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CRC Press eBooks

Ensembles, Energy Levels, and Microstates

Jonathan Allday, Simon Hands

Published Sep 3, 2024• 0 citations
Publisher

Abstract

In the previous chapter, we set up a basic framework for exploring thermodynamics in a quantum regime. We have seen that constrained particles “in a box” have quantized energies (energy levels) specified by a quantum number that helps us to index microstates. Under appropriate and limited circumstances, we can model work done by a change in the energy values of the different levels while heating the system shuffles the pack in terms of the probability for occupying the levels. In this chapter, we proceed to fill in some vital details. The idea of an ensemble is formalized, and two of the key examples explored. We also derive the Boltzmann distribution in two complementary ways. Finally, we turn the quantum version of an ideal gas, and in the process derive a formula for the entropy. Our first task, however, is to discuss the issues pertinent to our ability to count microstates .

DOI
10.1201/9781003121053-10

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•Feb 22, 2022•0 citations
In the previous chapter, we set up a basic framework for exploring thermodynamics in a quantum regime. We have seen that constrained particles “in a box” have quantized energies (energy levels) specified by a quantum number that helps us to index microstates. Under appropriate and limited circumstances, we can model work done by a change in the energy values of the different levels while heating the system shuffles the pack in terms of the probability for occupying the levels. In this chapter, we proceed to fill in some vital details. The idea of an ensemble is formalized, and two of the key examples explored. We also derive the Boltzmann distribution in two complementary ways. Finally, we turn the quantum version of an ideal gas, and in the process derive a formula for the entropy. Our first task, however, is to discuss the issues pertinent to our ability to count microstates .
An energy level consists of all microscopic states of a system with the same energy. The energy levels of a system depend on the number of particles and the volume. At each instance in time, many different quantum states are represented in the various systems in the ensemble. A microcanonical ensemble describes an isolated system which has a fixed energy, volume and number of particles. The chapter describes certain relationships between fluctuations in thermodynamical variables and some other thermodynamical entities. One case of particular interest is when each subsystem is composed of one single particle, for instance very weakly interacting particles adsorbed on a surface or the particles in an ideal gas. The chapter presents more strict derivations of the probability expressions in the canonical, isobaric-isothermal and grand canonical ensembles. Volume and number of particles can also be considered as being mechanical variables. Entropy and temperature are examples of nonmechanical variables.
We found in the previous chapter that the molecular partition function is required to determine the thermodynamic properties of an ideal gas. To evaluate the partition function, specification of pertinent energy levels and degeneracies is necessary. Such knowledge demands that we investigate at least the rudiments of quantum mechanics, and especially those quantum concepts required for subsequent applications to statistical thermodynamics. For this reason, we concentrate in the next few chapters on the Schrödinger wave equation, whose various solutions provide the ε j 's and g j 's needed for the eventual calculation of thermodynamic properties. Depending on your academic background, you might thus consider reviewing classical mechanics (Appendix G) and operator theory (Appendix H) in preparation for your upcoming study of quantum mechanics. We begin this chapter with a historical review of the developments leading to the formulation of quantum mechanics, subsequently focusing on the Bohr model for atomic hydrogen and the de Broglie hypothesis for matter waves. We then introduce the Schrödinger wave equation, the basic postulates of quantum mechanics, and salient insights from these postulates germane to the development of statistical thermodynamics. We next apply the Schrödinger wave equation to the translation energy mode of an atom or molecule. This application conveniently explains both quantum states and quantum numbers, including their relation to our previous notions of microstate and macrostate. We end this chapter by discussing the Heisenberg uncertainty principle, including its utility in defining indistinguishability and symmetry conditions for multiparticle systems.
This is a book about techniques, and the first few chapters are about the techniques you have to learn before you can learn the real techniques. Your mastery of these crucial chapters will be presumed in subsequent ones. So go though them carefully, paying special attention to exercises whose answers are numbered equations. I begin with a review of basic ideas from thermodynamics and statistical mechanics. Some books are suggested at the end of the chapter [1–4]. In the beginning there was thermodynamics. It was developed before it was known that matter was made of atoms. It is notorious for its multiple but equivalent formalisms and its orgy of partial derivatives. I will try to provide one way to navigate this mess that will suffice for this book. Energy and Entropy in Thermodynamics I will illustrate the basic ideas by taking as an example a cylinder of gas, with a piston on top. The piston exerts some pressure P and encloses a volume V of gas. We say the system (gas) is in equilibrium when nothing changes at the macroscopic level. In equilibrium the gas may be represented by a point in the (P , V) plane. The gas has an internal energy U . This was known even before knowing the gas was made of atoms. The main point about U is that it is a state variable : it has a unique value associated with every state, i.e., every point (P , V) . It returns to that value if the gas is taken on a closed loop in the (P , V) plane. There are two ways to change U . One is to move the piston and do some mechanical work, in which case dU = –PdV by the law of conservation of energy. The other is to put the gas on a hot or cold plate. In this case some heat δQ can be added and we write dU = δQ which acknowledges the fact that heat is a form of energy as well. The first law of thermodynamics simply expresses energy conservation: dU = δQ – PdV . I use δQ and not dQ since Q is not a state variable.
This chapter builds upon the previous chapters, applying the method of combining probability theory with Hamiltonian mechanics. To do so, one needs to build a meaningful sample space over states, in this case, quantum states. A substantial part of the chapter discusses how to construct these quantum states out of which one can build a sample space on which to apply a probability measure. Vector states and density operators are introduced and various worked examples are proposed. Once the quantum sample space is identified, the equilibrium quantum statistical mechanics is formulated. The ‘particle in a box’ problem turns out to be analytically intractable, unless we take a certain limit called the semi-classical limit. Heuristics as to what this limit means are proposed. Finally, the von Neumann (quantum) entropy is introduced and analogies with thermodynamics are made. An application to the heat capacity of solids is presented. As complement, the chapter also introduces a classical ‘ring-polymer’ analog of quantum statistical mechanics stating the formal equivalence between a one-particle quantum canonical system and an N-particle classical canonical system.
Thermodynamic probability Ω is defined as the number of alternative microscopic arrangements which correspond to the same macroscopic state.Thermodynamic probability Ω enables us to decide how much more probable certain situations are than others.The method of determining the number of microstates for a given macrostate decides the statistics, Bose-Einstein or Fermi-Dirac statistics; quantum or classical!The distribution of the particles in different microstates is demonstrated through animation with the help of computer graphics.
Shannon’s entropy: -k Sum over i P(i) ln(P(i)) is expressed in terms of P(i) the probability for state i. If entropy exists as a concept separated from the first law of thermodynamics with dWork=0, then it is not clear what set of states i should be taken in quantum mechanics. In classical statistical mechanics, each particle is automatically described by its position and momentum vectors for no internal motion. For example a pure energy eigenstate wavefunction Wn(x) may be written in terms of many different orthonormal mathematical basis sets e.g. Wn(x)= Sum over i bi phi(i)(x) with probabilities bi*bi. Thus one may create many types of entropy expressions using Shannon’s form without any other physical considerations. For example, W(x)=Sum over p a(p)exp(ipx) and one may create Sp which is usually done in the literature. In previous notes we have argued that Sn = Sp(n)+Sx(n). For a particle in a box with infinite potential walls, Sx(n)=Sx. The sum of the two entropies ensures that the parameter L (box size) vanishes so that a quantum adiabatic transformation is isentropic. Thus a consideration other than Shannon’s form has been used to obtain Sn=Sp(n)+Sx for a particle in a box. Furthermore one may argue Shannon’s form even for a pure state based on S=S1+S2 where 1 and 2 represent two systems. A question still remains: Why are Sx and Sp entropies used and not some other set? Furthermore for a system with several energy levels ei one might ask why -Sum over i P(ei)ln(P(ei)) is used as in (1)? In a previous note (2) we considered that Shannon’s form of entropy follows from dE= TdS (dWork=0) with dE=Sum over i ei dP(ei). Furthermore we argued that P(ei) = C(T)exp(-ei/T) is a solution, but so is C(T) exp(-ei/T) exp(Si) where Si=Sx,i + Sp,i for the pure bound state. In other words, specific states related to the physical situation are chosen and entropy constructed from dE=TdS to reflect this. In this note we argue that entropy may be less related to counting arrangements than to considering the issues involved in energy transfers within a system.