Wednesday, 25 December 2013

Why sugar is sweet ?


The human tongue responds to a range of different substances, registering them as various tastes. Evolution programmed our gustatory sense to find nutritious things tasty, and un-nutritious things un-tasty — for the most part. Human beings are flexible about what they eat relative to many animals, hence our omnivore status, but there are many types of organic material that we are incapable of digesting, and hence perceive as unpleasant. Sugar is highly digestible and offers a very condensed source of calories, so to us it tastes good — and has a distinct flavor that we label sweet. All mammals, except cats, can taste and enjoy this substance and are more inclined to eat poor-tasting food if it contains some.
Scientists now know that the tongue is covered with tiny clusters of chemical sensors called taste buds. It is the geometric shape of incoming molecules that determines how they taste. Some foods have multiple molecules that all contribute to their overall taste sensation. There are several types of sugar that exist, but by far the most frequently consumed by humans is a molecule called sucrose. There are also other molecules, like saccharine, that taste sweet even though they aren't sugar, although the taste sensation is slightly different.


Sunday, 8 September 2013

Notes on MOEL diagrams of octahedral,tetrahedral and square planer complexes involving sigma and pi bonding

MOEL diagram for a square planer complex

MOEL diagrams for octahedral,tetragonal and square planer complexes

Reactions of RMgX and RLi with esters



Reactions of RLi and RMgX with Esters
reaction of RLi or RMgX with esters 
Reaction usually in Et2O followed by H3O+ work-up
Reaction type:  Nucleophilic Acyl Substitution then Nucleophilic Addition
Summary:
  • Carboxylic esters, R'CO2R'', react with 2 equivalents of organolithium or Grignard reagents to give tertiary alcohols.
  • The tertiary alcohol contains 2 identical alkyl groups (see R)
  • The reaction proceeds via a ketone intermediate which then reacts with the second equivalent of the organometallic reagent.
  • Since the ketone is more reactive than the ester, the reaction cannot be used as a preparation of ketones.
REACTION OF RLi or RMgX WITH AN ESTER

Step 1:
The nucleophilic C in the organometallic reagent adds to the electrophilic C in the polar carbonyl group of the ester. Electrons from the C=O move to the electronegative O creating an intermediate metal alkoxide complex.
addition of Grignard reagent to an ester
Step 2:
The tetrahedral intermediate collapses and displaces the alcohol portion of the ester as a leaving group, this produces a ketone as an intermediate.
Step 3:
The nucleophilic C in the organometallic reagent adds to the electrophilic C in the polar carbonyl group of the ketone. Electrons from the C=O move to the electronegative O creating an intermediate metal alkoxide complex.
Step 4:
This is the  work-up step, a simple acid/base reaction. Protonation of the alkoxide oxygen creates the alcohol product from the intermediate complex.


Oxymercuration-demercuration of alkenes



Oxymercuration-Demercuration of Alkenes
alkene alkoxymercuration-demercuration to give an alcohol
Reaction type:  Electrophilic Addition
Summary
  • Overall transformation C=C to H-C-C-OH
  • This is an alternative method for hydrating alkenes to give alcohols
  • Typical reagents are mercury acetate, Hg(OAc)2 in aqueous THF
  • Unfortunately, mercury compounds are generally quite toxic
  • Regioselectivity predicted by Markovnikov's rule (most highly substituted alcohol)
  • The reaction is not stereoselective
  • Reaction proceeds via the formation of a cyclic mercurinium ion (compare with bromination of alkenes)
a mercurinium ion
  • The mercurinium ion is opened by the attack of water to complete the oxymercuration.
  • When the water attacks, it does so at the more highly substituted carbon.
  • Demercuration is effected by a reduction using sodium borohydride, NaBH4
  • If the reaction is carried out in the presence of an alcohol rather than water, then ethers are obtained via an alkoxymercuration :
alkoxymercuration-demercuration to give an ether
  • The only difference here is a change in the nucleophile from H2O to ROH

MECHANISM FOR REACTION OF ALKENES WITH Hg(OAc)2 / H2O
Step 1:
The C=C π electrons act as the nucleophile with the electrophilic Hg and loss of an acetate ion as a leaving group, forming the mercurinium ion.
oxymercuration / demercuration of C=C
Step 2:
Water functions as a nucleophile and attacks one of the carbons substituted with mercury resulting in cleavage of the C-Hg bond.
Step 3:
The acetate ion functions as a base deprotonating the oxonium ion to give the alcohol. This completes the oxymercurationpart of the reaction.
Step 4:(mechanism not shown)
The hydride reduces the Hg off, creating aC-H bond while breaking the C-Hg bond. This is the demercuration part of the process.

Simmons Smith reaction,formation of cycloalkanes


Synthesis of Cyclopropanes using RZnX (The Simmons-Smith reaction)
Cyclopropanation using the Simmons-Smith reaction
Reaction type:  1.  Oxidation-Reduction,  2.   Addition
Summary
  • This is the most important reaction involving an organozinc reagent.
  • Also known as the Simmons-Smith reaction
  • The iodomethyl zinc iodide is usually prepared using Zn activated with Cu.
  • The iodomethyl zinc iodide reacts with an alkene to give a cyclopropane.
  • The reaction is stereospecific with respect to to the alkene (mechanism is concerted).

  • Substituents that are trans in the alkene are trans in the cyclopropane etc.
Simmons-Smith reaction is stereospecific
Related reactions
 
MECHANISM OF THE SIMMONS-SMITH REACTION
Step 1:
A concerted reaction : both new C-C are formed simultaneously. Best viewed as the nucleophilic C=C causing loss of the iodide leaving group and the electrons from the nucleophilic C-Zn bond being used to form the other C-C bond.
cycloaddition mechanism of the Simmons-Smith
 

Reactions of RMgX and RLi with aldehydes and ketones



Reactions of RLi and RMgX with Aldehydes and Ketones

reaction of RLi or RMgX with aldehydes and ketones 
Reactions usually in Et2O or THF followed by H3O+ work-ups
Reaction type:  Nucleophilic Addition
Summary
  • Organolithium or Grignard reagents react with the carbonyl group, C=O, in aldehydes or ketones to give alcohols.
  • The substituents on the carbonyl dictate the nature of the product alcohol.
  • Addition to methanal (formaldehyde) gives primary alcohols.
  • Addition to other aldehydes gives secondary alcohols.
  • Addition to ketones gives tertiary alcohols.
  • The acidic work-up converts an intermediate metal alkoxide salt into the desired alcohol via a simple acid base reaction.
NUCLEOPHILIC ADDITION OF RLi or RMgX TO AN ALDEHYDE
Step 1:
The nucleophilic C in the organometallic reagent adds to the electrophilic C in the polar carbonyl group, electrons from theC=O move to the electronegative O creating an intermediate metal alkoxide complex.
addition of Grignard reagent to an aldehyde
Step 2:
This is the  work-up step, a simple acid/base reaction. Protonation of the alkoxide oxygen creates the alcohol product from the intermediate complex.

Organocatalysis in synthesis


Organocatalysis

Organocatalysis uses small organic molecules predominantly composed of C, H, O, N, S and P to accelerate chemical reactions. The advantages of organocatalysts include their lack of sensitivity to moisture and oxygen, their ready availability, low cost, and low toxicity, which confers a huge direct benefit in the production of pharmaceutical intermediates when compared with (transition) metal catalysts.
In the example of the Knoevenagel Condensation, it is believed that piperidine forms a reactive iminium ion intermediate with the carbonyl compound:
Another organocatalyst is DMAP, which acts as an acyl transfer agent:
Thiazolium salts are versatile umpolung reagents (acyl anion equivalents), for example finding application in the Stetter Reaction:
All of these organocatalysts are able to form temporary covalent bonds. Other catalysts can form H-bonds, or engage in pi-stacking and ion pair interactions (phase transfer catalysts). Catalysts may be specially designed for a specific task - for example, facilitating enantioselective conversions.
An early example of an enantioselective Stetter Reaction is shown below: :
D. Enders, K. Breuer, J. Runsink, Helv. Chim. Acta1996, 79, 1899-1902.

model explaining the facial selectivity
Enantioselective Michael Addition using phase transfer catalysis:
T. Ooi, D. Ohara, K. Fukumoto, K. Maruoka, Org. Lett.200573195-3197.

The first enantioselective organocatalytic reactions had already been described at the beginning of the 20th century, and some astonishing, selective reactions such as the proline-catalyzed synthesis of optically active steroid partial structures by Hajos, Parrish, Eder, Sauer and Wiechert had been reported in 1971 (Z. G. Hajos, D. R. Parrish, J. Org. Chem. 197439, 1615; U. Eder, G. Sauer, R. Wiechert, Angew. Chem. Int. Ed. 197110, 496, DOI). However, the transition metal-based catalysts developed more recently have drawn the lion’s share of attention.

Hajos-Parrish-Eder-Sauer-Wiechert reaction (example)

The first publications from the groups of MacMillan, List, Denmark, and Jacobson paved the way in the year 1990. These reports introduced highly enantioselective transformations that rivaled the metal-catalyzed reactions in both yields and selectivity. Once this foundation was laid, mounting interest in organocatalysis was reflected in a rapid increase in publications on this topic from a growing number of research groups.
Proline-derived compounds have proven themselves to be real workhorse organocatalysts. They have been used in a variety of carbonyl compound transformations, where the catalysis is believed to involve the iminium form. These catalysts are cheap and readily accessible:
A. J. A. Cobb, D. M. Shaw, D. A. Longbottom, J. B. Gold, S. V. Ley, Org. Biomol. Chem.20053, 84-96.

Y. Hayashi, T. Sumiya, J. Takahashi, H. Gotoh, T. Urushima, M. Shoji, Angew. Chem. Int. Ed.200645, 958-961.

Kumaragurubaran, K. Juhl, W. Zhuang, A. Gogevig, K. A. Jorgensen, J. Am. Chem. Soc.20021246254-6255.

A general picture of recent developments: V. D. B. Bonifacio, Proline Derivatives in Organic SynthesisOrg. Chem. Highlights2007, March 25.

Books on Organocatalysis
Albrecht Berkessel, Harald Gröger
Hardcover, 440 Pages
First Edition, 2005
ISBN: 3-527-30517-3 - Wiley-VCH


Recent Literature
An efficient one-pot procedure allows the preparation of substituted quinolines from activated acetylenes and o-tosylamidocarbonyl compounds under base-catalyzed, mild conditions. The generation of a β-phosphonium enoate α-vinyl anion in situ is followed by Michael addition of the deprotonated tosylamides and subsequent rapid aldol cyclization. Detosylation of the dihydroquinoline intermediates occurred readily in the presence of aqueous HCl.
S. Khong, O. Kwon, J. Org. Chem.2012778257-8267.

A practical and highly enantioselective Michael addition of malonates to enones to yield 1,5-ketoesters with good yields and excellent enantioselectivities is catalyzed by a simple and readily available bifunctional primary amine-thiourea derived from 1,2-diaminocyclohexane. The addition of weak acids and elevated temperature improved the efficiency of the reaction. This approach is applicable in multigram scale synthesis.
K. Dudziński, A. M. Pakulska, P. Kwiatkowski, Org. Lett.2012144222-4225.

N-hydroxyphthalimide (NHPI) catalyzes a metal-free, aerobic oxidative cleavage of olefins. This methodology avoids the use of toxic metals or overstoichiometric amounts of traditional oxidants, showing good economical and environmental advantages. Based on the experimental observations, a plausible mechanism is proposed.
R. Lin, F. Chen, N. Jiao, Org. Lett.2012144158-4161.

A one-pot conversion of aldehydes to esters interfaces N-heterocyclic carbene-based organocatalysis with electro-organic synthesis to achieve direct oxidation of catalytically generated electroactive intermediates. A broad range of aldehyde and alcohol substrates has been converted. Furthermore, the anodic oxidation reactions are very clean, producing only H2 gas as a result of cathodic reduction.
E. E. Finney, K. A. Ogawa, A. J. Boydston, J. Am. Chem. Soc.2012134, 12374-12377.

Aryl iodides are efficient catalysts in an organocatalytic syn diacetoxylation of alkenes. A broad range of substrates, including electron-rich as well as electron-deficient alkenes,  furnish the desired products in very good yields with high diastereoselectivity.
W. Zhong, S. Liu, J. Yang, X. Meng, Z. Li, Org. Lett.2012143336-3339.

Confined chiral Brønsted acids catalyze asymmetric oxidations of a broad range of sulfides to sulfoxides with hydrogen peroxide. The wide generality and high enantioselectivity of the developed method is comparable even to the best metal-based systems.
S. Liao, I. Čorić, Q. Wang, B. List, J. Am. Chem. Soc.2012134, 10765-10768.

A direct reductive amination of ketones using the Hantzsch ester in the presence of S-benzyl isothiouronium chloride as a recoverable organocatalyst converts a wide range of ketones as well as aryl amines to the expected products in good yields.
Q. P. B. Nguyen, T. H. Kim, Synthesis2012, 1977-1982.

An organocatalytic Dakin oxidation of electron-rich arylaldehydes to phenols can be performed under mild, basic conditions using flavin catalysts. Catechols are readily prepared and the oxidation of 2-hydroxyacetophenone was achieved.
S. C. M. S. Hoassain, F. W. Foss, Jr, Org. Lett.201214, 2806-2809.

The in situ generation of α-amino aldehydes followed by reaction with dimethyloxosulfonium methylide under Corey-Chaykovsky reaction conditions gives 4-hydroxypyrazolidine derivatives in high yields with excellent enantio- and diastereoselectivities. This organocatalytic sequential method enables an efficient synthesis of anti-1,2-aminoalcohols.
B. S. Kumar, V. Venkataramasubramanian, A. Sudalai, Org. Lett.201214, 2468-2471.

Ozonolysis in the presence of pyridine directly generates ketones or aldehydes through a process that neither consumes pyridine nor generates any detectable peroxides. The reaction is hypothesized to involve nucleophile-promoted fragmentation of carbonyl oxides via formation of zwitterionic peroxyacetals.
R. Willand-Charnley, T. J. Fisher, B. M. Johnson, P. H. Dussault, Org. Lett.201214, 2242-2245.

A bifunctional organocatalyst efficiently catalyzed not only enantioselective conjugate addition of aromatic ketones to nitroolefins in good yields with excellent enantioselectivities but also enantioselective conjugate addition of acetone to nitroolefins in excellent yields with high enantioselectivities.
Z.-W. Sun, F.-Z. Peng, Z.-Q. Li, L.-W. Zhou, S.-X. Zhang, X. Li, Z.-H. Shao, J. Org. Chem.2012774103-4110.

Organocatalytic stereospecific dibromination of various functionalized alkenes was achieved using a simple thiourea catalyst and 1,3-dibromo 5,5-dimethylhydantoin as a stable, inexpensive halogen source at room temperature. The procedure was extended to alkynes and aromatic rings and to dichlorination reactions by using the 1,3-dichloro hydantoin derivative.
G. Hernández-Torres, B. Tan, C. F. Barbas III, Org. Lett.201214, 1858-1861.

A nitroxyl-radical-catalyzed oxidation using diisopropyl azodicarboxylate (DIAD) allows the conversion of various primary and secondary alcohols to their corresponding aldehydes and ketones without overoxidation to carboxylic acids. 1,2-Diols are oxidized to hydroxyl ketones or diketones depending on the amount of DIAD used.
M. Hayashi, M. Shibuay, Y. Iwabuchi, J. Org. Chem.2012773005-3009.

An enantioselective synthesis of γ-nitroesters by a one-pot asymmetric Michael addition/oxidative esterification of α,β-unsaturated aldehydes is based on an enantioselective organocatalytic nitroalkane addition followed by an N-bromosuccinimide-based oxidation. The γ-nitroesters are obtained in good yields and enantioselectivities, and the method provides an attractive entry to optically active γ-aminoesters, 2-piperidones, and 2-pyrrolidones.
K. L. Jensen, P. H. Poulsen, B. S. Donslund, F. Morana, K. A. Jørgensen, Org. Lett.201214, 1516-1519.

A simple chiral primary amine catalyses a highly efficient reaction for the synthesis of both Wieland-Miescher ketone and Hajos-Parrish ketone as well as their analogues in high enantioselectivity and excellent yields. This procedure represents one of the most efficient methods for the synthesis of these versatile chiral building blocks even in gram scale with 1 mol% catalyst loading.
P. Zhou, L. Zhang, S. Luo, J.-P. Cheng, J. Org. Chem.201277, 2526-2530.

The of silica-coated magnetic nanoparticles allowed the construction of magnetically recoverable organic hydride compounds. Magnetic nanoparticle-supported BNAH (1-benzyl-1,4-dihydronicotinamide) showed efficient activity in the catalytic reduction of α,β-epoxy ketones. After reaction, the catalyst can be separated by simple magnetic separation and can be reused.
H.-J. Xu, X. Wan, Y.-Y. Shen, S. Xu, Y.-S. Feng, Org. Lett.201214, 1210-1213.

Activation of diphenylsilane in the presence of a catalytic amount of an N-heterocyclic carbene (NHC) enables hydrosilylation of carbonyl derivatives under mild conditions. Presumably, a hypervalent silicon intermediate featuring strong Lewis acid character allows dual activation of both the carbonyl moiety and the hydride at the silicon center. Some interesting selectivities have been encountered.
Q. Zhao, D. P. Curran, M. Malacria, L. Fensterbank, J.-P. Goddard, E. Lacôte, Synlett2012, 433-437.

A bifunctional squaramide catalyzes a sulfa-Michael/aldol cascade reaction between 1,4-dithiane-2,5-diol and chalcones with a low catalyst loading to yield trisubstituted tetrahydrothiophenes with three contiguous stereogenic centers in a highly stereocontrolled manner.
J.-B. Ling, Y. Su, H.-L. Zhu, G.-Y. Wang, P.-F. Xu, Org. Lett.201214, 1090-1093.

A phosphinite derivative that can be easily prepared in two steps from commercially available aminoindanol is an effective catalyst for enantioselective acylation of diols. For the asymmetric desymmetrization of meso-1,2-diols, the corresponding monoester was obtained in high enantioselectivity.
H. Aida, K. Mori, Y. Yamaguchi, S. Mizuta, T. Moriyama, I. Yamamoto, T. Fujimoto, Org. Lett.201214, 812-815.

Commercially available and very inexpensive benzoic acids catalyze an efficient and simple isomerization of readily prepared allylic alcohols to yield cyclic products, unusual enyne, and dienols. The catalysts can be tuned for reactivity and substrate sensitivity.
J. A. McCubbin, S. Voth, O. V. Krokhin, J. Org. Chem.2011768537-8542.

Cinchona-alkaloid-thiourea-based bifunctional organocatalysts enable a straightforward asymmetric cycloetherification of ε-hydroxy-α,β-unsaturated ketones for the synthesis of tetrahydrofuran rings. This catalytic process represents a highly practical cycloetherification method that provides excellent enantioselectivities, even with low catalyst loadings at ambient temperature.
K. Asano, S. Matsubara, J. Am. Chem. Soc.2011133, 16711-16713.



Tuesday, 27 August 2013

Reaction kinetics and their applications to the study of organic chemistry

Stability,chelation and chelate effect in coordination compounds


Stability, Chelation and the Chelate Effect

A metal ion in solution does not exist in isolation, but in combination with ligands (such as solvent molecules or simple ions) or chelating groups, giving rise to complex ions or coordination compounds.
These complexes contain a central atom or ion, often a transition metal, and a cluster of ions or neutral molecules surrounding it. Many complexes are relatively unreactive species remaining unchanged throughout a sequence of chemical or physical operations and can often be isolated as stable solids or liquid compounds.
Other complexes have a much more transient existence and may exist only in solution or be highly reactive and easily converted to other species.
All metals form complexes, although the extent of formation and nature of these depend very largely on the electronic structure of the metal.
The concept of a metal complex originated in the work of Alfred Werner, who in 1913 was awarded the first Nobel Prize in Inorganic chemistry. A description of his life and the influence his work played in the development of coordination chemistry is given by G.B. Kauffman in "Inorganic Coordination Compounds", Heyden & Son Ltd, 1981.
Complexes may be non-ionic (neutral) or cationic or anionic, depending on the charges carried by the central metal ion and the coordinated groups. The total number of points of attachment to the central element is termed the coordination number and this can vary from 2 to greater than 12, but is usually 6.
The term ligand (ligare [Latin], to bind) was first used by Alfred Stock in 1916 in relation to silicon chemistry. The first use of the term in a British journal was by H. Irving and R.J.P. Williams in Nature, 1948, 162, 746 in their paper describing what is now called the Irving-Williams series.
For a fascinating review of the origin and dissemination of the term 'ligand' in chemistry see: W.H. Brock, K.A Jensen, C.K. Jorgensen and G.B. Kauffman, Polyhedron, 2, 1983, 1-7.
Ligands can be further characterised as monodentate, bidentate, tridentate etc. where the concept of teeth (dent) is introduced, hence the idea of bite angle etc.
The term chelate was first applied in 1920 by Sir Gilbert T. Morgan and H.D.K. Drew [J. Chem. Soc., 1920, 117, 1456], who stated: 
"The adjective chelate, derived from the great claw or chela (from the Greek χηλη) of the lobster or other crustaceans, is suggested for the caliperlike groups which function as two associating units and fasten to the central atom so as to produce heterocyclic rings." 

lobster claw 
Metal complexation is of widespread interest. It is studied not only by inorganic chemists, but by physical and organic chemists and by biochemists, pharmacologists, molecular biologists and environmentalists. 

Thermodynamic Stability

In the laboratory course, it will have been pointed out that the "stability of a complex in solution" refers to the degree of association between the two species involved in the state of equilibrium. Qualitatively, the greater the association, the greater the stability of the compound. The magnitude of the (stability or formation) equilibrium constant for the association, quantitatively expresses the stability. Thus, if we have a reaction of the type: 
M   +   4L    →   ML4
then the larger the stability constant, the higher the proportion of ML4 that exists in the solution. Free metal ions rarely exist in solution so that M, will usually be surrounded by solvent molecules which will compete with the ligand molecules, L, and be successively replaced by them. For simplicity, we generally ignore these solvent molecules and write four stability constants as follows: 
l.       M + L → ML            K1 = [ML] / [M] [L] 
2.      ML + L → ML2        K2 = [ML2] / [ML] [L] 
3.      ML2 + L → ML3      K3 = [ML3] / [ML2] [L] 
4.      ML3 + L → ML4      K4 = [ML4] / [ML3] [L] 
where K1, K2 etc. are referred to as "stepwise stability constants". 
Alternatively, we can write the "Overall Stability Constant" thus: 
M   +   4L    →   ML4      β4 = [ML4]/ [M] [L]4
The stepwise and overall stability constants are therefore related as follows: 
β4 =K1.K2.K3.K4 or more generally, 
βn =K1.K2.K3.K4--------------K n
If we take as an example, the steps involved in the formation of the cuprammonium ion, we have the following: 
Cu2+ + NH3 ↔ Cu(NH3)2+ K1 = [Cu(NH3)2+]/[Cu2+] [NH3]
CuNH32+ + NH3 ↔ Cu(NH3)22+ K2 = [Cu(NH3)22+]/[Cu(NH3)2+] [NH3]
etc. where K1, K2 are the stepwise stability constants. 
Also: 
          β4  = [Cu(NH3)42+]/[Cu2+] [NH3]4
The addition of the four ammine groups to copper shows a pattern found for most formation constants, in that the successive stability constants decrease. In this case, the four constants are: 
     logK1 =4.0, logK2 =3.2, logK3 =2.7,  logK4 =2.0 or logβ4 =11.9
A number of texts refer to the instability constant or the dissociation constant of coordination complexes. This value corresponds to the reciprocalof the formation constant, since the reactions referred to are those where fully formed complexes break down to the aqua ion and free ligands. 
This should be compared with the equation for the formation constant given earlier. 
It is usual to represent the metal-binding process by a series of stepwise equilibria which lead to stability constants that may vary numerically from hundreds to enormous values such as 1035 and more. 
That is 100,000,000,000,000,000,000,000,000,000,000,000.0 
For this reason, they are commonly reported as logarithms. 
so log10 (β) = log10 (1035) = 35. 
It is additionally useful to use logarithms, since log(K) is directly proportional to the free energy of the reaction.

ΔG° = -RTln(β) 
ΔG° = -2.303 RTlog10(β) 
ΔG° = ΔH° - TΔS° 
For a problem relating to metal complex formation and calculations of free metal ions concentrations, try your hand at CALCULATION # ONE. Other problems can be found in the Tutorial paper for this course. 

The Chelate Effect

The chelate effect can be seen by comparing the reaction of a chelating ligand and a metal ion with the corresponding reaction involving comparable monodentate ligands. For example, comparison of the binding of 2,2'-bipyridine with pyridine or 1,2-diaminoethane (ethylenediamine=en) with ammonia.
It has been known for many years that a comparison of this type always shows that the complex resulting from coordination with the chelating ligand is much more thermodynamically stable. This can be seen by looking at the values for adding two monodentates compared with adding one bidentate, or adding four monodentates compared to two bidentates, or adding six monodentates compared to three bidentates. 

Some tables of thermodynamic data

Reaction of ammonia and 1,2-diaminoethane with Cd2+.
# of ligandsΔG° (kJmol-1)ΔH° (kJmol-1)ΔS° (JK-1mol-1)log β
2 NH3(1 en)-28.24 (-33.30)-29.79 (-29.41)-5.19 (+13.05)4.95 (5.84)
4 NH3(2 en)-42.51 (-60.67)-53.14 (-56.48)-35.50 (+13.75)7.44 (10.62)

Reaction of pyridine and 2,2'-bipyridine with Ni2+.
# of ligandslog βΔG° (kJmol-1)
2 py (1 bipy)3.5 (6.9)-20 (-39)
4 py (2 bipy)5.6 (13.6)-32 (-78)
6 py (3 bipy)9.8 (19.3)-56 (-110)

Reaction of ammonia and 1,2-diaminoethane with Ni2+.
# of ligandslog βΔG° (kJmol-1)
1 NH32.8-16
2 NH3 (1 en)5.0 (7.51)-28.5 (-42.8)
3 NH36.6-37.7
4 NH3 (2 en)7.87 (13.86)-44.9 (-79.1)
5 NH38.6-49.1
6 NH3 (3 en)8.61 (18.28)-49.2 (-104.4)

A number of points should be highlighted from this data. 
In the first table, it can be seen that the ΔH° values for the formation steps are almost identical, that is, heat is evolved to about the same extent whether forming a complex involving monodentate ligands or bidentate ligands. 
What is seen to vary significantly is the ΔS° term which changes from negative (unfavourable) to positive (favourable). Note as well that there is a dramatic increase in the size of the ΔS° term for adding two compared to adding four monodentate ligands. (-5 to -35 JK-1mol-1). 
What does this imply, if we consider ΔS° to give a measure of disorder?
In the case of complex formation of Ni2+ with ammonia or 1,2-diaminoethane, by rewriting the equilibria, the following equations are produced.
Ni reactions

Using the equilibrium constant for the reaction (3 above) where the three bidentates replace the six monodentates, we find that at a temperature of 25C:
ΔG° = -2.303 RT log10 (K) 
= -2.303 R T (18.28 - 8.61) 
= -54 kJ mol-1 
Based on measurements made over a range of temperatures, it is possible to break down the ΔG° term into the enthalpy and entropy components. ΔG° = ΔH° - TΔS° 
The result is that:
ΔH° = -29 kJ mol-1 
- TΔS° = -25 kJ mol-1 
and at 25C (298K) 
ΔS° = +88 J K-1 mol-1 

Note that for many years, these numbers have been incorrectly recorded in textbooks. 
For example, the third edition of "Basic Inorganic Chemistry" by F.A. Cotton, G. Wilkinson and P.L. Gaus, John Wiley & Sons, Inc, 1995, on page 186 gives the values as:
ΔG° = -67 kJ mol-1 
ΔH° = -12 kJ mol-1 
- TΔS° = -55 kJ mol-1 
The conclusion they drew from these incorrect numbers was that the chelate effect was essentially an entropy effect, since the TΔS° contribution was nearly 5 times bigger than ΔH°.

In fact, the breakdown of the ΔG° into ΔH° and TΔS° shows that the two terms are nearly equal (-29 cf. -25 kJ mol-1) with the ΔH° term a little bigger! The entropy term found is still much larger than for reactions involving a non-chelating ligand substitution at a metal ion. 
How can we explain this enhanced contribution from entropy? One explanation is to count the number of species on the left and right hand side of the equation above. 
It will be seen that on the left-hand-side there are 4 species, whereas on the right-hand-side there are 7 species, that is a net gain of 3 species occurs as the reaction proceeds. This can account for the increase in entropy since it represents an increase in the disorder of the system. 
An alternative view comes from trying to understand how the reactions might proceed. To form a complex with 6 monodentates requires 6 separate favourable collisions between the metal ion and the ligand molecules. To form the tris-bidentate metal complex requires an initial collision for the first ligand to attach by one arm but remember that the other arm is always going to be nearby and only requires a rotation of the other end to enable the ligand to form the chelate ring. 
If you consider dissociation steps, then when a monodentate group is displaced, it is lost into the bulk of the solution. On the other hand, if one end of a bidentate group is displaced the other arm is still attached and it is only a matter of the arm rotating around and it can be reattached again. 
Both sets of conditions favour the formation of the complex with bidentate groups rather than monodentate groups.

Advanced organic chemistry notes

Factors governing polarization and polarisability in Fazans Rule



FACTORS GOVERNING POLARIZATION AND POLARISABILITY (FAJAN’S RULE)

Cation Size: Smaller is the cation more is the value of charge density (Φ) and hence more its polarising power. As a result more covalent character will develop. Let us take the example of the chlorides of the alkaline earth metals. As we go down from Be to Ba the cation size increases and the value of Φ decreases which indicates that BaClis less covalent i.e. more ionic. This is well reflected in their melting points. Melting points of BeCl2 = 405°C and BaCl2 = 960°C.
Cationic Charge: More is the charge on the cation, the higher is the value of Φ and higher is the polarising power. This can be well illustrated by the example already given, NaBr and AlBr3. Here the charge on Na is +1 while that on Al in +3, hence polarising power of Al is higher which in turn means a higher degree of covalency resulting in a lowering of melting point of AlBr3 as compared to NaBr.  
Noble Gas vs Pseudo Noble Gas Cation:A Pseudo noble gas cation consists of a noble gas core surrounded by electron cloud due to filled d-subshell. Since d-electrons provide inadequate shielding from the nuclei charge due to relatively less penetration of orbitals into the inner electron core, the effective nuclear charge (ENC) is relatively larger than that of a noble gas cation of the same period. NaCl has got a melting point of 800°C while CuCl has got melting point of 425°C. The configuration of Cu+ = [Ar] 3d10 while that of Na+ = [Ne]. Due to presence of d electrons ENC is more and therefore Cl is more polarised in CuCl leading to a higher degree of covalency and lower melting point.
Anion Size:Larger is the anion, more is the polarisability and hence more covalent character is expected. An e.g. of this is CaF2 and CaI2, the former has melting point of 1400°C and latter has 575°C. The larger size of I ion compared to F causes more polarization of the molecule leading to a lowering of covalency and increasing in melting point.
Anionic Charge:Larger is the anionic charge, the more is the polarisability. A well illustrated example is the much higher degree of covalency in magnesium nitride (3Mg++ 2N3–) compared to magnesium fluoride (Mg++ 2F). This is due to higher charge of nitride compare to fluoride. These five factors are collectively known as Fajan’s Rule.
Example:
The melting point of KCl is higher than that of AgCl though the crystal radii of Ag+and K+ ions are almost same.
Solution:

Now whenever any comparison is asked about the melting point of the compounds which are fully ionic from the electron transfer concept it means that the compound having lower melting point has got lesser amount of ionic character than the other one. To analyse such a question first find out the difference between the 2 given compounds. Here in both the compounds the anion is the same. So the deciding factor would be the cation. Now if the cation is different, then the answer should be from the variation of the cation. Now in the above example, the difference of the cation is their electronic configuration. K+ = [Ar]; Ag+ = [Kr] 4d10. This is now a comparison between a noble gas core and pseudo noble gas core, the analysis of which we have already done. So try to finish off this answer.
Example: AlF3 is ionic while AlCl3 is covalent.
Solution: Since F is smaller in size, its polarisability is less and therefore it is having more ionic character. Whereas Cl being larger in size is having more polarisability and hence more covalent character.
Example:
Which compound from each of the following pairs is more covalent and why? 
(a) CuO or CuS                 (b) AgCl or AgI
(c) PbCl2 or PbCl4              (d) BeCl2 or MgCl2
Solution:
(a) CuS                           (b) AgI

(c) PbCl4                         (d) BeCl­2