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Describe how a cholesteric liquid crystal phase differs from a nematic phase.

Short Answer

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A cholesteric liquid crystal phase, also known as chiral nematic phase, is characterized by chiral molecules that cause a helical molecular orientation. It consists of layers with well-defined spacing, but no positional order within each layer. In contrast, the nematic phase consists of rod-like molecules aligned along a common direction called the director, with positional disorder but orientational order. The key differences between these phases stem from the presence of chiral molecules and their resulting molecular arrangements, leading to distinct properties such as selective reflection of light in cholesteric phase, not seen in the nematic phase.

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01

Cholesteric Phase Properties

The cholesteric liquid crystal phase, or chiral nematic phase, is a special type of nematic phase. It is characterized by the presence of chiral molecules, which causes the molecular orientation to twist in a helical pattern. The pitch of this helix, or the distance over which the director (orientation of the molecules) rotates by 360 degrees, is called the cholesteric pitch. In a cholesteric phase, the molecules are arranged into layers with a well-defined layer spacing, but the positions of the individual molecules are not ordered within each layer.
02

Nematic Phase Properties

The nematic phase is a type of liquid crystal phase in which the rod-like molecules are aligned along a common direction, called the director. In this phase, the molecules possess positional disorder, meaning they are not arranged into a regular lattice structure. However, they maintain a degree of orientational order, as their long axes are preferentially aligned along the director. The nematic phase typically exhibits birefringence, which means that the refractive index depends on the polarization of the light relative to the director.
03

Comparison of Cholesteric and Nematic Phases

The main differences between the cholesteric and nematic phases lie in the presence of chiral molecules and the resulting molecular arrangement. In the cholesteric phase, the helical structure arises due to the presence of chiral molecules. In contrast, the nematic phase consists of rod-like molecules aligned in parallel without any helical twisting. This difference in molecular arrangement leads to distinct properties, such as the cholesteric phase's selective reflection of light, which is not observed in the nematic phase.

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Most popular questions from this chapter

A number of salts containing the tetrahedral polyatomic anion, \(\mathrm{BF}_{4}^{-},\) are ionic liquids, whereas salts containing the somewhat larger tetrahedral ion \(\mathrm{SO}_{4}^{2-}\) do not form ionic liquids. Explain this observation.

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The following data present the temperatures at which certain vapor pressures are achieved for dichloromethane \(\left(\mathrm{CH}_{2} \mathrm{Cl}_{2}\right)\) and methyl iodide \(\left(\mathrm{CH}_{3} \mathrm{I}\right)\) : $$ \begin{array}{lllll} \text { Vapor Pressure } & & & & \\ \text { (torr): } & 10.0 & 40.0 & 100.0 & 400.0 \\ \hline T \text { for } \mathrm{CH}_{2} \mathrm{Cl}_{2}\left({ }^{\circ} \mathrm{C}\right): & -43.3 & -22.3 & -6.3 & 24.1 \\ T \text { for } \mathrm{CH}_{3} \mathrm{I}\left({ }^{\circ} \mathrm{C}\right): & -45.8 & -24.2 & -7.0 & 25.3 \end{array} $$ (a) Which of the two substances is expected to have the greater dipole-dipole forces? Which is expected to have the greater dispersion forces? Based on your answers, explain why it is difficult to predict which compound would be more volatile. (b) Which compound would you expect to have the higher boiling point? Check your answer in a reference book such as the CRC Handbook of Chemistry and Physics. (c) The order of volatility of these two substances changes as the temperature is increased. What quantity must be different for the two substances in order for this phenomenon to occur? (d) Substantiate your answer for part (c) by drawing an appropriate graph.

The critical temperatures \((\mathrm{K})\) and pressures \((\mathrm{atm})\) of a series of halogenated methanes are as follows: $$ \begin{array}{lcccc} \text { Compound } & \mathbf{C C l}_{3} \mathbf{F} & \mathbf{C C l}_{2} \mathbf{F}_{2} & \mathbf{C C I F}_{3} & \mathbf{C F}_{4} \\ \hline \text { Critical temperature } & 471 & 385 & 302 & 227 \\ \text { Critical pressure } & 43.5 & 40.6 & 38.2 & 37.0 \end{array} $$ (a) List the intermolecular forces that occur for each compound. (b) Predict the order of increasing intermolecular attraction, from least to most, for this series of compounds. (c) Predict the critical temperature and pressure for \(\mathrm{CCl}_{4}\) based on the trends in this table. Look up the experimentally determined critical temperatures and pressures for \(\mathrm{CCl}_{4}\), using a source such as the CRC Handbook of Chemistry and Physics, and suggest a reason for any discrepancies.

As the intermolecular attractive forces between molecules increase in magnitude, do you expect each of the following to increase or decrease in magnitude? (a) vapor pressure, (b) heat of vaporization, (c) boiling point, (d) freezing point, (e) viscosity, (f) surface tension, (g) critical temperature.

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