📚 AP Chemistry High-Frequency Vocabulary (Part 2) | AP 化学高频词汇汇编（下）
This second part of our AP Chemistry vocabulary collection covers essential terms from equilibrium, acids and bases, thermodynamics, electrochemistry, and more. Mastering these words will help you interpret exam questions accurately and express your reasoning with scientific precision.
本篇 AP 化学词汇汇编（下）涵盖了化学平衡、酸碱、热力学、电化学等核心单元的高频术语。掌握这些词汇不仅能让你准确理解题目要求，还能帮助你在自由回答题中用专业的科学语言进行表述。
1. Chemical Kinetics | 化学动力学
The field of chemical kinetics examines the speed at which reactions proceed and the pathway from reactants to products. Key vocabulary describes rate laws, activation energy, and the role of catalysts.
化学动力学研究反应进行的速率以及从反应物到产物的路径。核心词汇包括速率方程、活化能以及催化剂的作用。
Rate law: An equation that expresses the reaction rate as a function of reactant concentrations, normally in the form rate = k[A]ᵐ[B]ⁿ, where k is the rate constant and m, n are reaction orders.
速率方程：表示反应速率与反应物浓度关系的方程，通常形式为 速率 = k[A]ᵐ[B]ⁿ，其中 k 为速率常数，m、n 为反应级数。
Activation energy (Eₐ): The minimum energy required to form the transition state; it determines the temperature dependence of the rate constant through the Arrhenius equation.
活化能 (Eₐ)：形成过渡态所需的最低能量；通过阿伦尼乌斯方程决定速率常数对温度的依赖关系。
Catalyst: A substance that increases the reaction rate by providing an alternative pathway with a lower activation energy, without being consumed itself.
催化剂：一种通过提供具有较低活化能的替代路径来加快反应速率而自身不被消耗的物质。
Half-life (t₁/₂): The time required for the concentration of a reactant to decrease to half its initial value; for a first-order reaction it is independent of initial concentration.
半衰期 (t₁/₂)：反应物浓度降至初始值一半所需的时间；对于一级反应，半衰期与初始浓度无关。
Reaction coordinate: A diagrammatic representation showing the energy change along the progress of a reaction, with peaks corresponding to transition states and valleys to intermediates or products.
反应坐标图：显示反应进程中能量变化的图示，峰对应过渡态，谷对应中间体或产物。
2. Chemical Equilibrium | 化学平衡
At equilibrium the forward and reverse reaction rates are equal, and the concentrations of reactants and products remain constant. The equilibrium constant, K, quantifies the position of equilibrium.
达到平衡时，正逆反应速率相等，反应物和产物的浓度保持恒定。平衡常数 K 用于定量描述平衡的位置。
Equilibrium constant (K): A dimensionless value derived from the ratio of product concentrations to reactant concentrations, each raised to the power of its stoichiometric coefficient at equilibrium. K > 1 indicates products are favored.
平衡常数 (K)：由平衡时产物浓度与反应物浓度的比值得到的无量纲值，各项均以其化学计量数为指数。K > 1 表示反应倾向生成产物。
Le Chatelier’s principle: When a system at equilibrium is subjected to a change in concentration, pressure, or temperature, the system will shift to partially counteract the imposed change.
勒夏特列原理：当处于平衡状态的体系受到浓度、压强或温度的变化时，平衡会向减弱该改变的方向移动。
Reaction quotient (Q): Calculated using the same formula as K but with concentrations at any point in time; comparing Q to K predicts the direction the reaction must shift to reach equilibrium.
反应商 (Q)：使用与 K 相同的公式计算，但可以采用任意时刻的浓度；比较 Q 与 K 可预测反应达到平衡所需移动的方向。
ICE table: A tabular method that tracks Initial concentrations, Change in concentration, and Equilibrium concentrations to solve equilibrium problems systematically.
ICE 表：一种系统求解平衡问题的表格方法，追踪初始浓度 (Initial)、浓度变化 (Change) 和平衡浓度 (Equilibrium)。
3. Acids and Bases | 酸和碱
The Brønsted-Lowry theory defines acids as proton donors and bases as proton acceptors. Understanding acid-base strength, pH, and pKₐ is central to predicting reactivity in aqueous solutions.
布朗斯特-劳里酸碱理论将酸定义为质子给予体，碱定义为质子接受体。理解酸碱强度、pH 以及 pKₐ 对于预测水溶液中的反应性至关重要。
Conjugate acid-base pair: Two species that differ by a single proton; the conjugate base of an acid is formed when the acid donates a proton.
共轭酸碱对：相差一个质子的两种物质；酸失去一个质子后即形成其共轭碱。
pH and pOH: pH = -log[H⁺] and pOH = -log[OH⁻]; in water at 25 °C, pH + pOH = 14.00.
pH 与 pOH：pH = -log[H⁺]，pOH = -log[OH⁻]；25 °C 的水中，pH + pOH = 14.00。
Acid dissociation constant (Kₐ): The equilibrium constant for the ionization of an acid in water; a larger Kₐ indicates a stronger acid. pKₐ = -log Kₐ.
酸解离常数 (Kₐ)：酸在水溶液中电离的平衡常数；Kₐ 越大表明酸性越强。pKₐ = -log Kₐ。
Autoionization of water (Kₓ): 2H₂O ⇌ H₃O⁺ + OH⁻; Kₓ = [H₃O⁺][OH⁻] = 1.0 × 10⁻¹⁴ at 25 °C.
水的自电离 (Kₓ)：2H₂O ⇌ H₃O⁺ + OH⁻；25 °C 时 Kₓ = [H₃O⁺][OH⁻] = 1.0 × 10⁻¹⁴。
Polyprotic acid: An acid that can donate more than one proton, such as H₂SO₄ or H₃PO₄; each proton loss has its own Kₐ value.
多元酸：能提供多个质子的酸，如 H₂SO₄ 或 H₃PO₄；每一步失质子都有相应的 Kₐ 值。
4. Buffers and Titrations | 缓冲溶液与滴定
Buffers resist significant changes in pH upon addition of small amounts of acid or base. Titration curves display characteristic shapes that reveal the equivalence point and buffer region.
缓冲溶液能在加入少量酸或碱时抵抗 pH 的显著变化。滴定曲线展示出特征性的形状，可用于判断等当点和缓冲区域。
Buffer solution: A mixture of a weak acid and its conjugate base (or a weak base and its conjugate acid) that maintains an almost constant pH.
缓冲溶液：由弱酸及其共轭碱（或弱碱及其共轭酸）组成的混合物，能维持近乎恒定的 pH。
Henderson-Hasselbalch equation: pH = pKₐ + log([A⁻]/[HA]), used to calculate the pH of a buffer or during a titration before the equivalence point.
亨德森-哈塞尔巴赫方程：pH = pKₐ + log([A⁻]/[HA])，用于计算缓冲溶液的 pH 或等当点前的滴定 pH。
Equivalence point: The point in a titration where the number of moles of added titrant exactly equals the number of moles of the substance being titrated.
等当点：滴定中加入的滴定剂摩尔数恰好与被滴定物质的摩尔数相等的一点。
Half-equivalence point: The midpoint of the buffer region where [HA] = [A⁻] and pH = pKₐ; especially useful for determining Kₐ experimentally.
半等当点：缓冲区域的中心点，此时 [HA] = [A⁻] 且 pH = pKₐ；常用于实验测定 Kₐ。
5. Thermodynamics | 热力学
Thermodynamics links energy changes with spontaneity. Essential terms include enthalpy, entropy, Gibbs free energy, and the three laws that govern energy transfer.
热力学将能量变化与自发性联系起来。核心词汇包括焓、熵、吉布斯自由能以及支配能量传递的三大定律。
Enthalpy (H): The heat content of a system at constant pressure; ΔH = H_products – H_reactants. Exothermic reactions have ΔH < 0; endothermic reactions have ΔH > 0.
焓 (H)：恒压条件下体系的热含量；ΔH = H_产物 – H_反应物。放热反应 ΔH < 0，吸热反应 ΔH > 0。
Entropy (S): A measure of the disorder or randomness of a system; the second law states that the total entropy of the universe increases in spontaneous processes.
熵 (S)：体系混乱度或随机度的量度；热力学第二定律指出，自发过程中宇宙的总熵增加。
Gibbs free energy (G): ΔG = ΔH – TΔS; a process is spontaneous at constant temperature and pressure when ΔG < 0.
吉布斯自由能 (G)：ΔG = ΔH – TΔS；恒温恒压下当 ΔG < 0 时过程自发进行。
Standard state conditions: Definitions of reference states used for tabulating thermodynamic data; for gases 1 bar, for solutes 1 M, for elements their most stable form at 25 °C.
标准状态：用于列表热力学数据的参考状态规定；气体为 1 bar，溶质为 1 M，元素为 25 °C 下最稳定形态。
6. Electrochemistry | 电化学
Electrochemistry deals with the interconversion of chemical and electrical energy. Redox reactions, standard reduction potentials, and the Nernst equation are essential for understanding cells and batteries.
电化学研究化学能与电能之间的相互转换。氧化还原反应、标准还原电势以及能斯特方程是理解原电池和电解池的核心。
Redox reaction: A reaction in which oxidation (loss of electrons) and reduction (gain of electrons) occur simultaneously.
氧化还原反应：氧化（失去电子）和还原（得到电子）同时发生的反应。
Standard reduction potential (E°): The voltage associated with a half-reaction under standard conditions, measured relative to the standard hydrogen electrode (0 V). A higher E° indicates greater oxidizing strength.
标准还原电势 (E°)：标准条件下与半反应相关的电压，相对于标准氢电极 (0 V) 测量。E° 越高表明氧化能力越强。
Cell potential (E_cell): E_cell = E°_cathode – E°_anode under standard conditions; for a spontaneous cell, E_cell > 0.
电池电动势 (E_cell)：标准条件下 E_cell = E°_阴极 – E°_阳极；自发电池的 E_cell > 0。
Nernst equation: E = E° – (RT/nF)ln Q, used to calculate cell potential under non-standard concentrations.
能斯特方程：E = E° – (RT/nF)ln Q，用于计算非标准浓度下的电池电动势。
7. Nuclear Chemistry | 核化学
Nuclear chemistry explores changes in an atom’s nucleus, including radioactive decay, fission, and fusion. Vocabulary focuses on stability, half-life, and types of radiation.
核化学探索原子核的变化，包括放射性衰变、裂变和聚变。相关词汇集中在稳定性、半衰期及辐射类型上。
Radioactive decay: The spontaneous disintegration of an unstable nucleus emitting particles or electromagnetic radiation, such as alpha (⁴₂He), beta (⁰₋₁e), or gamma (γ) rays.
放射性衰变：不稳定原子核自发崩解并放出粒子或电磁辐射的过程，如 α 衰变 (⁴₂He)、β 衰变 (⁰₋₁e) 或 γ 射线。
Half-life (nuclear): The time it takes for half of a radioactive sample to decay; it remains constant and is independent of the initial amount.
半衰期（核）：放射性样品衰变一半所需的时间；半衰期恒定，不受初始量影响。
Mass defect: The difference between the mass of an atomic nucleus and the sum of the masses of its individual protons and neutrons; this “lost” mass is converted to binding energy via E = mc².
质量亏损：原子核的质量与其所有独立质子和中子的质量总和之差；这部分“损失”的质量通过 E = mc² 转化为结合能。
Nuclear binding energy: The energy required to separate a nucleus into its constituent protons and neutrons; a measure of nuclear stability.
核结合能：将原子核分解为组成它的质子和中子所需的能量；是衡量核稳定性的指标。
8. Organic and Biochemistry Concepts | 有机与生化基本概念
Organic chemistry in AP focuses on functional groups, isomerism, and naming conventions. Basic biochemistry terms link molecular structure to biological function.
AP 有机化学部分侧重于官能团、同分异构现象和命名规则。基础生物化学词汇将分子结构与生物功能联系起来。
Functional group: A specific arrangement of atoms that imparts characteristic chemical reactivity; examples include hydroxyl (-OH), carboxyl (-COOH), and amino (-NH₂).
官能团：赋予分子特征化学性质的特定原子组合；例如羟基 (-OH)、羧基 (-COOH) 和氨基 (-NH₂)。
Isomer: Compounds sharing the same molecular formula but differing in structure or spatial arrangement. Structural isomers differ in connectivity; stereoisomers differ only in 3D orientation.
同分异构体：分子式相同但结构或空间排列不同的化合物。构造异构体连接方式不同；立体异构体仅在三维取向上不同。
Polymer: A large molecule composed of repeating subunits called monomers; e.g., polyethylene from ethylene, or proteins from amino acids.
聚合物：由称为单体的重复单元组成的大分子；例如由乙烯聚合而成的聚乙烯，或由氨基酸构成的蛋白质。
Enzyme: A biological catalyst, typically a protein, that accelerates biochemical reactions by lowering activation energy; highly specific to its substrate.
酶：一种生物催化剂，通常为蛋白质，通过降低活化能加快生化反应速率，对其底物具有高度专一性。
9. Intermolecular Forces and Properties | 分子间作用力与性质
Intermolecular forces determine physical properties such as boiling point, vapor pressure, and solubility. Understanding these non-covalent interactions is key to predicting behavior in condensed phases.
分子间作用力决定了沸点、蒸气压和溶解度等物理性质。理解这些非共价相互作用是预测凝聚相行为的关键。
London dispersion forces: Weak attractive forces arising from temporary dipoles induced in molecules; present in all substances but dominant in nonpolar molecules.
伦敦色散力：由分子中瞬时偶极产生的弱吸引力；所有物质中都存在，但在非极性分子中起主导作用。
Dipole-dipole forces: Attractive forces between the positive end of one polar molecule and the negative end of another; stronger than dispersion forces.
偶极-偶极作用力：一个极性分子的正端与另一个极性分子的负端之间的引力；比色散力强。
Hydrogen bonding: A very strong dipole-dipole interaction occurring when hydrogen is bonded to N, O, or F; it explains the unusually high boiling point of water.
氢键：一种极强的偶极-偶极相互作用，存在于氢与氮、氧或氟成键时；它解释了水异常高的沸点。
Like dissolves like: A general rule stating that solutes dissolve best in solvents with similar polarity; polar solutes dissolve in polar solvents, nonpolar in nonpolar.
相似相溶：一个经验规则，指出溶质在极性相似的溶剂中溶解最佳；极性溶质溶于极性溶剂，非极性溶于非极性。
10. Laboratory and Data Analysis | 实验与数据分析
Familiarity with laboratory equipment, safety practices, and data interpretation is essential. Terms related to precision, accuracy, and significant figures appear frequently in AP exam questions.
熟悉实验设备、安全操作以及数据解读是必要的。与精密度、准确度和有效数字相关的术语在 AP 考试中频繁出现。
Accuracy vs. Precision: Accuracy refers to how close a measurement is to the true value; precision refers to the closeness of repeated measurements to each other.
准确度与精密度：准确度指测量值与真值的接近程度；精密度指重复测量结果彼此之间的接近程度。
Percent error: |experimental value – accepted value| / accepted value × 100%; used to assess the accuracy of an experimental result.
百分误差：|实验值 – 公认值| / 公认值 × 100%；用于评估实验结果的准确度。
Significant figures: Digits in a measurement that carry meaningful information about the precision of the instrument; rules for addition/subtraction differ from multiplication/division.
有效数字：测量中包含有关仪器精密度有意义信息的数字；加减运算与乘除运算的规则不同。
Spectrophotometry: A technique measuring the absorbance of light by a sample; used to determine concentration via Beer’s law, A = εbc.
分光光度法：测量样品吸收光的程度的技术；利用比尔定律 A = εbc 测定浓度。
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