufficient size that all the changes in the main discontinuous variables (reactor materials, reactor shape, minimal stirrable volume, type of agitation, heat transfer etc.) are introduced together. Making these changes together often can be better accommodated by also including initially an increase in the amount of solvent in the reactor, to give an overall dilution. Often the biggest risk impediment to moving into the pilot plant is the cost of materials to operate at the minimum stirrable volume in the larger reactor. Making an initial dilution that can later we reversed, may set up a more acceptable combination of risks at a more acceptable price.

Said another way, it may be better to delay the optimization of the throughput, which is very often the result of the consequence of increasing the concentration of the reactants and reducing the amount of diluents (ie solvent) until after  the transition to the pilot plant or manufacturing equipment. This will result in a less expensive transition from laboratory to pilot plant. It will require less of the expensive chemical to reach the minimum stirrable volume at the start of the reaction.

Catalyst poisoning will be treated in a separate article.

Balancing Chemical Equations and Calculating Heats of Reaction: Two Often Overlooked Helps for Chemical Process Developers.




Many years ago, when I was a graduate student with Professor R.B. Woodward, at a group party at Harvard University, my wife asked Woodward, who was arguably the finest synthetic organic chemist in the world, what kept him modest. Although the question was expressed with a fair measure of pique, Dr. Woodward did not seem flustered.  He replied something to the effect that Nature itself did this, since even the most accomplished chemist more often proposes what turns out to be unsuccessful than what is successful.

How true. How true. But even so in our false sophistication we often fail to take simple precautions, which would easily avoid silly errors. I would like to speak of two of these:

·        failing to balance the chemical equation, and
·        failing  to calculate the enthalpy change in a reaction using simple bond energies

Balancing the Chemical Equation


Inorganic chemists rarely show this delinquency but organic chemists, because they are so accustomed to writing a starting material, a reagent and a product as part of a proposed series of reactions, almost never balance equations.  The result is that more often than you would expect even experienced lab workers do not get the stoichiometry correct and add either an excess or a deficiency of a reagent.  This is particularly true of oxidation reactions.  The second difficulty that results is that they cannot see the importance of the coproduct, which is formed along with their desired product, because the coproduct only ecomes import when one tries to balance and so they cannot see the possibilities and the complications that may arise from its presence. 

Calculating the Enthalpy of the Reaction


We organic chemists often seem to have gotten it into our heads that so long as we can draw a self-consistent series of arrows, showing the movement of electron pairs, then a reaction has a reasonable possibility to proceed. Usually we are protected from error by the fact that the transformation we are contemplating is completely analogous to a known reaction.  Nevertheless, it is a simple matter using bond energy tables to calculate the net enthalpy change of the reaction we are hoping will occur.  The result is that it will become more apparent to us whether a desired reaction is just weakly favored (so that steric hindrance, inadequate solvation etc. can inhibit it), disfavored or so strongly favored that we need to be concerned about the exothermicitry of the process and take appropriate precautions.

To be sure, it is negative free energy not a negative enthalpy, which is necessary to have a favorable equilibrium. but it is the less common situation when the entropy of the reaction makes the difference in driving the reaction and when it does, this is almost always when gases are involved or when the reaction is a fragmentation.

To make simpler the calculation of Enthalpy of Reaction, I have gathered together typical bond energies for the covalency between different atoms listed them below.  These should be treated as median or average values.  You may be able by inspection of the substrate or the reagent you intend to employ to recognize bonds, which can be expected to be stronger or weaker than these representative values.

Bond
Value
Bond
Value
Bond
Value
F-C
108
O-H
110-111
N≡C
212.6
F-F
37
O-C
85-91
N≡N
225.8
F-H
135
O=C
173-181
N-Si
76.5
F-O
45
O-O
35
P-P
41
F-C
108-116
O-N
53
P-C
65
F-Si
193
O=N
145
P-H
76
Cl-Cl
58
O-Cl
52
Si-Si
81
Cl-Br

O-Br
48
Si-C
77
Cl-I

O-P
91
Si-H
94
Cl-S

O=P
119-130
C-H
98.7
Cl-N
46
O-Si
111
C-H (vinyl)
108
Cl-P

O-I
56
C-H(acetylene)
128
Cl-C
81
O=S
132
C-C
82.6
Cl-Si
113
S-H
88
C=C
145.8
Cl-H
103.2
S-S
54
C≡C
199.6
Br-Br
46.1
S-C
60


Br-I

S-Si
70


Br-P

S=C
128


Br-S

N-N
39


Br-N

N=N
100


Br-Si
97
N-H
93.4


Br-C
66
N-C
72.8


I-I
36.1
N=C
147