化学专业英语

专业英语词汇Unit 1TEXT A ： Chemical Reactions and Group Reactionscustomary a. 通常的，惯例的handle n.柄vt.触摸handling n.处理，管理derive vt.取得，得到，衍生oxidate vt.使氧化oxidation n.satisfactory a.令人满意的，符合要求的rapid a.快的，迅速的，动作快的combustion n.燃烧somewhat pron. ad. 一点点，几分，有点effort n.努力commercial a.商业的，商务的undesirable a不.合需要的，不受欢迎的，讨厌的retard vt.延迟，放慢，使停滞transformer n.变压器transform vt.改变，转变automotive a.自动的，机动的，汽车的cracked裂化的sluge n.软泥，淤泥stiff a.硬的，强烈的extent 广度，程度distillation n.蒸馏distill vt.vi.unrefined a.未精致，未提炼的acidity n.酸味，酸性acidify vt. Vi.Involve vt. 包缠，卷缠Fell=followingIndividual a.个人的，个体的Presumable a可.假定的，可推测的Destruction n.破坏，毁灭Overall n。

a.全面的，综合的Exceed 超过，胜过Isolate vt.隔离，孤立，使离析iso—构词成分“均匀”“异构”“苯”Analyse vt. 分析，分解Carbonyl 羰基Carboxyl羧基Hydroxyl羟基Decomposition分解Alkyl烷基，烃基Ketone 酮Aldehyde n.醛Yield vt. 出产，产出Explosive a. 爆炸Vapor n.蒸汽， vi.蒸发Propagation 繁殖，增殖；传播Dehydrate vt.使脱水Acet 构词成分Acetaldehyde乙醛Resin n.树脂Resinous a.树脂的Carboxylic a.羟基的Substantial a.物质的，实质的Susceptible a易.受感动的，敏感的Analogous a.类似的，相似的（ to）Response n.作答，回答，响应，反应Readily ad.乐意地，很快地Readiness n准.备就绪，愿意Extent n.广度长度Steric 空间的，位的Likewise ad.同样的，照样地；也，又Suffer vt.遭受，经历Progressive a进.步的，长进的，渐次的Adjacent a.邻近的，紧挨着的Terminal a.末端的，终点的MethyleneBromide n.溴化物Substitute n.代替物（人），代用品substitution n.代替，替换Remote a相.隔较远的Acetone n.丙酮Ether n.醚，乙醚Correspond vi.符合，一致；相当，相应Reservation n保.留，预定Tend vi.走向，趋向。

化学专业英语词汇表本文介绍了化学专业需要用到的英语词汇，包括基础的化学术语、常用的化学分支、常用的化学实验和常用的化学反应。

文章采用表格形式列出了中文和英文对照的词汇，并给出了一些例句和注释，以便于理解和记忆。

文章的目的是帮助化学专业的学生和研究者提高英语水平，更好地阅读和撰写化学相关的文献和报告。

一、基础化学术语中文英文例句或注释化学chemistry Chemistry is the science of matter and its transformations. 化学是研究物质及其变化的科学。

元素element An element is a substance that cannot be decomposed into simpler substances bychemical means. 元素是一种不能通过化学手段分解为更简单物质的物质。

原子atom An atom is the smallest unit of an element that retains the chemical properties of thatelement. 原子是元素的最小单位，保持了该元素的化学性质。

原子核nucleus The nucleus is the central part of an atom, containing protons and neutrons. 原子核是原子的中心部分，包含了质子和中子。

质子proton A proton is a positively charged subatomic particle, found in the nucleus of an atom. 质子是一种带正电的亚原子粒子，存在于原子核中。

中子neutron A neutron is a neutrally charged subatomic particle, found in the nucleus of an atom. 中子是一种不带电的亚原子粒子，存在于原子核中。

☆常用： ppm: parts per millionppb: parts per billion pH: potential of hydrogen1. 化合物的命名：规则：金属(或某些非金属)元素+阴离子名称(1)MgCl2 magnesium [mæɡ’ni:zj əm] chloride (2)NaNO2 sodium nitrite [‘naitrait](3)KNO3 potassium[p ə’tæsi əm] nitrate [‘naitreit] (4)硝酸 nitric acid(5)NaHCO3 sodium hydrogen carbonate练习：▪ FeBr2 ▪ (NH4)2SO4 ▪ NH4H2PO4▪KMnO4▪亚硫酸▪sulfurous acid▪H2S▪NO2 有机物命名▪Hydrocarbon▪{Aliphatic hydrocarbon; Aromatic Hydrocarbon}▪Aliphatic hydrocarbon (脂肪烃)▪{Alkane (烷); Alkene(烯); Alkyne(炔)}▪Alcohol 醇▪Aldehyde 醛▪Ketone [‘ki:təun] 酮▪Carboxylic acid 羧酸▪Aromatic hydrocarbon(芳香烃)▪{benzene (苯) hydroxybenzene(酚) quinone(醌)无机物中关于数字的写法mono-, di-, tri-, tetra-, penta- hexa-, hepta-, octa-, nona-, deca-一，二，三，四，五，六，七，八，九，十有机物中关于数字的写法meth-, eth-, prop-, but-, pent-, hex-,甲乙丙丁戊已hept-, oct-, non-, dec-, cyclo-, poly-庚辛壬葵环聚练习▪甲烷乙炔▪丙酮丁醇▪戊烷己烯▪庚醛辛烷▪2-甲基壬酸 3,5-二乙基癸醇Lithium [‘liθiəm] n.锂Beryllium [bə’riljəm] n.铍(Be)Sodium [‘səudiəm] n.钠Potassium [pə’tæsiəm] 钾Rubidium [ru:’bidiəm] 铷Caesium [‘si:ziəm] 铯Nucleus[‘nju:kli s] 原子核，是nuclear的复数Halogen[‘hælədʒən] 卤素general chemistry 普通化学positive[‘pƆzətiv] ion 阳离子orbital electron 轨道电子effective nuclear charge 有效核电荷atomic radius 原子半径，raddi的复数ionic radius 离子半径negative ion 阴离子electron cloud 电子云Van der Waals non-bounded radius单质分子晶体中相邻分子间两个非键合原子核间距离的一半称为范德华半径metallic [mi’tælik] character[‘kæriktə] 金属特性electropositive [I’lektrəu’pɔzətiv] a.带正电的Ionization [‘aiənai’zeiʃən] energy 电离能carbon 碳 germanium[dʒə:’meiniəm] 锗tin [tin] 锡 lead [led] 铅sodium[‘səudiəm] 钠 magnesium[mæɡ’ni:zjəm] 镁silicon [‘silikən] 硅 chlorine [’klɔ:ri:n] 氯nonmetallic [‘nɔnmi’tælik]adj.n.非金属的，非金属Electronegativity 电负性Metallic oxide 金属氧化物Metallic hydroxide [hai’drɔksaid] 金属氢氧化物Hydroxyl [hai‘drɔksil] ions 氢氧根离子insoluble[in’sɔljubl] 不溶解的Ionic [ai‘ɔnik] adj. 离子的Transition element 过渡元素Basicity [bə’sisiti] n. 碱性，碱度Oxyacid [,ɔksi’æsid] 含氧酸Carbonate [‘kɑ:bəneit] 碳酸盐Nitrate [‘naitreit] 硝酸盐Sulphate [‘sʌlfeit] 硫酸盐 = sulfateAmphoteric [,æmfə’terik] adj.两性的Acid [‘æsid] n. adj.alkali [‘ælkəlai] n.adj.Hydration [hai’dreiʃən] 水合作用Hydrolyze [‘haidrəlaiz] vi. 水解Oxysalt [‘ɔksisɔ:lt] 含氧酸盐Complex 络合物，复合物句子理解1) Metals are electropositive and have a tendency to loss electrons, if suppliedwith energy: M M+ + e. 金属是电正性的，如果供给能量，有失去电子的趋势。

Chapter 1 Matter and MeasurementChemistry 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 MatterMatter 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 distinct 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 fixedmass 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 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.1.2. Properties of MatterAll 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 MixturesThe 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 separatethe mixture of coarse particles of a solidfrom a liquid e.g., muddy river water.(2)Filtration. To separate the insoluble solidcomponent of a mixture from the liquidcompletely i.e. separating the precipitate(solid phase) from any solution.(3)Evaporation. To separate a non-volatilesoluble salt from a liquid or recover thesoluble solid solute from the solution.(4)Crystallization. To separate a solidcompound in pure and geometrical form.(5)Sublimation. To separate volatile solids,from a non-volatile solid.(6)Distillation. To separate the constituents of aliquid mixture, which differ in their boilingpoints.(7)Solvent extraction method. Organiccompounds, which are easily soluble inorganic solvents but insoluble or immisciblewith water forming two separate layers canbe easily separated.1.3 Atoms, Molecules and CompoundsThe 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 to 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 nucleosynthesisthat 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 contains acharacteristic 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. Consequently, 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 Quantities1.4.1. Measurement1.Physical QuantitiesPhysical 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 NumbersExact Numbers are numbers known withcertainty. 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 g1 L = 1000 mL, 1 minute = 60seconds3.Uncertainty in MeasurementNumbers 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 AccuracyIn 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 terms are bias (non-random or directed effects caused by a factor or factors unrelated by the independent variable) and error(random variability), respectively. Random errors result from uncontrolled variables in an experiment and affect precision; systematic errors can be assigned to definite causes and affect accuracy. For example, if an experiment contains a systematic error, then increasing the sample size generally increases precision but does not improve accuracy. Eliminating the systematic error improves accuracy but does not change precision.1.4.2 Significant FiguresThe number of digits reported in a measurement reflects the accuracy of the measurement and the precision of the measuring device. Significant figures in a number include all of the digits that are known with certainty, plus the first digit to the right that has an uncertain value. For example, the uncertainty in the mass of a powder sample, i.e., 3.1267g as read from an “analytical balance” is 0.0001g.In any calculation, the results are reported to the fewest significant figures (for multiplication and division) or fewest decimal places (addition and subtraction).1.Rules for deciding the number of significantfigures in a measured quantity:The number of significant figures is found by counting from left to right, beginning with the first nonzero digit and ending with the digit that has the uncertain value, e.g.,459 (3) 0.206 (3) 2.17(3) 0.00693 (3) 25.6 (3) 7390 (3) 7390. (4)(1)All nonzero digits are significant, e.g., 1.234g has 4 significant figures, 1.2 g has 2significant figures.(2)Zeroes between nonzero digits aresignificant: e.g., 1002 kg has 4 significantfigures, 3.07 mL has 3 significant figures.(3)Leading zeros to the left of the first nonzerodigits are not significant; such zeroes merelyindicate the position of the decimal point:e.g., 0.001 m has only 1 significant figure,0.012 g has 2 significant figures.(4)Trailing zeroes that are also to the right of adecimal point in a number are significant:e.g., 0.0230 mL has 3 significant figures,0.20 g has 2 significant figures.(5)When a number ends in zeroes that are notto the right of a decimal point, the zeroes arenot necessarily significant: e.g., 190 milesmay be 2 or 3 significant figures, 50,600calories may be 3, 4, or 5 significant figures.The potential ambiguity in the last rule can be avoided by the use of standard exponential, or "scientific" notation. For example, depending onwhether the number of significant figures is 3, 4, or 5, we would write 50,600 calories as:5.06 × 104 calories (3 significant figures)5.060 ×104calories (4 significant figures), or5.0600 × 104 calories (5 significant figures).2.Rules for rounding off numbers(1)If the digit to be dropped is greater than 5,the last retained digit is increased by one.For example, 12.6 is rounded to 13.(2)If the digit to be dropped is less than 5, thelast remaining digit is left as it is. Forexample, 12.4 is rounded to 12.(3)If the digit to be dropped is 5, and if anydigit following it is not zero, the lastremaining digit is increased by one. Forexample, 12.51 is rounded to 13.(4)If the digit to be dropped is 5 and isfollowed only by zeroes, the last remainingdigit is increased by one if it is odd, but leftas it is if even. For example, 11.5 is roundedto 12, 12.5 is rounded to 12.This rule means that if the digit to be dropped is 5 followed only by zeroes, the result is always rounded to the even digit. The rationale is to avoid bias in rounding: half of the time we round up, half the time we round down.3.Arithmetic using significant figuresIn carrying out calculations, the general rule is that the accuracy of a calculated result is limited by the least accurate measurement involved in the calculation.(1) In addition and subtraction, the result is rounded off to the last common digit occurring furthest to the right in all components. Another way to state this rules, is that, in addition and subtraction, the result is rounded off so that it has the same number of decimal places as the measurement having the fewest decimal places. For example,100 (assume 3 significant figures) + 23.643 (5 significant figures) = 123.643,which should be rounded to 124 (3 significant figures).(2) In multiplication and division, the resultshould be rounded off so as to have the same number of significant figures as in the component with the least number of significant figures. For example,3.0 (2 significant figures ) ×12.60 (4 significant figures) = 37.8000which should be rounded off to 38 (2 significant figures).1.4.3 Scientific NotationScientific notation, also known as standard form or as exponential notation, is a way of writing numbers that accommodates values too large or small to be conveniently written in standard decimal notation.In scientific notation all numbers are written like this:a × 10b("a times ten to the power of b"), where the exponent b is an integer, and the coefficient a is any real number, called the significant or mantissa (though the term "mantissa" may cause confusion as it can also refer to the fractional part of the common logarithm). If the number is negative then a minus sign precedes a (as in ordinary decimal notation).In standard scientific notation the significant figures of a number are retained in a factor between 1 and 10 and the location of the decimal point is indicated by a power of 10. For example:An electron's mass is about 0.00000000000000000000000000000091093822 kg. In scientific notation, this is written 9.1093822×10−31 kg.The Earth's mass is about 5973600000000000000000000 kg. In scientific notation, this is written 5.9736×1024 kg.1.5 Units of Measurement1.5.1 Systems of Measurement1.United States Customary System (USCS)The United States customary system (also called American system) is the most commonly used system of measurement in the United States. It is similar but not identical to the British Imperial units. The U.S. is the only industrialized nation that does not mainly use the metric system in its commercial and standards activities. Base units are defined butseem arbitrary (e.g. there are 12 inches in 1 foot)2.MetricThe metric system is an international decimalized system of measurement, first adopted by France in 1791, that is the common system of measuring units used by most of the world. It exists in several variations, with different choices of fundamental units, though the choice of base units does not affect its day-to-day use. Over the last two centuries, different variants have been considered the metric system. Metric units are universally used in scientific work, and widely used around the world for personal and commercial purposes. A standard set of prefixes in powers of ten may be used to derive larger and smaller units from the base units.3.SISI system (for Système International) was adopted by the International Bureau of Weights and Measures in 1960, it is a revision and extension of the metric system. Scientists and engineers throughout the world in all disciplines are now being urged to use only the SI system of units.1.5.2 SI base unitsThe SI is founded on seven SI base units for seven base quantities assumed to be mutually independent, as given in Table 1.1.Table 1.1 SI Base Physical Quantities and UnitsU n i tN a m e UnitSymbolBaseQuantityQuantitySymbolDimensionSymbolm m l l Le t e r e n g t hk i lo g r a m kgmassm Ms ec o nd stimet Ta mp e r e AelectriccurrentI Ik el v i n KthermodynTΘm i ct e m p e r a t u r em o l e molamountofsubstancen Nc an d e l a cdluminousIvJntensity1.5.3 SI derived unitsOther quantities, called derived quantities, aredefined in terms of the seven base quantities via asystem of quantity equations. The SI derived unitsfor these derived quantities are obtained from theseequations and the seven SI base units. Examples ofsuch SI derived units are given in Table 1.2, where itshould be noted that the symbol 1 for quantities ofdimension 1 such as mass fraction is generallyomitted.Table 1.2 SI Derived Physical Quantities and(symbol) Unit(symbol)UArea (A) squaremeterm V olume (V) cubicmeterm Density (ρ) kilogramper cubicmeterkVelocity (u) meterpersecondmPressure (p) pascal(Pa)kEnergy (E) joule (J) (k Frequency (ν) hertz(Hz)1Quantity of electricity (Q) coulomb(C)AElectromotive force (E) volt (V) (kmsForce (F) newton(N)kFor ease of understanding and convenience, 22SI derived units have been given special names andsymbols, as shown in Table 1.3.Table 1.3 SI Derived Units with special names andsymbolsD e r i v e dq u a n t i t y SpecialnameSpecialSymbolExpressionintermsofotherSIunitsSIbaseunitsp r r ml a n ea n g l e adianad·m-1=1s o l i da n g l e steradiansrm2·m-2=1f r e q u e n c y hertzHzs-1f o r c e newtonN m·kg·s-2p p P N mr e s s u r e ,s t r e s s ascala/m21·kg·s-2e n e r g y ,w o r k ,q u a n t i t yo fh e a jouleJ N·mm2·kg·s-2p o w e r ,r a d i a n tf l u x wattW J/sm2·kg·s-3e l e c t r i cc h a r g e q u a n t i t y coulombC s·Afe l e c t r i c i t ye l e c t r i cp o t e n t i a l ,p o t e n t i a l voltV W/Am2·kg·s-3·A-1i f f e r e n c e ,e l e c t r o m o t i v ef o r c ec a p a c i t a n c e faradF C/Vm-2·kg-1·s 4·A 2e l e c t r i cr e s i s t a n c e ohmΩV/Am2·kg·s-3·A-2e l e c t r i cc o nd u c t a n c siemensS A/Vm-2·kg-1·s2·Aem a g n e t i cf l u x weberWbV·sm2·kg·s-2·A-1m a g n e t i cf l u xd e n s i t y teslaT Wb/m2kg·s-2·A-1i n d henH Wb/m2u c t a n c e ryA ·kg·s-2·A-2C e l s i u st e m p e r a t u r e degreeCelsius°CKl u m i n o u s lumenlmcd·srcd·srl u xi l l u m i n a n c e luxlxlm/m2m-2·cd·sra c t i v i t y( o far a d i o n u c l i d e becquerelBqs-1a b s o r b e dd o se ,s p e c i f i ce n e r g y( i m p a r t e d ) ,grayGyJ/kgm2·s-2e r m ad o s ee q u i v a l e n t ,e ta l .sievertSvJ/kgm2·s-2c a t a l y t i ca c t i v i katalkats-1·molyCertain units that are not part of the SI are essential and used so widely that they are accepted by the CIPM (Commission Internationale des Poids Et Mesures) for use with the SI. Some commonly used units are given in Table 1.4.Table 1.4 Non-SI units accepted for use with theSIN a m e SymbolQuantityEquivalentSIunitmi n u t e mintime1min=6sho u r htime1h6min=36s da y dtime1d=24h=144min=864sdegreeo fa r c °planeangle1°=(π/18)radm i n u t eo fa r c ′planeangle1′=(1/6)°=(π/18radsecondo fa r c ″planeangle1″=(1/6)′=(1/36)°=(π/648)rdhect a r e haarea1ha=1a=1m²l i t r e lorLvolume1l=1dm3=.1m3ton n e tmass1t=13kg=1MgThe 20 SI prefixes used to form decimal multiples and submultiples of SI units are given in Table 1.5.Table 1.5 SI PrefixesF a c t o r NameSymbolFactorNameSymbol1 0 24yottaY 1-1decid1 0 21zettZ 1-2centc。

unite 1. Inorganic chemistry1.1 what is chemistry（1）. 重点专业词汇讲解：Chemical: adj . 化学的、化学药品Transformation: 变化，化学转变，转化Dye: n. 染料染色，或者vt. 染Charcoal: ['t ? ck??l] 木炭Cellulose : 纤维素细胞的['selj?l??z; ] Fat：n. 脂肪肥肉adj . 肥大的alkalis ：碱adj . 碱性的glycerin: 甘油丙三醇alkalis: n. 碱金属alloy: 合金使成合金bronze：青铜色的n. 青铜（铜和锡的合金）brass：[br a s] n.黄铜（铜和锌）要求学生会区别黄铜及青铜的不同翻译Poison：毒物毒药t.毒害放毒下毒Proton：n. 质子Nulei: n.核（nucleus 的复数形式）['njukl ??s]Identical : adj . 同一的Chirality n.手性手征和Handeness的区别Amino acid ：n. 氨基酸Ala nine: n.丙氨酸2. 课文中重点词组（phrase）Chemical change:化学变化physical change：物理变化Explore: 探险研究research investigate studyIsolate: 分离chemical bonds 化学键chemical reaction ：化学反应Natural substance 天然物质Coke : 焦炭carbon monoxide 一氧化碳Carbon Dioxide 二氧化碳Chemical bond 化学键fundamental principle 基本原理The periodic table of elements ：元素周期表numbers of protons 质子数atomic number 原子序数covalent bonds 共价键positive 正阳性negative 负阴性3. 课文中重点句子The first and most important principle is that chemical substances are made up of molecules in which atoms of various elements are linked in well-defined ways. 需要着重给学生讲解第一条也是最重要的原理是化学物质是有分子组成的，分子中的不同元素的原子是以一定的方式连接在一起的。

化学专业英语1、化学专业英语：一、无机化学术语1、periodic table 元素周期表2、electronic structure电子构型3、wavelength波长4、frequency频率5、wave number波数6、diffraction衍射7、quantum量子8、quantized量子化9、quantum theory量子理论10、photoelectric effect光电效应11、photon光子12、quantum mechanics量子力学13、Heisenberg uncertainty principle海森堡测不准原理14、momentum动量15、angular momentum角动量16、ground state基态17、excited states激发态18、quantum number量子数19、atomic orbital原子轨道20、the four quantum numbers四个量子数21、electron configuration电子构型22、Pauli exclusion principle泡利不相容原理23、Hund’s principle洪特规则24、paramagnetism顺磁性25、diamagnetism反磁性26、period周期27、noble gas惰性气体28、Representative elements代表性元素29、Transition elements过渡元素30、Metals金属31、nonmetals非金属32、semiconducting elements半导体元素33、chemical bond化学键34、valence electrons价电子35、Lewis symbol路易斯符号36、Chemical stability化学稳定性37、octet rule八隅体规则38、chemical reactivity化学反应性39、metallic bonding金属键40、ionic bonding 离子键41、Lewis structures路易斯结构42、nonbonding electron pairs(lone pairs)非成键电子对43、covalent bonding共价键44、single单键45、multiple(double,triple) and coordinate(donor atom and acceptor atom) covalent bond配位键46、resonance共振47、resonance hybrid共振杂化48、nonpolar and polar covalent bond非极性和极性共价键49、dipole偶极50、network covalent substances51、bond dissociation energy键解离能52、lattice energy点阵能，晶格能53、atomic radii原子半径54、effective nuclear charge有效核电荷55、screening effect屏蔽效应56、Scanning 扫描57、Lanthanide contraction镧系收缩58、isoelectronic ions等电子离子59、ionization energy电离能60、noble gas configuration惰性气体构型61、electron affinity电子亲和能62、pseudo-noble gas configuration稀有气体原子实63、polarization of an ion离子极化64、electronegativity电负性65、electronegative atom电正性原子66、electropositive atom电负性原子67、Oxidation numbers氧化值68、Oxidation state氧化态69、molecular geometry分子几何70、bond axis键轴71、valence bond theory价键理论72、hybridization杂化73、isomers异构体74、structural isomers结构异构75、delocalized electrons离域电子76、dipole moment偶极矩77、London bond色散力78、nuclide核素79、nucleons核子80、mass defect质量缺陷81、nuclear binding energy核结合能82、nuclear fusion核聚变83、nuclear fission核裂变84、radioactivity放射性85、radionuclides放射性核素86、magic number幻数87、bombardment reaction轰击反应88、antineutrino反中微子89、neutrino中微子90、positron正电子（阳电子）91、electron capture电子捕获92、chain reaction链式反应93、crtical mass临界质量94、nuclear reaction 核反应95、thermonuclear reactions热核反应96、breeder reactor增殖反应97、hydration水合98、solvation溶剂化99、chemical equilibrium化学平衡100、hydrolysis水解101、hydrates水合物102、efflorescence风化物103、hygroscopic 吸湿104、deliquescence潮解105、electrolytes电解质106、strong（weak）electrolytes强电解质107、nonelectrolytes非电解质108、acidic（alkaline）aqueous solution109、polyprotic acids多元酸110、neutralization中和反应111、complex ion络合离子112、ligands配体113、hard water 硬水114、carbonate hardness碳酸盐硬度115、water softening水软化116、permanent hardness永久硬度117、ion exchange离子交换118、fossil fuels化石燃料119、oxidation氧化120、reduction还原121、oxidation-reduction（redox）reactions氧化还原反应122、oxidizing agent氧化剂123、heavy water重水124、absorption吸附125、acidic anhydride(oxide)酸性酸酐126、basic anhydride(oxide)碱性酸酐127、amphoteric两性128、allotropes同素异形体129、acid salt酸式盐130、oxidizing anion氧化性阴离子131、disproportionation reaction歧化反应132、oxidizing acids氧化性酸。

专业英语词汇Unit 1 TEXT A：Chemical Reactions and Group Reactions customary a. 通常的，惯例的handle n.柄vt.触摸handling n.处理，管理derive vt.取得，得到，衍生oxidate vt.使氧化oxidation n.satisfactory a.令人满意的，符合要求的rapid a.快的，迅速的，动作快的combustion n.燃烧somewhat pron. ad. 一点点，几分，有点effort n.努力commercial a.商业的，商务的undesirable a.不合需要的，不受欢迎的，讨厌的retard vt.延迟，放慢，使停滞transformer n.变压器transform vt.改变，转变automotive a.自动的，机动的，汽车的cracked 裂化的sluge n.软泥，淤泥stiff a.硬的，强烈的extent 广度，程度distillation n.蒸馏distill vt.vi.unrefined a.未精致，未提炼的acidity n.酸味，酸性acidify vt. Vi.Involve vt.包缠，卷缠Fell=followingIndividual a.个人的，个体的Presumable a.可假定的，可推测的Destruction n.破坏，毁灭Overall n。

a.全面的，综合的Exceed 超过，胜过Isolate vt.隔离，孤立，使离析iso—构词成分“均匀”“异构”“苯”Analyse vt. 分析，分解Carbonyl 羰基Carboxyl 羧基Hydroxyl 羟基Decomposition 分解Alkyl 烷基，烃基Aldehyde n.醛Yield vt. 出产，产出Explosive a. 爆炸Vapor n.蒸汽，vi.蒸发Propagation 繁殖，增殖；传播Dehydrate vt.使脱水Acet 构词成分Acetaldehyde 乙醛Resin n.树脂Resinous a.树脂的Carboxylic a.羟基的Substantial a.物质的，实质的Susceptible a.易受感动的，敏感的Analogous a.类似的，相似的（to）Response n.作答，回答，响应，反应Readily ad.乐意地，很快地Readiness n.准备就绪，愿意Extent n.广度长度Steric 空间的，位的Likewise ad.同样的，照样地；也，又Suffer vt.遭受，经历Progressive a.进步的，长进的，渐次的Adjacent a.邻近的，紧挨着的Terminal a.末端的，终点的MethyleneBromide n.溴化物Substitute n.代替物（人），代用品substitution n.代替，替换Remote a.相隔较远的Acetone n.丙酮Ether n.醚，乙醚Correspond vi.符合，一致；相当，相应Reservation n.保留，预定Tend vi.走向，趋向。

Inorganic chemistry 无机化学Organic chemistry 有机化学Physical chemistry 物理化学Analytical chemistry 分析化学Polymer chemistry 高分子化学Biochemistry 生物化学Radiochemistry 放射化学Theoretical chemistry 理论化学Matter ['mætə] n 物质Mass [mæs] n 质量V olume ['vɔljuːm] n 体积Pure substance 纯净物Element ['elim(ə)nt] n 元素Compound ['kɔmpaund] n 化合物Mixture ['mikstʃə] n 混合物Homogeneous [,hɔmə(u)'dʒiːniəs; -'dʒen-] 均匀的Homogeneous mixture 均匀混合物Solution [sə'luːʃ(ə)n] n 溶液Heterogeneous mixture 非均匀混合物Solid ['sɔlɪd] n 固体Liquid ['likwid] n 液体Gas [gæs] n 气体Plasma ['plæzmə] n 等离子体Excited state 激发态Physical property 物理性质Physical change 物理变化Chemical property 化学性质Chemical change 化学变化Separation of mixture 混合物分离Molecule ['mɔlikjuːl] n分子Chemical element 化学元素Atomic number 原子序数Technetium [tek'niːʃɪəm] n 锝Promethium [prə'miːθɪəm] n 钷Bismuth ['bizməθ] n 铋Radioactive decay 放射性衰变Nucleosynthesis [,njuːkliəʊ'si nθisis] n 核合成Artificial [ɑːtifiʃ(ə)l] adj 人工的Synthetic [si n'θet ik] adj 合成的Molecular compound 分子化合物Ionic compound 离子化合物Ionic bond 离子键Cation 阳离子Anion 阴离子Polyatomic ion 多原子离子Chemical formula 化学式Empirical formula 实验式Molecular formula 分子式Elemental analysis 元素分析Physical quantity 物理量Accuracy 准确度Precision 精确度Reproducibility [riprə,dju:sə'biliti] 再现性Repeatability [ri'pi:tə'biliti] 重复性Valid ['vælid] n 有效Bias ['baiəs] n 偏差Error ['erə] n 错误Random error 随机误差Systematic error 系统误差Significant figure有效数字Addition [ə'diʃ(ə)n] n 加法Subtraction [səb'trækʃn] n减法Multiplication [,mʌltipli'keiʃ(ə)n] n 乘法Division [di'viʒ(ə)n] n 除法Scientific notation/ Standard form / Exponential notation 科学计数法Coefficient [,kəui'fiʃ(ə)nt] n 系数Significant [sig'nifɪk(ə)nt] P10Mantissa [mæn'tisə] P10Minus sign 减号United States Customary System 美国习惯体系British Imperial Units P10Metric ['metrik] adj 公制的Decimalized system 十进制系统SI system 国际单位制Derived quantities 导出量Length [leŋθ] n 长度Density ['densiti] n 密度Temperature ['temp(ə)rətʃə] n 温度Potential energy 势能Kinetic energy 动能Heat [hiːt] n 热量Specific heat 比热Force [fɔːs] n 压力Pressure ['preʃə] n 压强Factor-lable/united-factor method量纲分析Dimensional analysis 量纲分析Conversion factor 转换因子Numerator ['njuːməreitə] n 分子Denominator [di'nɔmineitə] n 分母。

(完整版)化学专业英语一、基础词汇篇1. 原子与分子Atom（原子）：物质的基本单位，由质子、中子和电子组成。

2. 化学反应Reactant（反应物）：参与化学反应的物质。

Product（物）：化学反应后的物质。

Catalyst（催化剂）：能改变化学反应速率而本身不发生永久变化的物质。

3. 物质状态Solid（固体）：具有一定形状和体积的物质。

Liquid（液体）：具有一定体积，无固定形状的物质。

Gas（气体）：无固定形状和体积的物质。

4. 酸碱盐Acid（酸）：在水溶液中能电离出氢离子的物质。

Base（碱）：在水溶液中能电离出氢氧根离子的物质。

Salt（盐）：由酸的阴离子和碱的阳离子组成的化合物。

5. 溶液与浓度Solution（溶液）：由溶剂和溶质组成的均匀混合物。

Solvent（溶剂）：能溶解其他物质的物质。

Solute（溶质）：被溶解的物质。

Concentration（浓度）：溶液中溶质含量的度量。

二、专业术语篇1. 有机化学Organic Chemistry（有机化学）：研究碳化合物及其衍生物的化学分支。

Functional Group（官能团）：决定有机化合物化学性质的原子或原子团。

Polymer（聚合物）：由许多重复单元组成的大分子化合物。

2. 无机化学Inorganic Chemistry（无机化学）：研究不含碳的化合物及其性质的化学分支。

Crystal（晶体）：具有规则排列的原子、离子或分子的固体。

OxidationReduction Reaction（氧化还原反应）：涉及电子转移的化学反应。

3. 物理化学Physical Chemistry（物理化学）：研究化学现象与物理现象之间关系的化学分支。

Chemical Bond（化学键）：原子间相互作用力，使原子结合成分子。

Thermodynamics（热力学）：研究能量转换和物质性质的科学。

4. 分析化学Analytical Chemistry（分析化学）：研究物质的组成、结构和性质的科学。