📚 AP Chemistry High-Frequency Vocabulary Compilation from Past Exams | AP化学历年真题高频词汇汇编
AP Chemistry demands not only a solid conceptual understanding but also a strong command of subject-specific terminology. Over the years, College Board exams have repeatedly tested key terms that describe fundamental principles, quantitative relationships, and experimental set-ups. This article compiles the high-frequency vocabulary from real past papers, grouped by topic, so that you can sharpen your lexical precision and avoid common misinterpretations on test day. Each term is presented with a concise definition in English followed by its Chinese equivalent, mirroring the dual-language approach needed for thorough comprehension.
AP化学不仅要求扎实的概念理解，还要求对学科专业术语的熟练掌握。多年来，大学理事会的真题反复考查描述基本原理、定量关系和实验设置的核心词汇。本文按主题分类整理了历年真题中的高频词汇，每个术语都给出了简明的英文定义及对应的中文解释，采用双语对照的方式帮助你提升用词准确性，避免考试中常见的理解偏差。
1. Fundamentals and Measurements | 基础与测量
Precision – The degree to which repeated measurements under unchanged conditions show the same results; it reflects the consistency of a set of data.
精密度 (Precision) – 指在不变条件下重复测量所得结果的一致性程度，衡量一组数据的分散程度，但与真实值无关。
Accuracy – How close a measured value is to the true or accepted value; it indicates the correctness of a measurement.
准确度 (Accuracy) – 测量值与真实值或可接受值之间的接近程度，反映测量的正确性。
Significant Figures – All the digits in a measurement that are known with certainty plus the first uncertain digit; they convey the precision of the measuring instrument.
有效数字 (Significant Figures) – 测量记录中确定已知的数字加上第一位不确定数字，用来表示测量仪器的精密度。
Dimensional Analysis – A problem-solving method that uses conversion factors to move from one unit to another, ensuring the correct cancellation of units.
量纲分析 (Dimensional Analysis) – 利用换算因子进行单位转换的解题方法，通过单位对消来验证计算轨迹的正确性。
Intensive Property – A physical property that does not depend on the amount of matter present, such as density, boiling point, or color.
强度性质 (Intensive Property) – 不随物质多少变化的物理性质，如密度、沸点、颜色，常用于辨识物质。
Extensive Property – A property that depends on the amount of matter in a sample, e.g., mass, volume, and total charge.
广延性质 (Extensive Property) – 与试样中物质数量相关的性质，如质量、体积、总电荷。
2. Stoichiometry and the Mole Concept | 化学计量与摩尔概念
Mole (mol) – The SI unit for amount of substance, containing exactly 6.02214076 × 10²³ elementary entities (Avogadro’s number).
摩尔 (mol) – 物质的量的国际单位，精确包含6.02214076 × 10²³个基本单元（阿伏伽德罗常数）。
Molar Mass – The mass of one mole of a substance, expressed in grams per mole (g·mol⁻¹), numerically equal to the average atomic or formula mass in u.
摩尔质量 (Molar Mass) – 一摩尔物质的质量，单位为g·mol⁻¹，数值上等于以u为单位的平均原子质量或式量。
Empirical Formula – The simplest whole-number ratio of atoms of each element present in a compound.
实验式 (Empirical Formula) – 化合物中各元素原子的最简整数比。
Molecular Formula – The actual number of atoms of each element in a molecule; it may be a multiple of the empirical formula.
分子式 (Molecular Formula) – 一个分子中每种元素的实际原子数目，可以是实验式的整数倍。
Limiting Reactant – The reactant that is completely consumed in a chemical reaction, thereby determining the maximum amount of product that can be formed.
限制反应物 (Limiting Reactant) – 在化学反应中完全消耗的反应物，它决定了所能生成的最大产物的量。
Percent Yield – The ratio of the actual yield (experimentally obtained) to the theoretical yield, multiplied by 100%.
产率 (Percent Yield) – 实际产量与理论产量的比值，乘以100%，用于评价反应效率。
3. Atomic Structure and Periodicity | 原子结构与周期性
Atomic Number (Z) – The number of protons in the nucleus of an atom, which uniquely identifies the element.
原子序数 (Atomic Number, Z) – 原子核内质子的数目，决定元素的化学身份。
Isotopes – Atoms of the same element with the same number of protons but different numbers of neutrons, thus differing in mass number.
同位素 (Isotopes) – 质子数相同而中子数不同的同种元素的原子，质量数不同。
Electron Configuration – The distribution of electrons among the orbitals of an atom, often written in spdf notation following the Aufbau principle.
电子排布 (Electron Configuration) – 原子中电子在各轨道的分布，通常按构造原理用spdf符号书写。
Ionization Energy – The minimum energy required to remove the most loosely held electron from a gaseous atom or ion; it generally increases across a period and decreases down a group.
电离能 (Ionization Energy) – 从气态原子或离子中移去一个束缚最松的电子所需的最低能量；同周期递增大致增加，同族递增大致减小。
Electronegativity – A measure of the tendency of an atom to attract a bonding pair of electrons; fluorine is the most electronegative element.
电负性 (Electronegativity) – 衡量原子吸引共用电子对能力的尺度；氟是电负性最强的元素。
Shielding Effect – The reduction of the effective nuclear charge on an electron cloud due to inner-shell electrons repelling outer electrons.
屏蔽效应 (Shielding Effect) – 内层电子对原子核吸引外层电子的削弱作用，导致有效核电荷降低。
4. Chemical Bonding and Molecular Geometry | 化学键与分子构型
Ionic Bond – The electrostatic attraction between oppositely charged ions formed when electrons are transferred from a metal to a nonmetal.
离子键 (Ionic Bond) – 通过电子转移形成的阳离子和阴离子间的静电吸引力，通常存在于金属与非金属之间。
Covalent Bond – A chemical bond that involves the sharing of electron pairs between atoms, typical of nonmetal–nonmetal combinations.
共价键 (Covalent Bond) – 原子间通过共享电子对形成的化学键，常见于非金属原子之间。
Lewis Structure – A diagram that shows the bonding between atoms of a molecule and the lone pairs of electrons that may exist in the molecule.
路易斯结构 (Lewis Structure) – 表示分子内部原子间键合情况以及孤对电子分布的示意图。
VSEPR Theory – Valence Shell Electron Pair Repulsion theory; it predicts the three-dimensional shape of a molecule based on the repulsion between electron pairs around a central atom.
VSEPR理论 (VSEPR Theory) – 价层电子对互斥理论，根据中心原子周围电子对的排斥作用预测分子的三维空间构型。
Hybridization – The mixing of atomic orbitals to form new hybrid orbitals suitable for the pairing of electrons to form chemical bonds (e.g., sp, sp², sp³).
杂化 (Hybridization) – 原子轨道重新组合形成新轨道的过程，新轨道可以用于成键，如sp、sp²、sp³杂化。
Polarity – The separation of electric charge leading to a molecule having a dipole moment, caused by differences in electronegativity between bonded atoms.
极性 (Polarity) – 由于电负性差异引起的电荷分离，使分子产生偶极矩，分为极性分子与非极性分子。
5. Intermolecular Forces and States of Matter | 分子间作用力与物态
London Dispersion Forces – Weak intermolecular forces arising from temporary fluctuations in electron distribution, present in all molecules; they increase with molecular size.
伦敦色散力 (London Dispersion Forces) – 由瞬间电子分布不均产生的微弱分子间作用力，所有分子都有，随分子体积增大而增强。
Dipole-Dipole Forces – Attractive forces between the positive end of one polar molecule and the negative end of another polar molecule.
偶极-偶极力 (Dipole-Dipole Forces) – 极性分子正、负电端之间的静电吸引作用。
Hydrogen Bond – A particularly strong type of dipole-dipole interaction that occurs when hydrogen is bonded to highly electronegative N, O, or F.
氢键 (Hydrogen Bond) – 氢原子与电负性很大的N、O或F键合时产生的一种特强偶极-偶极相互作用，对水的异常性质起关键作用。
Vapor Pressure – The pressure exerted by a vapor in thermodynamic equilibrium with its condensed phases at a given temperature.
蒸气压 (Vapor Pressure) – 在给定温度下液体与其蒸气达到平衡时蒸气所显示的压力，反映液体分子逃逸趋势。
Sublimation – The direct transition from the solid phase to the gas phase without passing through the liquid state.
升华 (Sublimation) – 物质从固态直接转变为气态而未经液态的过程，如干冰的蒸发。
6. Gases and Kinetic Molecular Theory | 气体与分子动理论
Ideal Gas Law – The equation of state for an ideal gas: PV = nRT, relating pressure, volume, amount, and temperature.
理想气体状态方程 (Ideal Gas Law) – 描述理想气体行为的方程：PV = nRT，关联压强、体积、物质的量和温度。
Partial Pressure – The pressure that a gas in a mixture would exert if it alone occupied the entire volume; according to Dalton’s Law, total pressure equals the sum of partial pressures.
分压 (Partial Pressure) – 混合气体中某一组分单独占据整个体积时所具有的压强；道尔顿分压定律指出总压等于分压之和。
Graham’s Law of Effusion – The rate of effusion of a gas is inversely proportional to the square root of its molar mass: r₁/r₂ = √(M₂/M₁).
格锐目扩散定律 (Graham’s Law of Effusion) – 气体的隙流速率与其摩尔质量的平方根成反比：r₁/r₂ = √(M₂/M₁)。
Real Gas – A gas that does not obey the ideal gas law perfectly because of finite molecular volume and intermolecular forces; the van der Waals equation corrects for these effects.
真实气体 (Real Gas) – 由于分子本身体积和分子间作用力的存在而不严格符合理想气体定律的气体，常用范德华方程修正。
7. Thermochemistry and Thermodynamics | 热化学与热力学
Enthalpy (H) – The heat content of a system at constant pressure; change in enthalpy (ΔH) equals the heat absorbed or released under constant pressure.
焓 (Enthalpy, H) – 体系在恒定压力下的热含量，焓变 (ΔH) 等于恒压条件下吸收或释放的热量。
Exothermic Reaction – A reaction that releases heat, giving ΔH < 0; products are lower in energy than reactants.
放热反应 (Exothermic Reaction) – 释放热量的反应，ΔH < 0，生成物能量低于反应物。
Endothermic Reaction – A reaction that absorbs heat, ΔH > 0; energy is taken in from the surroundings.
吸热反应 (Endothermic Reaction) – 吸收热量的反应，ΔH > 0，体系从环境吸收能量。
Hess’s Law – The total enthalpy change for a reaction is the same regardless of the route taken, as long as initial and final conditions are identical.
盖斯定律 (Hess’s Law) – 反应的总焓变只取决于始终状态，与途径无关，允许通过已知反应焓的代数和求算目标焓变。
Entropy (S) – A measure of the disorder or randomness of a system; the second law of thermodynamics states that the total entropy of the universe always increases for a spontaneous process.
熵 (Entropy, S) – 体系混乱度的量度；热力学第二定律指出在自发过程中宇宙的总熵总是增加。
Gibbs Free Energy (G) – A thermodynamic potential defined as G = H − TS; a process at constant T and P is spontaneous if ΔG < 0.
吉布斯自由能 (Gibbs Free Energy, G) – 定义为 G = H − TS 的热力学函数；在恒温恒压下 ΔG < 0 时过程自发进行。
8. Kinetics | 化学动力学
Reaction Rate – The change in concentration of a reactant or product per unit time, often expressed in mol·L⁻¹·s⁻¹.
反应速率 (Reaction Rate) – 单位时间内反应物或产物浓度的变化量，常用单位为 mol·L⁻¹·s⁻¹。
Rate Law – An equation that relates the reaction rate to the concentrations of reactants raised to some powers: rate = k[A]ᵐ[B]ⁿ, where m and n are reaction orders.
速率方程 (Rate Law) – 将反应速率与各反应物浓度次幂关联起来的方程：rate = k[A]ᵐ[B]ⁿ，m和n为反应级数。
Activation Energy (Eₐ) – The minimum energy that colliding particles must have for a reaction to occur; it determines the temperature dependence of the rate constant via the Arrhenius equation.
活化能 (Activation Energy, Eₐ) – 反应物分子发生有效碰撞所需的最低能量，通过阿伦尼乌斯方程决定速率常数的温度依赖性。
Catalyst – A substance that speeds up a reaction by providing an alternative pathway with a lower activation energy, without being consumed itself.
催化剂 (Catalyst) – 通过提供较低活化能的替代途径加快反应速率，反应前后自身的组成和质量不变。
Rate-Determining Step – The slowest elementary step in a reaction mechanism; it dictates the overall rate law.
速率决定步骤 (Rate-Determining Step) – 反应机理中最慢的基元步骤，决定了总反应的速率方程。
9. Chemical Equilibrium | 化学平衡
Dynamic Equilibrium – The state in a reversible reaction where the forward and reverse reaction rates are equal, so the macroscopic concentrations remain constant.
动态平衡 (Dynamic Equilibrium) – 可逆反应达到正逆反应速率相等的状态，宏观浓度不再改变但微观反应仍在进行。
Equilibrium Constant (K) – The ratio of product concentrations to reactant concentrations, each raised to the power of its stoichiometric coefficient, at equilibrium. Kc uses molarity; Kp uses partial pressures.
平衡常数 (Equilibrium Constant, K) – 平衡时生成物浓度幂乘积与反应物浓度幂乘积之比；Kc用浓度表示，Kp用分压表示。
Le Chatelier’s Principle – If a dynamic equilibrium is disturbed by changing the conditions, the position of equilibrium shifts to partially counteract the change.
勒夏特列原理 (Le Chatelier’s Principle) – 改变平衡体系的条件（浓度、压力、温度）时，平衡会向着减弱这种改变的方向移动。
Reaction Quotient (Q) – The ratio of concentrations (or pressures) at any point in the reaction; comparing Q to K indicates the direction in which the reaction will proceed to reach equilibrium.
反应商 (Reaction Quotient, Q) – 反应进行到任一时刻的浓度比（或压力比），与K比较即可判断反应进行方向；Q Solubility Product (Ksp) – The equilibrium constant for the dissolution of a sparingly soluble ionic compound; it represents the maximum product of ion concentrations in a saturated solution. 溶度积 (Solubility Product, Ksp) – 难溶电解质溶解平衡的平衡常数，等于饱和溶液中各离子浓度幂的乘积，用于预测沉淀生成。 Brønsted-Lowry Acid/Base – An acid is a proton (H⁺) donor; a base is a proton acceptor. This definition is central to AP acid-base equilibria. 布朗斯特-劳里酸碱 (Brønsted-Lowry Acid/Base) – 酸是质子（H⁺）给予体，碱是质子接受体，是AP化学中最常用的酸碱定义。 pH and pOH – pH = −log[H₃O⁺]; pOH = −log[OH⁻]; at 25 °C, pH + pOH = 14. These logarithmic scales describe the acidity/basicity of aqueous solutions. pH和pOH – pH = −log[H₃O⁺]，pOH = −log[OH⁻]；25 °C时pH + pOH = 14，用于描述水溶液的酸碱度。 Acid Dissociation Constant (Kₐ) – The equilibrium constant for a weak acid dissociation; larger Kₐ indicates a stronger weak acid. 酸解离常数 (Kₐ) – 弱酸电离平衡的平衡常数；Kₐ越大，弱酸相对越强。 Buffer Solution – A solution that resists changes in pH upon the addition of small amounts of acid or base, typically containing a weak acid and its conjugate base in comparable concentrations. 缓冲溶液 (Buffer Solution) – 能抵抗少量外加酸碱引起的pH变化的溶液，通常由浓度相近的弱酸及其共轭碱组成。 Equivalence Point – The point in a titration at which the number of moles of added titrant is stoichiometrically equal to the number of moles of analyte. 等当点 (Equivalence Point) – 滴定中滴加的标准溶液与被测物质按化学计量恰好完全反应的点，与终点不同。 Henderson-Hasselbalch Equation – pH = pKₐ + log([A⁻]/[HA]), used to estimate the pH of a buffer solution. 亨德森-哈塞尔巴尔赫方程 (Henderson-Hasselbalch Equation) – pH = pKₐ + log([A⁻]/[HA])，用于计算缓冲溶液的pH或配制目标缓冲液。 Oxidation and Reduction – Oxidation is the loss of electrons (increase in oxidation number); reduction is the gain of electrons (decrease in oxidation number). They always occur together. 氧化与还原 (Oxidation and Reduction) – 氧化指失去电子（氧化数升高），还原指得到电子（氧化数降低）；二者总是同时发生。 Half-Reaction – Either the oxidation or the reduction part of a redox reaction, written explicitly showing the electron transfer. 半反应 (Half-Reaction) – 将氧化还原反应拆分为氧化半反应和还原半反应，明确显示电子转移过程。 Galvanic (Voltaic) Cell – An electrochemical cell that converts chemical energy into electrical energy via a spontaneous redox reaction; the anode is negative, the cathode positive. 原电池 (Galvanic/Voltaic Cell) – 利用自发氧化还原反应将化学能转化为电能的装置；阳极为负，阴极为正。 Standard Reduction Potential (E°) – The voltage associated with a reduction half-reaction under standard conditions (1 M, 1 atm, 25 °C), measured relative to the standard hydrogen electrode (0 V). 标准还原电势 (Standard Reduction Potential, E°) – 标准态下（1 M, 1 atm, 25 °C）还原半反应的电极电势，相对于标准氢电极（0 V）测量；E°越正，氧化型越易被还原。 Nernst Equation – E = E° − (RT/nF) ln Q, which relates cell potential to nonstandard concentrations; at 25 °C it simplifies to E = E° − (0.0592/n) log Q. 能斯特方程 (Nernst Equation) – E = E° − (RT/nF) ln Q，计算非标准态下的电池电势；25 °C时常简化为 E = E° − (0.0592/n) log Q。 Spectrophotometry – An analytical technique that measures the absorbance of light by a sample; used to determine concentration via the Beer-Lambert Law (A = εbc). 分光光度法 (Spectrophotometry) – 通过测量样品对光的吸光度进行定量分析的方法，常用比尔-朗伯定律A=εbc计算浓度。 Titration – A technique in which a solution of known concentration (titrant) is used to determine the concentration of an unknown solution (analyte) through a controlled reaction. 滴定 (Titration) – 利用已知浓度标准溶液（滴定剂）与待测溶液按化学计量反应，通过指示剂或仪器确定终点并计算待测液浓度的分析方法。 Calibration Curve – A plot of instrument response vs. concentration of a series of standards, used to interpolate the concentration of an unknown sample. 校准曲线 (Calibration Curve) – 以标准溶液浓度对仪器响应值作图得到的曲线，用于内插未知样品的浓度。 Percent Error – (|experimental value − accepted value|/accepted value) × 100%, used to assess the accuracy of experimental data. 百分误差 (Percent Error) – (|实验值−真值|/真值)×100%，用于评估实验数据的准确度。 Filtration and Decantation – Simple separation techniques; filtration separates solid from liquid through a porous barrier, while decantation pours off a supernatant liquid. 过滤与倾析 (Filtration and Decantation) – 过滤利用多孔材料分离固/液混合物；倾析则通过倾倒上清液实现分离。 Published by TutorHao | AP Chemistry Revision Series | aleveler.com 更多咨询请联系16621398022（同微信）
10. Acid-Base Chemistry and Buffers | 酸碱化学与缓冲溶液
11. Electrochemistry | 电化学
12. Laboratory Techniques and Data Analysis | 实验技能与数据分析
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