1. Liquid Crystals Recall that the total phase change entropy of semi- perfluorinated compounds were considerably less than the values estimated. Many of these materials form liquid crystals.

2. Table. Molar Transition Enthalpies (kJ mol -1 ) and Entropies (J mol -1 K -1 ) of Select Amphiphilic Semiperfluorinated-Semiper- hydrogenated Diblock and Triblock Organic Compounds a T(K)  H pce  S pce  S tpce 0.6  S tcpe  S tcpe  H tpce  H tpce exptcalcd calcd exptcalcd UNSUBSTITUTED DIBLOCK MOLECULES C 16 H 9 F 25 F 3 C(CF 2 ) 11 (CH 2 ) 4 H 147.0 0.7 5 314.0 1.4 4 349.021.06169.457.193.6 23.119.9 C 16 H 13 F 21 F 3 C(CF 2 ) 9 (CH 2 ) 6 H 306.0 4.214 318.016.9536761.6 100.921.119.6 C 16 H 17 F 17 F 3 C(CF 2 ) 7 (CH 2 ) 8 H 301.29.531.6 303.25.718.850.390.2 147.9 15.227.3 C 17 H 21 F 15 (CF 3 ) 2 CF(CF 2 ) 4 (CH 2 ) 10 H 220.0 313.6 261.01869.082.684.6 138.621.018.9

3. T(K)  H pce  S pce  S tpce 0.6  S tcpe  S tcpe  H tpce  H tpce exptcalcd calcd exptcalcd C 18 H 13 F 25 F 3 C(CF 2 ) 11 (CH 2 ) 6 H 164.0 0.5 1 316.0 3.511 357.023.465.579.765.7 107.827.423.5 C 18 H 21 F 17 F 3 C(CF 2 ) 7 (CH 2 ) 10 H 288.0 3.512 308.020.26577.786.8 142.323.726.9 C 19 H 21 F 19 (CF 3 ) 2 CF(CF 2 ) 6 (CH 2 ) 10 H 274.0 1 3.6 298.02583.987.584.6 138.62622.1 C 20 H 17 F 25 F 3 C(CF 2 ) 11 (CH 2 ) 8 H 192.0 2.412.5 329.0 6.419.5 361.023.765.797.674.712232.526.9 C 20 H 21 F 21 F 3 C(CF 2 ) 9 (CH 2 ) 10 H 317.0 4.012 337.024.4728578.9 129.328.426.6

4. Figure. A comparison of calculated and experimental total phase change entropies for the partially fluorinated amphiphilic compounds.

5.  S tcpe(calcd) = (0.648  0.06)  S tcpe expt + (30.1  13.5); r 2 = 0.6525

6. Since their first discovery back in 1888, interest in the properties and practical applications of liquid crystals has increased dramatically. 1,2 General acceptance of liquid crystals as a distinct phase of matter was slow, occurring some 30 years since they were first reported. Liquid crystalline behavior is found among numerous classes of compounds that include biphenyls, cholesterol esters, soaps, lipids, polymers and elastomers. More than 76000 compounds have been identified as exhibiting liquid crystalline behavior. Liquid Crystals

7. Between 1850 and 1888, researchers found that several materials behaved strangely at temperatures near their melting points. It was observed that the optical properties of these materials changed discontinously with increasing temperatures. W. Heintz, for example, reported in 1850 that stearin melted from a solid to a cloudy liquid at 52°C, changed at 58°C to an opaque and at 62.5°C to a clear liquid. Others reported observing blue colors when cholesterol esters were cooled. Biologists observed anisotropic optical behavior in "liquid" biological materials, a behavior usually expected only in the crystal phase.

8. In 1888, an Austrian botanist named Friedrich Reinitzer, interested in the biological function of cholesterol in plants, was looking at the melting behaviour of an organic substance related to cholesterol. (The chemical structure of cholesterol was still unknown. Today we know that the observed substance was cholesteryl benzoate). He observed, as W. Heintz did with stearin 38 years before, that the substance melted to a cloudy liquid at 145.5°C and became a clear liquid at 178.5°C. He repeated an earlier observation which showed that upon cooling the clear liquid, a brief appearance of blue color could be seen at the transition temperature, and that a blue violet color appeared just before crystallization from: http://www.lci.kent.edu/lc_history.html

9. An examination of the phase change enthalpies of liquid crystals reveals that these substances exhibit several thermal transitions that can be detected. For most substances, the largest enthalpic change occurs upon conversion of the solid to a nematic or smectic phase. DSC is a common way of studying the thermal behavior of liquid crystals

11. In the most popular DSC design, two pans sit on a pair of identically positioned platforms connected to a furnace by a common heat flow path. In one pan, you put your sample. The other one is the reference pan. You place an MT cell. You then program the computer to turn on the furnace to heat the two pans at a specific rate, usually something like 5 o C per minute. If heat is adsorbed or emitted, the power supplied to maintain a constant temperature is measured.

12. Figure. DSC trace of a typical compounds exhibiting liquid crystal formation.

13. Schlieren texture of a nematic film with surface point defects (boojums). This picture was taken under a polarization microscope with polarizer and analyzer crossed. From every point defect emerge four dark brushes. For these directions the director is parallel either to the polarizer or to the analyzer. The colors are newton colors of thin films and depend on the thickness of the sample. Point defects can only exist in pairs. One can see two types of boojuns with "opposite sign of topological charge"; one type with yellow and red brushes, the other kind not that colorful. The difference in appearance is due to different core structures for these defects of different "charge".

15. T >230 ºC

16. 230 > T > 195 ºC

17. 195 > T > 165 ºC

18. 165 > T > 140 ºC

19. 140 > T > 85 ºC

20. 85 > T > mp ºC

21. C 14 H 30 O 4 CH 2 OHCHOH(CH 2 ) 10 CHOHCH 2 OH  tpce S m (exp) = 131.3 J mol -1. K -1 ;  tpce S m (calc) = 176.6 J mol -1. K -1  tpce S m (calc) = 2(7.1)+2(16.4)(0.6)+2(1.7)(13.1)+10(1.31)(7.1) C 20 H 28 O 3  tpce S m (exp) = 82.7 J mol -1. K -1 ;  tpce S m (calc) = 107.9 J mol -1. K -1 (calc) =2*17.6+3*7.1+33.4+3*3.7+2*(-14.7) +5.3*0.75 +5.3 +4*7.4+2(-7.5)+7.7+ 4.7

22. Fig. A comparison of the experimental and calculated total phase change entropies of 2637 compounds. The area between the two lines represents  2 .

24. Fig. A comparison of calculated and experimental values for 627 liquid crystals. The solid line represents the equation obtained by a linear regression analysis and the area within the two dotted lines represents anticipated values of falling within  2  based on the evaluations of database compounds.

25. Fig. A histogram of the distribution of errors in (exp) - (calc) for liquid crystals. Each interval represents one standard deviation (15.3 J. mol -1. K -1 ). Six compounds has errors equal to or larger than -30 .

26. Possible reasons responsible for both the scatter and overestimations observed in Fig. 3. 1.Some residual molecular association exists at the clearing temperature. 2.Attenuation in phase change entropies is compensated at some temperature by increases in the heat capacity of the crystal. 3.Polymorphism may also play a role. 4.The solid phase may not possess total crystallinity. Studies on polymeric materials have shown that the measured enthalpies of fusion depend on the degree of crystallinity. 5.Occurrence of undetected solid-solid phase transitions at low temperatures is certainly a possibility.

27. Table. A series of compound including liquid crystals whose heat capacity and phase transitions of the crystalline phase have been studied over most of the experimentally accessible region a TransitionT/K  pce H m  pce S m  tpce S m (exp)  tpce S m (estimated) S o (385 K) C 36 H 54 O 12 benzene hexa-n-pentanoate Sol/Sol173.1 8.850.83 Sol/Sol313.215.348.85 Sol/Liq379.530.379.84 183.5 234.6 1629.9 C 42 H 66 O 12 benzene hexa-n-hexanoate Sol/Sol251.625.67102.0 Sol/Sol291.512.27 42.1 Sol/Sol348.316.26 46.7 Sol/Liq368.733.50 90.9 281.7 2771877.1 C 48 H 78 O 12 benzene hexa-n-heptanoate Sol/Sol129 1.1 8.5 Sol/Meso353.832.291.1 Meso/Liq359.321.559.9 159.5 319.82114.4 C 54 H 90 O 12 benzene hexa-n-octanoate Sol/Sol301.949.0164.0 Sol/Meso355.146.1129.8 Meso/Liq357.119.2 53.8 347.6 362.42361.3 C 60 H 102 O 12 benzene hexa-n-nonanoate Sol/Sol248.319.4 78.13 Sol/Sol278.3 4.9 17.60 Sol/Liq353.169.2195.98 291.7 4052597.8 Liq/Meso350NA C 66 H 114 O 12 benzene hexa-n-decanoate Sol/Sol330.875.7228.9 Sol/Liq360.991.8254.3 483.2 4482861.5 a Cp measurements of the solid from approximately 15 K to the isotropic liquid at 385 K.

28. S o = +  pce H/T + +  fus H/T fus + … Recall that S o evaluated from 15 K to 385 K 1.M. Sorai, K. Tsuji, H. Suga and S. Seki, Mol. Cryst. Liq. Cryst., 80, 33-58 (1980). 2.M. Sorai and H. Suga, Mol. Cryst. Liq. Cryst., 73, 47-69 (1981).12.M. Sorai, H. Yoshioka and H. Suga, Mol. Cryst. Liq. Cryst., 84, 39-54 (1982). 3.S. Asahina and M. Sorai, J. Chem. Thermodyn., 35, 649-666 (2003). 4.S. Asahina, and M. Sorai, Liq Cryst., 28, 1085-1092 (2001).

29. Fig. A plot of the entropy of the benzene hexa-n-alkanoates at T = 385 K as a function of the number of carbon atoms.

30. The pentanoate, hexanoate and decanoate do not form liquid crystals. The nonanoate does so only on supercooling the isotropic liquid below the melting temperature. Both the heptanoate and octanoate form liquid crystals. Agreement between estimated and experimental total phase change entropies is within the noise level expected for these estimations for the pentanoate, hexanoate, octanoate and decanoate. Values for the heptanoate and nonanoate are clearly overestimated. Even for the octanoate, although the two values are within experimental uncertainty, the calculated value is somewhat larger.

31. Conclusions 1.Deviations not due to residual molecular association existing at the clearing temperature. 2.Effects due to polymorphism not likely. 3.The solid phase is crystalline. 4.Undetected phase transitions are not responsible. 5.Attenuation in phase change entropies is compensated at some temperatures by “abnormal” increases in the heat capacity of the crystal.

32. Definition of T fus, T clr and T iso for Liquid Crystals T fus = melting temperature T clr = temperature at which the liquid crystal clears; for some samples, this could below T fus if the sample supercools T iso = temperature at which the liquid crystal becomes isotropic; for most compounds also equal to T clr T iso = T iso max (  )[1- 1/(mN + b)] for increasing T f (n) T iso = T iso min / [1- 1/(mN + b)] for decreasing T f (n)

33. Question: How do the melting temperatures of liquid crystals compare to the melting temperatures of analogous compounds that do not form liquid crystals?

34. Figure. Circles: melting temperatures or temperatures at which the trans-4-n-alkoxy-3- chlorocinnamic acids becomes isotropic; squares are melting temperatures for compounds forming liquid crystals; triangles: smectic to nematic transitions

35. Figure. A plot of 1/[1-T(  )/T(n)] versus the number of methylene groups for trans-4-n-alkoxy-3- chlorocinnamic acids. The solid circles represent melting temperatures, the solid squares represent nematic to isotropic transitions, the circles represent smectic to nematic transitions and the squares represent from nematic to isotropic transitions. The temperatures at which the liquids become isotropic appear to correlate best. A value of 380 K was used for T(  ).

36. Fig. A comparison of the melting and clearing temperatures of the thiocholesteryl n- alkanoates (odd series); circles: melting temperatures; squares: clearing temperatures. The first and third compounds in the series do not form liquid crystals. 16 T fus (n) = 317/ [1- 1/((0.564)n + 5.133)]; r 2 = 0.6586 T iso (n) = 234/ [1- 1/((0.0238)n + 2.528)]; r 2 = 0.9661

37. Fig. A comparison of the melting and clearing temperatures of the thiocholesteryl n- alkanoates (even series); circles: melting temperatures; squares: clearing temperatures T fus (n) = 259/ [1- 1/((0.0745)n + 3.065)]; r 2 = 0.7508 T iso (n) = 328/ [1- 1/((0.4185)n + 5.436)]; r 2 = 0.9931

38. It appears that the melting temperature correlates best with the temperature at which the liquid crystals become isotropic. This means that the temperature at which the solid melts is lowered as a result of formation of the smectic or nematic phase. Why is there a melting point lowering? Why do impure materials melt lower than pure materials?

39. T fus (n) = 317/ [1- 1/((0.564)n + 5.133)]; r 2 = 0.6586 T iso (n) = 234/ [1- 1/((0.0238)n + 2.528)]; r 2 = 0.9661 T fus (n) = 259/ [1- 1/((0.0745)n + 3.065)]; r 2 = 0.7508 T iso (n) = 328/ [1- 1/((0.4185)n + 5.436)]; r 2 = 0.9931 T iso = T iso min / [1- 1/(mN + b)] for decreasing T f (n) Question: How was T iso min determined for each of these series?

40. Ans: 1/[1- T iso min /T(n)] was plotted against n using T iso min, as a variable. The best value of T iso min was chosen on the basis of a non-linear least squares program.

41. Binary phase diagram 100 %A 0 %A 0% B 100%B mp

42. Packing of the solid in series that form liquid crystals is affected much like the presence of an impurity.

43. What happens when the descending portion of the T iso is reached?

44. Fig. A comparison of the melting and clearing temperatures of the alkyl 4’-methoxybiphenyl-4- carboxylates (odd series); circles: melting temperatures; squares: clearing temperatures. The first two and last entries do not form liquid crystals. A portion of the melting behavior expected of a homologous series after the minimum is reached. The members of the series exhibiting liquid crystalline behavior occur on the descending portion of the curve. Liquid crystalline behavior appears to cease before the minimum. Once the minimum is reached, the melting temperatures are predicted to increase gradually to T = 411 K.

45. Why Do Compounds Form Liquid Crystals?

46. Table Group values for estimating heat capacities of solids at T = 298 K GroupValues ab GroupValues ab Hydrocarbon Groups  (c)  (c) primary sp 3 C 36.6tertiary aromatic sp 2 C17.5 secondary sp 3 C 26.9quaternary aromatic sp 2 C 8.5 tertiary sp 3 C 9.0internal quaternary aromatic sp 2 C [9.1] quaternary sp 3 C -4.98 cyclic secondary sp 3 C 24.6 secondary sp 2 C [46.0]cyclic tertiary sp 3 C 11.7 tertiary sp 2 C 21.4 cyclic quaternary sp 3 C 6.1 quaternary sp 2 C [6.86]cyclic tertiary sp 2 C15.9 tertiary sp C [23.9]cyclic quaternary sp 2 C [4.73] quaternary sp C [15.2]

47. Functional Groups alcohols, phenols 23.5 cyclic ether9.71 fluorine [24.8] isocyanate [52.7] chlorine 28.7 nitro group 56.1 bromine 32.4 thiols [51.9] nitrile [42.3] primary sp 3 N 21.6 carboxylic acid 53.1 secondary sp 3 N [-0.29] aldehyde [84.5] tertiary sp 3 N [31.5] ketones [28.0]tertiary sp 2 N 10.7 cyclic ketones 34.3 cyclic secondary sp 3 N [23.9] ester40.3 cyclic tertiary sp 3 N1.21 lactone [45.2]cyclic tertiary sp 2 N13.9 ether49.8 sulfides[116] cyclic sulfides 18.2

48. Simple dialkyl ethers and n-alkanes do not form liquid crystals. In addition, their heat capacities at T = 298.15 K are generally well modeled by the group values listed in the previous tables. Why is it that dialkyl ethers and n-alkanes do not form liquid crystals and why are the Cp(c) values for these molecules at various temperatures less than the values found for compounds forming liquid crystals? Recall that  tpce S m (exp) <  tpce S m (estimated) but that S° m (total) appears to be a linear function in homologous series.

49. Figure. Melting temperatures of the odd 1-alkenes, n-alkylbenzenes, n-carboxylic acids, N- (2-hydroxyethyl)alkanamides and 1,  -dicarboxylic acids versus the number of methylene groups, circles, squares triangles and hexagons: experimental data; lines: calculated results.

50. The fact that the first few members of the series deviate from the remaining members is explained as a result of a change in packing from one dominated by the functional group or head group to one dominated by the chain. In liquid crystals, this deviation is exaggerated. However, if the packing is dominated by the head group, then the alkyl chains will be packed loosely and their contribution to the heat capacity will be even larger than their normally high value. Why would the contribution of Cp of a loosely packed group be greater than for a more tightly packed group?

51. Empirical Justification

53. ____________ ____--____-- Theoretical Perspective

55. As a crystal is heated, more thermal motion will be concentrated in the alkyl chains and less in the rigid component. At some point the thermal energy will be enough to disrupt the alkyl chains so they become fluid, before all the attractive forces associated with the head group are overcome As a consequence, the tails are fluid while the heads retain some degree of order. The hydrophobic and hydrophillic interactions then are responsible for the nature of the order obtained. Whether a compound forms a liquid crystal is likely to be a delicate balance between how evenly or unevenly thermal motion is distributed within the crystal.