专业英语电子版教材.doc

注意事项 2
专业英语课程简介 2
Chapter 1 Matter and Measurement 3
1.1. Classification of Matter 3
1.2. Properties of Matter 4
1.3 Atoms, Molecules and Compounds 5
1.4. Numbers in Physical Quantities 6
1.5 Units of Measurement 8
1.6 The Dimensional Method 12
Word and sentence: 12
Chapter 2 Nomenclature of Inorganic Chemistry 13
2.1 Chemical Language 13
2.2 Nomenclature of Elements 14
2.3 Nomenclature of Inorganic Compounds 21
Chapter 3 Inorganic Chemistry 28
3.1 The Atomic Nature of Matter 28
3.2 Electronic Structure of Atoms 30
3.3 Periodicity of Atomic Properties 33
3.5 Molecular Geometry and Bonding Theories 37
3.6 Chemical Reactions 39
3.7 The Behavior of Gases 41
3.8 Aqueous Reactions and Solution Stoichiometry 43
3.9 Chemical Equilibrium 44
3.10 Thermochemistry 45
3.11 Acid-Base Equilibria 47
3.12 Additional Aspects of Aqueous Equilibria 49
3.13 Chemistry of Coordination Compounds 50
3.14 Nuclear Chemistry 52
《专业英语》教学大纲 54
语言不相同 culture shock normal university 54
Decrease and increase 55
descend 55
-ium 55
Ratio of … to … 56
Be derived from 56
虚拟条件句 56
Concern 57
available 57
常用简写 58
Involve 59
though 59
Bound 60
available 61
高分子化学专业英语.rar 62
By means of (lesson12) ( by all means，by no means lesson 5 63
ability/ be able to/ be capable of/can 关于「能力」的表达方式 63
As such such as 66
因果关系 67
形式主语 It is + adj.+ to 67
科技论文的结构Full Paper (lesson 12) 68
As 引出宾语补语、主语补语(complement 补语) return Lesson 11 69
According to 按照，与…相应 70
Whether与if的区别 Lesson 13 70
Ratio …to… 71
绝佳中英文翻译 2010-03-15 72
Chinglish 72
交通大学 2010-03-08讲 73
方便 2010-09-16 73
不折腾 2010-03-15 73
你的英语够老外吗？ 74
Humor 幽默 76
常用英语标识语 77
错误英文标示 81
use is made of 82
Culture shock 82
外国的品牌的中国名，中国品牌的外国名 83
英语课堂练习 83
英语课堂用语100句 83
化学四门基础课 85
考试 86

注意事项

1． 音标显示 把Ksphonet.ttf放入 C:\WINDOWS\Fonts C:\Program Files\Kingsoft\PowerWord 2006\fonts 中找到 Ksphonet.ttf 考入 C:\WINDOWS\Fonts
2． 科技论文结构
3． 专利结构

1.

Chapter 1 Matter and Measurement

Chemistry is the science of matter and the changes it undergoes. Chemists study the composition, structure, and properties of matter. They observe the changes that matter undergoes and measure the energy that is produced or consumed during these changes. Chemistry provides an understanding of many natural events and has led to the synthesis of new forms of matter that have greatly affected the way we live.
Disciplines within chemistry are traditionally grouped by the type of matter being studied or the kind of study. These include inorganic chemistry, organic chemistry, physical chemistry, analytical chemistry, polymer chemistry, biochemistry, and many more specialized disciplines, e.g. radiochemistry, theoretical chemistry.
Chemistry is often called "the central science" because it connects the other natural sciences such as astronomy, physics, material science, biology and geology.

1.1. Classification of Matter
Matter is usually defined as anything that has mass and occupies space. Mass is the amount of matter in an object. The mass of an object does not change. The volume of an object is how much space the object takes up.
All the different forms of matter in our world fall into two principal categories: (1) pure substances and (2) mixtures. A pure substance can also be defined as a form of matter that has both definite composition and distinctSee note
properties. Pure substances are subdivided into two groups: elements and compounds. An element is the simplest kind of material with unique physical and chemical properties; it can not be broken down into anything simpler by either physical or chemical means. A compound is a pure substance that consists of two or more elements linked together in characteristic and definite proportions; it can be decomposed by a chemical change into simpler substances with a fixed mass ratio. Mixtures contain two or more chemical substances in variable proportions in which the pure substances retain their chemical identities. In principle, they can be separated into the component substances by physical means, involving physical changes. A sample is homogeneous if it always has the same composition, no matter what part of the sample is examined. Pure elements and pure chemical compounds are homogeneous. Mixtures can be homogeneous, too; in a homogeneous mixture the constituents are distributed uniformly and the composition and appearance of the mixture are uniform throughout. A solutions is a special type of homogeneous mixture. A heterogeneous mixture has physically distinct parts with different properties. The classification of matter is summarized in the diagram below:
Matter
Pure Substances
Mixtures
Elements
Compounds
Homogeneous mixtures
Heterogeneous mixtures

Matter can also be categorized into four distinct phases: solid, liquid, gas, and plasma. The solid phase of matter has the atoms packed closely together. An object that is solid has a definite shape and volume that cannot be changed easily. The liquid phase of matter has the atoms packed closely together, but they flow freely around each other. Matter that is liquid has a definite volume but changes shape quite easily. Solids and liquids are termed condensed phases because of their well-defined volumes. The gas phase of matter has the atoms loosely arranged so they can travel in and out easily. A gas has neither specific shape nor constant volume. The plasma phase of matter has the atoms existing in an excited state.
Break 2011-8-30 1st
1.2. Properties of Matter
All substances have properties, the characteristics that give each substance its unique identity. We learn about matter by observing its properties. To identify a substance, chemists observe two distinct types of properties, physical and chemical, which are closely related to two types of change that matter undergoes.
Physical properties are those that a substance shows by itself, without changing into or interacting with another substance. Some physical properties are color, smell, temperature, boiling point, electrical conductivity, and density. A physical change is a change that does not alter the chemical identity of the matter. A physical change results in different physical properties. For example, when ice melts, several physical properties have changed, such as hardness, density, and ability to flow. But the sample has not changed its composition: it is still water.
Chemical properties are those that do change the chemical nature of matter. A chemical change, also called a chemical reaction, is a change that does alter the chemical identity of the substance. It occurs when a substance (or substances) is converted into a different substance (or substances). For example, when hydrogen burns in air, it undergoes a chemical change because it combines with oxygen to form water.
Separation of Mixtures
The separation of mixtures into its constituents in a pure state is an important process in chemistry. The constituents of any mixture can be separated on the basis of their differences in their physical and chemical properties e.g., particle size, solubility, effect of heat, acidity or basicity etc.
Some of the methods for separation of mixtures are:
(1) Sedimentation or decantation. To separate the mixture of coarse particles of a solid from a liquid e.g., muddy river water.
(2) Filtration. To separate the insoluble solid component of a mixture from the liquid completely i.e. separating the precipitate (solid phase) from any solution.
(3) Evaporation. To separate a non-volatile soluble salt from a liquid or recover the soluble solid solute from the solution.
(4) Crystallization. To separate a solid compound in pure and geometrical form.
(5) Sublimation. To separate volatile solids, from a non-volatile solid.
(6) Distillation. To separate the constituents of a liquid mixture, which differ in their boiling points.
(7) Solvent extraction method. Organic compounds, which are easily soluble in organic solvents but insoluble or immiscible with water forming two separate layers can be easily separated.
1.3 Atoms, Molecules and Compounds
The fundamental unit of a chemical substance is called an atom. The word is derived from the Greek atomos, meaning “undivisible” or “uncuttable”. An atom is the smallest possible particle of a substance.
Molecule is the smallest particle of a substance that retains the chemical and physical properties of the substance and is composed of two or more atoms; a group of like or different atoms held together by chemical forces. A molecule may consist of atoms of a single chemical element, as with oxygen (O2), or of different elements, as with water (H2O).
A chemical element is a pure chemical substance consisting of one type of atom distinguished by its atomic number, which is the number of protons in its nucleus. The term is also used to refer toSee 定义
a pure chemical substance composed of atoms with the same number of protons. Until March 2010, 118 elements have been observed. 94 elements occur naturally on earth, either as the pure element or more commonly as a component in compounds. 80 elements have stable isotopes, namely all elements with atomic numbers 1 to 82, except elements 43 and 61 (technetium and promethium). Elements with atomic numbers 83 or higher (bismuth and above) are inherently unstable, and undergo radioactive decay. The elements from atomic number 83 to 94 have no stable nuclei, but are nevertheless found in nature, either surviving as remnants of the primordial stellar nucleosynthesis that produced the elements in the solar system, or else produced as short-lived daughter-isotopes through the natural decay of uranium and thorium. The remaining 24 elements so are artificial, or synthetic, elements, which are products of man-induced processes. These synthetic elements are all characteristically unstable. Although they have not been found in nature, it is conceivable that in the early history of the earth, these and possibly other unknown elements may have been present. Their unstable nature could have resulted in their disappearance from the natural components of the earth, however.
The naturally occurring elements were not all discovered at the same time. Some, such as gold, silver, iron, lead, and copper, have been known since the days of earliest civilizations. Others, such as helium, radium, aluminium, and bromine, were discovered in the nineteenth century. The most abundant elements found in the earth’s crust, in order of decreasing percentage, are oxygen, silicon, aluminium, and iron. Others present in amounts of 1% or more are calcium, sodium, potassium, and magnesium. Together, these represent about 98.5% of the earth’s crust.
The nomenclature and their origins of all known elements will be described in Chapter 2.
A chemical compound is a pure chemical substance consisting of two or more different chemical elements that can be separated into simpler substances by chemical reactions. Chemical compounds have a unique and defined chemical structure; they consist of a fixed ratio of atoms that are held together in a defined spatial arrangement by chemical bonds. Compounds that exist as molecules are called molecular compounds. An ionic compound is a chemical compound in which ions are held together in a lattice structure by ionic bonds. Usually, the positively charged portion consists of metal cations and the negatively charged portion is an anion or polyatomic ion.
The relative amounts of the elements in a particular compound do not change: Every molecule of a particular chemical substance containsSee 组成 构成
a characteristic number of atoms of its constituent elements. For example, every water molecule contains two hydrogen atoms and one oxygen atom. To describe this atomic composition, chemists write the chemical formula for water as H2O.
The chemical formula for water shows how formulas are constructed. The formula lists the symbols of all elements found in the compound, in this case H (hydrogen) and O (oxygen). A subscript number after an element's symbol denotes how many atoms of that element are present in the molecule. The subscript 2 in the formula for water indicates that each molecule contains two hydrogen atoms. No subscript is used when only one atom is present, as is the case for the oxygen atom in a water molecule. Atoms are indivisible, so molecules always contain whole numbers of atoms. ConsequentlyAccordingly，as a result，hence，therefore
, the subscripts in chemical formulas of molecular substances are always integers. We explore chemical formulas in greater detail in Chapter 2.
The simple formula that gives the simplest whole number ratio between the atoms of the various elements present in the compound is called its empirical formula. The simplest formula that gives the actual number of atoms of the various elements present in a molecule of any compound is called its molecular formula. Elemental analysis is an experiment that determines the amount (typically a weight percent) of an element in a compound. The elemental analysis permits determination of the empirical formula, and the molecular weight and elemental analysis permit determination of the molecular formula.

1.4. Numbers in Physical Quantities
1.4.1. Measurement
1. Physical Quantities
Physical properties such as height, volume, and temperature that can be measured are called physical quantity. A number and a unit of defined size are required to describe physical quantity, for example, 10 meters, 9 kilograms.
2. Exact Numbers
Exact Numbers are numbers known with certainty. They have unlimited number of significant figures. They arise by directly counting numbers, for example, the number of sides on a square, or by definition:
1 m = 100 cm, 1 kg = 1000 g
1 L = 1000 mL, 1 minute = 60 seconds
3. Uncertainty in Measurement
Numbers that result from measurements are never exact. Every experimental measurement, no matter how precise, has a degree of uncertainty to it because there is a limit to the number of digits that can be determined. There is always some degree of uncertainty due to experimental errors: limitations of the measuring instrument, variations in how each individual makes measurements, or other conditions of the experiment.
Precision and Accuracy
In the fields of engineering, industry and statistics, the accuracy of a measurement system is the degree of closeness of measurements results to its actual (true) value. The precision of a measurement system, also called reproducibility or repeatability, is the degree to which repeated measurements under unchanged conditions show the same results. Although the two words can be synonymous in colloquial use, they are deliberately contrasted in the context of the scientific method.
A measurement system can be accurate but not precise, precise but not accurate, neither, or both. A measurement system is called valid if it is both accurate and precise. Related t