📚 IB Chemistry: Final Exam Review Guide | IB 化学：期末复习提纲
Mastering IB Chemistry requires a strategic review of core concepts, command terms, and data-analysis skills. This guide provides a structured summary of the essential topics you must know for the final exam, from stoichiometry to organic chemistry, along with crucial exam techniques. Use it as a checklist to identify areas for further study and to solidify your understanding of the interconnected principles that form the heart of the IB Diploma Programme Chemistry course.
掌握 IB 化学需要对核心概念、命令术语和数据分析技能进行战略性复习。本提纲为你系统梳理了从化学计量学到有机化学等期末必考的关键主题，并附上重要的考试技巧。你可以把它当作一份自查清单，找出需要深入学习的薄弱环节，同时巩固对贯穿 IB 文凭课程化学部分之互联原理的理解。
1. Stoichiometric Relationships | 化学计量关系
the molar mass (M) is numerically equal to the relative atomic or formula mass expressed in g mol⁻¹. Always convert masses and volumes into moles before solving proportion problems.
摩尔概念是化学计量的核心。任何物质一摩尔都精确含有 6.02214076 × 10²³ 个基本单元，摩尔质量 (M) 在数值上等于相对原子质量或式量，单位为 g mol⁻¹。解决比例问题前，务必先把质量和体积都换算为物质的量。
n = m / M n = V / 22.4 dm³ (at STP) c = n / V
ntify the smallest value. Percentage yield compares experimental mass to theoretical mass: % yield = (actual yield / theoretical yield) × 100%.
限量反应物决定了产物理论产量的最大值。计算各反应物的物质的量，除以其化学计量比系数，找出最小比值。产率用实验质量与理论质量相比：产率 = (实际产量 / 理论产量) × 100%。
| Empirical formula gives the simplest whole-number ratio of atoms; molecular formula is a multiple of that ratio found using the molar mass. | 实验式 给出最简原子整数比；分子式 是借助摩尔质量求出的该比例的整数倍。 |
2. Atomic Structure | 原子结构
eighted average of the masses of naturally occurring isotopes on the scale where ¹²C = 12.
原子由含质子 (Z) 和中子的原子核以及绕核运动的电子构成。同位素质子数相同但中子数不同，因而质量数 (A) 不同。相对原子质量是天然存在同位素质量的加权平均值，以 ¹²C = 12 为基准。
The electron configuration is written using the Aufbau principle: 1s, 2s, 2p, 3s, 3p, 4s, 3d, 4p... For HL, you must understand that s, p, d orbitals have distinct shapes and that chromium and copper display exceptional configurations ([Ar] 4s¹ 3d⁵ and [Ar] 4s¹ 3d¹⁰) due to half-filled and fully filled d sub-shell stability.
电子排布式按构造原理书写：1s, 2s, 2p, 3s, 3p, 4s, 3d, 4p……HL 考生需理解 s、p、d 轨道形状不同，并且铬和铜因半满和全满 d 亚层的稳定性而呈现特殊的排布式 ([Ar] 4s¹ 3d⁵ 和 [Ar] 4s¹ 3d¹⁰)。
Ionization energy trends are fundamental: the first ionization energy generally increases across a period (increased nuclear charge, similar shielding) and decreases down a group (increased distance and shielding). Sharp drops in successive ionization energies of an element provide evidence for electron shells.
电离能变化趋势十分关键：第一电离能通常在同周期中从左到右递增（核电荷增加，屏蔽效应相近），沿同族从上到下递减（距离增大，屏蔽增加）。元素逐级电离能的陡然跌落为电子层结构提供了证据。
3. Periodicity | 周期性
The Periodic Table arranges elements by increasing atomic number, grouping those with similar outer electron configurations. Core trends you must explain for Period 3 are atomic radius (decreases across), ionic radius, first ionization energy (general increase with dips at Al and S), electronegativity, and electron affinity.
元素周期表按原子序数递增排列，将外层电子构型相似的元素归为一族。你必须能够解释第三周期的核心变化趋势：原子半径（跨周期递减）、离子半径、第一电离能（总体上升，在铝和硫处降低）、电负性及电子亲和能。
Period 3 oxides illustrate the change from metallic to non-metallic character. Na₂O and MgO are basic, Al₂O₃ is amphoteric, and SiO₂, P₄O₁₀ and SO₂ are acidic. The trend in bonding also shifts from giant ionic, to giant covalent, to simple molecular structures. Be prepared to write balanced equations for their reactions with water and with acids or bases.
第三周期氧化物体现了从金属性到非金属性的变化：Na₂O 和 MgO 呈碱性，Al₂O₃ 为两性，SiO₂、P₄O₁₀ 和 SO₂ 呈酸性。成键类型也从巨型离子、巨型共价变为简单分子结构。要准备好书写它们与水、酸或碱反应的配平方程式。
- Melting point trend: Increases from Na to Si (giant structures with strong bonding), then drops sharply at P₄, S₈, Cl₂ (weak intermolecular forces).
- 熔点变化趋势：从钠到硅升高（巨型结构，强键能），到白磷、硫、氯气急剧下降（分子间作用力弱）。
4. Chemical Bonding and Structure | 化学键与结构
Ionic bonding results from electrostatic attraction between oppositely charged ions, typically formed when a metal with low ionization energy reacts with a non-metal of high electron affinity. Lattice enthalpy is the energy released when gaseous ions form one mole of solid ionic compound and is a measure of lattice strength.
离子键是带相反电荷离子之间的静电引力，通常由电离能低的金属与电子亲和能高的非金属反应而成。晶格能是气态离子形成一摩尔离子固体时释放的能量，是衡量晶格稳定性的标尺。
with 0 lone pairs → tetrahedral (109.5°), 4 pairs with 1 lone pair → trigonal pyramidal (~107°), 4 pairs with 2 lone pairs → bent (104.5°).
共价键涉及电子对的共用。用 VSEPR 理论根据中心原子周围的成键和非键电子对数来预测分子形状：2对 → 直线形 (180°)，3对 → 平面三角形 (120°)，4对且 0 个孤电子对 → 四面体形 (109.5°)，4对且有 1 个孤电子对 → 三角锥形 (~107°)，4对且有 2 个孤电子对 → V 形 (104.5°)。
Polarity of a bond arises from electronegativity difference; a molecule is polar if the vector sum of bond dipoles is non-zero. Intermolecular forces, in order of increasing strength, are London (dispersion) forces < dipole-dipole forces < hydrogen bonding. For HL, you must also understand sigma (σ) and pi (π) bonds, hybridization (sp, sp², sp³), and delocalization in benzene.
键的极性源于电负性差；若键偶极矢量和不为零，分子便具有极性。分子间作用力按强度递增依次为伦敦色散力 < 偶极-偶极力 < 氢键。HL 考生还需理解 σ 和 π 键、杂化轨道 (sp、sp²、sp³) 以及苯中的离域大 π 键。
5. Energetics / Thermochemistry | 热化学
e m is mass of the solution (usually water), c is specific heat capacity (4.18 J g⁻¹ K⁻¹).
标准焓变 ΔH° 在标准条件 (100 kPa、298 K，溶液浓度 1 mol dm⁻³) 下测定。放热反应 ΔH 为负（向环境释放能量）；吸热反应 ΔH 为正。用量热法按 q = mcΔT 计算热量变化，其中 m 为溶液（通常为水）的质量，c 为比热容 (4.18 J g⁻¹ K⁻¹)。
Hess's Law states that the total enthalpy change for a reaction is independent of the path taken. It is applied through energy cycles, using standard enthalpies of formation (ΔHf°) or combustion (ΔHc°). Be able to construct and manipulate these cycles to find an unknown ΔH.
盖斯定律指出，反应的总焓变与途径无关。通过能量循环，利用标准生成焓 (ΔHf°) 或标准燃烧焓 (ΔHc°) 进行计算。必须能构建并处理这类循环来求解未知焓变。
ΔH_reaction = Σ ΔHf°(products) – Σ ΔHf°(reactants)
ber cycles for ionic solids, calculate entropy changes (ΔS°), Gibbs free energy (ΔG° = ΔH° – TΔS°), and relate ΔG° to equilibrium constant K.
键焓是平均值；断键吸热，成键放热。HL 考生还需运用玻恩-哈伯循环计算离子固体的能量变化，计算熵变 (ΔS°)、吉布斯自由能 (ΔG° = ΔH° – TΔS°)，并联系 ΔG° 与平衡常数 K。
6. Chemical Kinetics | 化学动力学
The rate of a reaction is defined as the change in concentration of a reactant or product per unit time. Rates are determined experimentally by monitoring gradients on concentration–time graphs or by measuring the time taken for a visible change (e.g., formation of a precipitate).
反应速率定义为单位时间内反应物或产物浓度的变化。通过监测浓度–时间图的斜率，或记录可见变化（如沉淀生成）所需的时间，可实验测定反应速率。
action of particles with E ≥ Eₐ, dramatically increasing rate. Catalysts lower Eₐ by providing an alternative pathway.
碰撞理论认为，粒子必须发生能量充足 (E ≥ 活化能 Eₐ) 且取向正确的碰撞，反应才能发生。麦克斯韦-玻尔兹曼分布曲线展示粒子动能分布；升高温度使 E ≥ Eₐ 的粒子比例增大，速率显著增加。催化剂通过提供替代路径降低 Eₐ。
For HL, the rate equation is rate = k[A]m[B]n mentally, not from stoichiometry. The overall order is m+n. The Arrhenius equation (k = Ae–Eₐ/RT) quantifies the temperature dependence of the rate constant k.
HL 内容：速率方程为 rate = k[A]m[B]n，其中 m 和 n 分别为反应级数，由实验确定而非化学计量比，总级数为 m+n。阿伦尼乌斯公式 (k = Ae–Eₐ/RT) 定量描述了速率常数 k 与温度的关系。
7. Equilibrium | 化学平衡
Many reactions are reversible and reach a state of dynamic equilibrium in a closed system when the rates of the forward and reverse reactions are equal. Macroscopic properties (concentration, color, pressure) remain constant, but microscopically, particles continue to react. The equilibrium constant Kc for the generic reaction aA + bB ⇌ cC + dD is:
许多反应在封闭体系中可逆进行并达到动态平衡，此时正逆反应速率相等。宏观性质（浓度、颜色、压强）恒定，但微观上粒子持续反应。对于通式 aA + bB ⇌ cC + dD，平衡常数 Kc 表达式为：
Kc = [C]c [D]d / [A]a [B]b
Kc is temperature dependent only. Le Châtelier's principle allows qualitative predictions: if a stress (change in concentration, pressure, or temperature) is applied to a system at equilibrium, the equilibrium shifts to partially oppose the change. For endothermic reactions, increasing temperature increases Kc; for exothermic, it decreases. Adding a catalyst has no effect on Kc or equilibrium position; it only speeds up attainment of equilibrium.
Kc 仅取决于温度。勒夏特列原理用于定性判断：若对平衡体系施加扰动（浓度、压强或温度变化），平衡将向减弱该变化的方向移动。吸热反应升温使 Kc 增大；放热反应升温则使 Kc 减小。加入催化剂不影响 Kc 或平衡位置，只加速到达平衡。
HL students must also handle Kp for gaseous systems, expressed in partial pressures, and link ΔG° to K via ΔG° = –RT ln K. Heterogeneous equilibria exclude solids and liquids from the expression.
HL 考生还需处理气相体系平衡常数 Kp（用分压表示），并用 ΔG° = –RT ln K 关联自由能与平衡常数。多相平衡表达式中不含纯固体和纯液体。
8. Acids and Bases | 酸与碱
According to Brø water, while a weak acid (e.g., CH₃COOH) only partially dissociates. The pH is defined as – monoprotic strong acid, [H⁺] = initial acid concentration; for weak acids, use Kₐ or pKₐ.
根据布朗斯特-劳里理论，酸是质子给予体，碱是质子接受体。强酸（如 HCl）在水中完全解离，弱酸（如 CH₃COOH）仅部分解离。pH 定义为 –log[H⁺]，其中 [H⁺] 单位为 mol dm⁻³。一元强酸的 [H⁺] 等于初始酸浓度；弱酸则需运用 Kₐ 或 pKₐ。
pH = –log[H⁺] pOH = –log[OH⁻] pH + pOH = 14 at 298 K
the weak acid. Indicators change color over a pH range approximately equal to pK_ind ± 1.
缓冲溶液能抵抗少量外加酸碱引起的 pH 变化，通常由弱酸及其共轭碱组成。滴定曲线可展示等当点与缓冲区；半等当点对应的 pH 即为弱酸的 pKₐ。指示剂变色范围约为 pK_ind ± 1。
HL topics include more rigorous calculations for weak acid/base equilibrium (using Kₐ, Kb, and Kw), salt hydrolysis, and Lewis acid-base theory where acids are electron-pair acceptors and bases are electron-pair donors.
HL 专题涵盖弱酸弱碱平衡的严格计算（利用 Kₐ、Kb、Kw）、盐类水解以及路易斯酸碱理论（酸为电子对接受体，碱为电子对给予体）。
9. Redox Processes | 氧化还原过程
sign oxidation numbers using rules: free elements = 0, hydrogen usually +1, oxygen usually –2, and the sum equals overall charge. Half-equations show electron transfer explicitly.
氧化为失去电子（氧化数升高），还原为得到电子（氧化数降低）。按规则分配氧化数：游离态元素为 0，氢通常 +1，氧通常 –2，总和等于所带电荷。半反应式明确显示电子转移。
A voltaic (galvanic) cell converts chemical energy into electrical energy through spontaneous redox reactions, while an electrolytic cell uses external electrical energy to drive non-spontaneous reactions. In a voltaic cell, oxidation occurs at the anode (negative pole) and reduction at the cathode (positive pole).
伏打（原）电池通过自发的氧化还原反应将化学能转化为电能，而电解池利用外部电能驱动非自发反应。在原电池中，氧化发生在阳极（负极），还原发生在阴极（正极）。
HL, standard electrode potentials (E°) allow calculation of cell EMF: E°_cell = E°_cathode – E°_anode. A positive E°_cell indicates spontaneity (ΔG° < 0). The Nernst equation (E = E° – tions requires comparing electrode potentials of water and the solute to predict products.
HL 内容：标准电极电势 (E°) 可用于计算电池电动势 E°_cell = E°_正极 – E°_负极。E°_cell 为正表明反应自发 (ΔG° < 0)。能斯特方程 (E = E° – (RT/nF) ln Q) 修正非标态影响。电解水溶液时需比较水与溶质的电极电势以预测产物。
10. Organic Chemistry | 有机化学
Organic chemistry is the study of carbon compounds. Homologous series are families of compounds with the same general formula, functional group, and gradual variation in physical properties. Master IUPAC nomenclature: identify the longest carbon chain, locate the principal functional group for lowest numbering, and name substituents alphabetically.
有机化学研究碳化合物。同系物是具有相同通式、相同官能团且物理性质渐变的化合物家族。要掌握 IUPAC 命名法：找出最长碳链，让主官能团位次最低，取代基按字母顺序排列。
| Alkane (CₙH₂ₙ₊₂): free-radical substitution with Cl₂/UV | 烷烃 (CₙH₂ₙ₊₂)：与 Cl₂/紫外线发生自由基取代 |
| Alkene (CₙH₂ₙ): electrophilic addition (Br₂, HBr, H₂O/H⁺); test with bromine water | 烯烃 (CₙH₂ₙ)：亲电加成 (Br₂, HBr, H₂O/H⁺)；用溴水检验 |
| Alcohol (VI); primary → aldehyde → carboxylic acid; secondary → ketone; tertiary resists oxidation | 醇 (CₙH₂ₙ₊₁OH)：用酸化重铬酸钾氧化；伯醇→醛→羧酸；仲醇→酮；叔醇不氧化 |
| Halogenoalkane (R–X): nucleophilic substitution (SN1/SN2 for HL) with OH⁻, NH₃ | 卤代烷 (R–X)：与 OH⁻、NH₃ 发生亲核取代 (HL 涉及 SN1/SN2) |
Structural isomerism (chain, position, functional group) and stereoisomerism (cis-trans or E/Z, optical isomerism for HL) are key. HL students must draw and interpret reaction mechanisms using curly arrows, including electrophilic addition, nucleophilic substitution, and elimination.
结构异构（碳链、位置、官能团异构）和立体异构（顺反或 E/Z 异构，HL 含光学异构）是重点。HL 考生必须能用卷曲箭头画出并解释反应历程，包括亲电加成、亲核取代和消除反应。
11. Measurement and Data Processing | 测量与数据处理
ing instrument, and percentage uncertainty = (absolute uncertainty / measured value) × 100% ting, add absolute uncertainties; when multiplying/dividing, add percentage uncertainties.
任何测量都带有不确定度。绝对不确定度通常取仪器最小分度值的一半，相对不确定度 = (绝对不确定度 / 测量值) × 100%。通过测量值计算最终结果时，需正确传递不确定度：加减运算传递绝对不确定度，乘除运算传递相对不确定度。
Significant figures reflect the precision of data. In calculations, answer is rounded to the least number of significant figures among the data used. For titrations and other quantitative work, always record data to the correct number of decimal places reflecting the instrument precision.
有效数字体现了数据的精密度。在计算中，结果应修约至所用数据中最少的有效数字位数。滴定等定量实验中，务必按仪器精度将数据记录为正确的小数位数。
scopy identifies functional groups from characteristic absorption bands (e.g., C=O stretch ~1700 cm⁻¹, O–H broad ~ tes need to interpret ¹H NMR spectra (chemical shift, integration, splitting) and ¹³C NMR.
图表分析要求画出最佳拟合线，用斜率和截距求出物理量。波谱技术威力强大：红外光谱 (IR) 通过特征吸收峰识别官能团（如 C=O 伸缩约 1700 cm⁻¹，O–H 宽峰 3200-3600 cm⁻¹）；质谱给出分子离子峰和碎片模式。HL 考生需解析 ¹H 核磁共振谱（化学位移、积分、裂分）和 ¹³C NMR。
12. Exam Techniques and Common Pitfalls | 考试技巧与常见误区
Command terms in IB Chemistry are precise: "State" requires a brief answer without explanation; "Describe" asks for an account of characteristics; "Explain" demands reasons linking cause and effect, often using a scientific principle; "Deduce" means reach a conclusion from evidence. Always read the question carefully and match your answer to the command term.
IB 化学命令术语十分精准：“State” 只需简短回答，无需解释；“Describe” 要求描述特征；“Explain” 必须给出因果联系，通常运用科学原理；“Deduce” 要求根据证据推断结论。务必仔细审题，紧扣命令术语作答。
Manage your time: allocate roughly 1.3 minutes per mark. Do not spend too long on a single mark; if stuck, move on and return later. Always show working for calculations—partial credit is often awarded. For extended response questions, structure your answer logically; for 'Explain' questions, use the PEEL approach: Point, Evidence/principle, Explanation, Link back to the context.
管理时间：大致每分用时 1.3 分钟。不要在单个分值上耗费过久；遇到卡壳先跳过，稍后再回看。计算题务必展示过程——常有步骤分。对于长答题，组织要富有逻辑；回答“Explain”类题目可采用 PEEL 法：观点、证据/原理、阐释、回扣情境。
Common pitfalls include: forgetting state symbols in equations, confusing intermolecular forces with covalent bonds, misapplying Le Châtelier's principle to changes in solids, using atomic mass instead of molar mass units, and failing to check that oxidation number changes balance correctly in redox equations. In organic chemistry, missing hidden hydrogens or drawing incorrect bond angles are frequent errors.
常见误区有：方程式中遗漏物态符号、混淆分子间作用力与共价键、错将勒夏特列原理用于固体变化、以原子质量单位代替摩尔质量、在氧化还原方程中未核对氧化数变化是否配平。有机化学中，漏掉隐藏氢原子或画出错误键角也是高频错误。
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