无机化学双语教学 参考资料(上册)

班 级：050911 指导教师：夏 平 教 师：吕春燕 Main Contents of Inorganic Chemistry: Ⅰ Theory (first term) Equilibrium: chemical equilibrium (base); dissociation equilibrium; precipitation and dissolution equilibrium;

hydrolysis equilibrium; redox equilibrium; complexing equilibrium. Structure: atomic structure; molecular structure; crystal structure.

Ⅱ Element chemistry (second term) the properties, preparations and

applications of elements and compounds

Chapter One Mass Relationship and Energy Relationship in Chemical Reaction

Central contents: 1. Understand the concepts of state function、heat、work、enthalpy and change in enthalpy; 2. Know well how to write chemical equations and how to use Hess’s Law; 3. Use standard molar enthalpy of formation to calculate chemical enthalpy of reaction

Section One Basic Concepts

1.Thermochemistry, thermodynamics Thermochemistry: the study of the quantitative relationship between heat and other energy in chemical reactions Thermodynamics: the study of the conversion and transfer of incidental energy in chemical or physical changes 2.System and surroundings When we analyze energy changes, we focus our attention on a limited and well-defined part of the universe. The portion we single out for study is called the system, everything else is called the surroundings. There are three types of systems: Open system can exchange mass and energy (usually in the form of heat) with its surroundings. Closed system allows the transfer of energy (heat) but no mass. Isolated system does not allow the transfer of either mass or energy 3.State function A property of a system that is determined by specifying its condition or its state (in terms of temperature, pressure, location, and so forth). The value of a state function does not depend on the particular history of the sample, only depends on its present condition. For example: U, n, T, V and p are said to be state functions - properties that are determined by the state the system is in. pV = nRT R: molar gas constant(8.314 J·K-1·mol-1) Characteristics: 1). When the system’s state is specified, we can give a state function a certain value. 2). When the system’s state is changed, the value of a state function only depends on its initial state and final state, doesn’t depend on the particular history of the system. 3). When the system comes back to the beginning state, the value of a state function will return to the initial magnitude.

4. Heat and work Energy is transferred in two general ways: to cause the motion of an object against a force or to cause a temperature change. Heat is the energy transferred from a hotter object to a colder one (between system and surroundings because different temperature). It is symbolized by symbol Q. Work is the other way energy is transferred between system and surroundings. It is symbolized by symbol W. The SI unit of Q or W is J (1J=1kg.m2/s2) pv work: the work transferred between system and surroundings as the volume of system is changed. W = -p (V2 – V1) = -p∆V So W (expand)<0 W (compress)>0 Note: Q and W are not state functions Symbol and units: Units: kJ, J Heat absorbed by the system from the surroundings Q>0 positive (endothermic process) Heat absorbed by the surroundings from the system Q<0 negative (exothermic process) Work done by system on the surroundings W<0 negative Work done on system by the surroundings W>0 positive 5. Thermodynamic energy(internal energy) The internal energy of a system has two components: kinetic energy and potential energy. The kinetic energy consists of various types of molecular motion and the movement of electrons within molecules. Internal energy is symbolized by symbol U (a state function), so in a system, the value of ∆U only depends on its initial state and final state, doesn’t depend on the particular variational process.

∆U = Ufinal - Uinitial =U2 – U1 If U2 >U1 ∆U>0 system has gained energy from its surroundings or heat is absorbed If U2 < U1 ∆U<0 system has lost energy to surroundings or heat is given off 6. Law of conservation of energy All forms of energy can be changed (at least in principle) from one form to another. We have also seen that energy can be transferred back and forth between a system and its surroundings in the forms of work and heat. One of the most important observations is that although energy can assume many different forms, energy can be neither created nor destroyed. When one form of energy disappears, some other forms of energy (of equal magnitude) must appear, and vice versa. The total quantity of energy in the universe is thus assumed to remain constant. This statement is generally known as the law of conservation of energy. The first law of thermodynamics describes the conservation of energy; it states that energy can be converted from one form to another, but cannot be created or destroyed. The algebraic expression of first law of thermodynamics is: ∆U = Q + W. The signification is in a closed system, when it undergoes any chemical or physical change, the accompanying change in its internal energy, ∆U, is given